chem 106 - empirical kinetics
If the rate law for the reaction of R and P is Rate = k then which of the following could be a unit for the rate constant (k)?
mol L-1 min-1
If the rate law for the reaction of R and P is Rate = k [P]2 then which of the following could be a unit for the rate constant (k)?
L mol-1 s-1
If the rate law for the reaction of R and P is Rate = k [R] [P] then which of the following could be a unit for the rate constant (k)?
L mol-1 s-1
If the rate law for the reaction of R and P is Rate = k [R]2 then which of the following could be a unit for the rate constant (k)?
L mol-1 s-1
The initial rates for a reaction A and B were studied using the following initial concentrations in mol/L. Expt 1. [A]=0.100, [B]=0.500, rate=1.05x10-4 M/s Expt 2. [A]=0.301, [B]=0.500, rate=1.05x10-4 M/s Expt 3. [A]=0.301, [B]=0.982, rate=2.06x10-4 M/s What is the value of the rate constant?
0.000210 s-1
The initial rates for a reaction A and B were studied using the following initial concentrations in mol/L. Expt 1. [A]=0.300, [B]=0.200, rate=7.17x10-5 M/s Expt 2. [A]=0.664, [B]=0.200, rate=7.17x10-5 M/s Expt 3. [A]=0.664, [B]=0.221, rate=7.92x10-5 M/s What is the value of the rate constant?
0.000358 s-1
The initial rates for a reaction A and B were studied using the following initial concentrations in mol/L. Expt 1. [A]=0.200, [B]=0.400, rate=1.72x10-4 M/s Expt 2. [A]=0.647, [B]=0.400, rate=1.72x10-4 M/s Expt 3. [A]=0.647, [B]=0.411, rate=1.82x10-4 M/s What is the value of the rate constant?
0.00108 M-1 s-1
If the rate law for the reaction of R and P is Rate = k [P] then which of the following could be a unit for the rate constant (k)?
yr-1
The initial rates for a reaction A and B were studied using the following initial concentrations in mol/L. Expt 1. [A]=0.300, [B]=0.500, rate=1.10x10-3 M/s Expt 2. [A]=0.219, [B]=0.500, rate=1.10x10-3 M/s Expt 3. [A]=0.219, [B]=1.53, rate=3.37x10-3 M/s What is the value of the rate constant?
0.00220 s-1
The initial rates for a reaction A and B were studied using the following initial concentrations in mol/L. Expt 1. [A]=0.100, [B]=0.400, rate=1.61x10-3 M/s Expt 2. [A]=0.152, [B]=0.400, rate=1.61x10-3 M/s Expt 3. [A]=0.152, [B]=1.57, rate=6.32x10-3 M/s What is the value of the rate constant?
0.00402 s-1
The initial rates for a reaction A and B were studied using the following initial concentrations in mol/L. Expt 1. [A]=0.200, [B]=0.400, rate=1.72x10-4 M/s Expt 2. [A]=0.647, [B]=0.400, rate=1.72x10-4 M/s Expt 3. [A]=0.647, [B]=0.411, rate=1.77x10-4 M/s What is the value of the rate constant?
0.00430 s-1
The initial rates for a reaction A and B were studied using the following initial concentrations in mol/L. Expt 1. [A]=0.200, [B]=0.100, rate=6.72x10-4 M/s Expt 2. [A]=0.100, [B]=0.100, rate=6.72x10-4 M/s Expt 3. [A]=0.100, [B]=0.400, rate=2.69x10-3 M/s What is the value of the rate constant?
0.00672 s-1
The initial rates for a reaction A and B were studied using the following initial concentrations in mol/L. Expt 1. [A]=0.100, [B]=0.400, rate=1.61x10-3 M/s Expt 2. [A]=0.152, [B]=0.400, rate=2.45x10-3 M/s Expt 3. [A]=0.152, [B]=1.57, rate=9.62x10-3 M/s What is the value of the rate constant?
0.0402 M-1 s-1
Suppose the rate law for a reaction is rate = k[X]3[Y]1 and the rate of the reaction is 0.842 M/min when [X] = 0.344 M. All other factors being equal, if [X] = 0.172 M, the rate of the reaction would be
0.105 M/min
The initial rates for a reaction A and B were studied using the following initial concentrations in mol/L. Expt 1. [A]=0.200, [B]=0.200, rate=4.29x10-3 M/s Expt 2. [A]=0.397, [B]=0.200, rate=8.52x10-3 M/s Expt 3. [A]=0.397, [B]=0.409, rate=1.74x10-2 M/s What is the value of the rate constant?
0.107 M-1 s-1
Suppose the rate law for a reaction is rate = k[X]2[Y]3 and the rate of the reaction is 0.774 M/min when [X] = 0.324 M. All other factors being equal, if [X] = 0.162 M, the rate of the reaction would be
0.194 M/min
Suppose the rate law for a reaction is rate = k[X]2[Y]2 and the rate of the reaction is 0.821 M/min when [X] = 0.299 M. All other factors being equal, if [X] = 0.150 M, the rate of the reaction would be
0.205 M/min
The initial rates for a reaction A and B were studied using the following initial concentrations in mol/L. Expt 1. [A]=0.400, [B]=0.100, rate=3.86x10-3 M/s Expt 2. [A]=1.02, [B]=0.100, rate=3.86x10-3 M/s Expt 3. [A]=1.02, [B]=0.384, rate=5.69x10-2 M/s What is the value of the rate constant?
0.386 M-1 s-1
Suppose the rate law for a reaction is rate = k[X]1[Y]2 and the rate of the reaction is 0.778 M/min when [X] = 0.312 M. All other factors being equal, if [X] = 0.156 M, the rate of the reaction would be
0.389 M/min
Suppose the rate law for a reaction is rate = k[X]1[Y]2 and the rate of the reaction is 0.804 M/min when [X] = 0.346 M. All other factors being equal, if [X] = 0.173 M, the rate of the reaction would be
0.402 M/min
Suppose the rate law for a reaction is rate = k[X]1[Y]2 and the rate of the reaction is 0.894 M/min when [X] = 0.399 M. All other factors being equal, if [X] = 0.205 M, the rate of the reaction would be
0.459 M/min
Suppose the rate law for a reaction is rate = k[X]1[Y]1 and the rate of the reaction is 0.823 M/min when [X] = 0.292 M. All other factors being equal, if [X] = 0.254 M, the rate of the reaction would be
0.715 M/m
The initial rates for a reaction A and B were studied using the following initial concentrations in mol/L. Expt 1. [A]=0.100, [B]=0.300, rate=1.42x10-4 M/s Expt 2. [A]=0.0844, [B]=0.300, rate=1.42x10-4 M/s Expt 3. [A]=0.211, [B]=0.778, rate=3.68x10-4 M/s What is the order of reaction with respect to B?
1
The initial rates for a reaction A and B were studied using the following initial concentrations in mol/L. Expt 1. [A]=0.100, [B]=0.400, rate=1.61x10-3 M/s Expt 2. [A]=0.152, [B]=0.400, rate=2.45x10-3 M/s Expt 3. [A]=0.152, [B]=1.57, rate=9.62x10-3 M/s What is the order of reaction with respect to B?
1
The initial rates for a reaction A and B were studied using the following initial concentrations in mol/L. Expt 1. [A]=0.200, [B]=0.200, rate=4.29x10-3 M/s Expt 2. [A]=0.397, [B]=0.200, rate=8.52x10-3 M/s Expt 3. [A]=0.397, [B]=0.409, rate=1.74x10-2 M/s What is the order of reaction with respect to B?
1
The initial rates for a reaction A and B were studied using the following initial concentrations in mol/L. Expt 1. [A]=0.300, [B]=0.400, rate=2.80x10-4 M/s Expt 2. [A]=1.04, [B]=0.400, rate=2.80x10-4 M/s Expt 3. [A]=0.695, [B]=1.63, rate=1.14x10-3 M/s What is the order of reaction with respect to B?
1
Consider the reaction 2 A(aq) + 3 B(aq) → C(aq) If the rate of consumption of A is 7.39x10-3 mol L-1 min-1, what is the rate of production of C?
3.70x10-3 mol L-1 min-1
The initial rates for a reaction A and B were studied using the following initial concentrations in mol/L. Expt 1. [A]=0.300, [B]=0.400, rate=2.80x10-4 M/s Expt 2. [A]=1.04, [B]=0.400, rate=9.71x10-4 M/s Expt 3. [A]=1.04, [B]=1.63, rate=3.96x10-3 M/s What is the order of reaction with respect to B?
1
The initial rates for a reaction A and B were studied using the following initial concentrations in mol/L. Expt 1. [A]=0.300, [B]=0.500, rate=1.10x10-3 M/s Expt 2. [A]=0.219, [B]=0.500, rate=8.03x10-4 M/s Expt 3. [A]=0.219, [B]=1.53, rate=2.46x10-3 M/s What is the order of reaction with respect to B?
1
What is the rate of consumption of reactant A if its concentration decreases from 5.70x10-3 mol/L to 3.40x10-3 mol/L in 228.9 seconds.
1.00x10-5 M/s
What is the rate of consumption of reactant A if its concentration decreases from 7.59x10-3 mol/L to 2.52x10-3 mol/L in 456.7 seconds.
1.11x10-5 M/s
The rate law for a reaction is: rate = 6.98x10-6 M s-1. If the initial concentration of R is 1.27x10-2 M, calculate its concentration at 134 s.
1.18x10-2 M
Consider the reaction 3 A(aq) + B(aq) → 2 C(aq) If the rate of consumption of A is 1.91x10-4 M s-1, what is the rate of production of C?
1.27x10-4 M s-1
The rate law for a reaction is: rate = 2.07x10-5 M s-1. If the initial concentration of R is 1.69x10-2 M, calculate its concentration at 98.8 s.
1.48x10-2 M
The initial rates for a reaction A and B were studied using the following initial concentrations in mol/L. Expt 1. [A]=0.100, [B]=0.400, rate=1.61x10-3 M/s Expt 2. [A]=0.152, [B]=0.400, rate=2.45x10-3 M/s Expt 3. [A]=0.152, [B]=1.57, rate=2.45x10-3 M/s What is the value of the rate constant?
1.61x10-2 s-1
Consider the reaction 2 A(aq) + 3 B(aq) → C(aq) If the rate of consumption of A is 3.85x10-3 mol L-1 min-1, what is the rate of production of C?
1.92x10-3 mol L-1 min-1
What is the rate of production of product X if its concentration increases from 2.14x10-3 mol/L to 3.83x10-3 mol/L in 514.3 seconds.
1.97x10-4 M/min
The rate law for a reaction involving reactant Q was determined to be: rate = k[A] over a range of temperatures. A plot of ln(k) vs. 1/T from 25oC to 100oC and the energy of activation was found from the slope to be 47.8 kJ/mol. If the half life at 32.3oC is found to be 808 s, calculate the half life at 68.7oC.
109 s
The initial rates for a reaction A and B were studied using the following initial concentrations in mol/L. Expt 1. [A]=0.100, [B]=0.500, rate=1.05x10-4 M/s Expt 2. [A]=0.301, [B]=0.500, rate=1.05x10-4 M/s Expt 3. [A]=0.781, [B]=0.982, rate=4.05x10-4 M/s What is the order of reaction with respect to B?
2
The initial rates for a reaction A and B were studied using the following initial concentrations in mol/L. Expt 1. [A]=0.100, [B]=0.500, rate=1.05x10-4 M/s Expt 2. [A]=0.301, [B]=0.500, rate=9.51x10-4 M/s Expt 3. [A]=0.301, [B]=0.982, rate=1.87x10-3 M/s What is the order of reaction with respect to A?
2
The initial rates for a reaction A and B were studied using the following initial concentrations in mol/L. Expt 1. [A]=0.200, [B]=0.400, rate=1.72x10-4 M/s Expt 2. [A]=0.647, [B]=0.400, rate=5.56x10-4 M/s Expt 3. [A]=0.647, [B]=0.411, rate=5.87x10-4 M/s What is the order of reaction with respect to B?
2
The initial rates for a reaction A and B were studied using the following initial concentrations in mol/L. Expt 1. [A]=0.300, [B]=0.500, rate=1.10x10-3 M/s Expt 2. [A]=0.219, [B]=0.500, rate=5.86x10-4 M/s Expt 3. [A]=0.219, [B]=1.53, rate=1.79x10-3 M/s What is the order of reaction with respect to A?
2
The initial rates for a reaction A and B were studied using the following initial concentrations in mol/L. Expt 1. [A]=0.300, [B]=0.500, rate=1.10x10-3 M/s Expt 2. [A]=0.219, [B]=0.500, rate=8.03x10-4 M/s Expt 3. [A]=0.219, [B]=1.53, rate=7.52x10-3 M/s What is the order of reaction with respect to B?
2
Consider the reaction 3 A(aq) + B(aq) → 2 C(aq) If the rate of consumption of A is 3.85x10-3 M s-1, what is the rate of production of C?
2.56x10-3 M s-1
The rate law for a reaction is: rate = 7.35x10-6 M s-1. If the initial concentration of R is 3.00x10-3 M, calculate its concentration at 57.9 s.
2.57x10-3 M
Consider the reaction 2 A(aq) + 3 B(aq) → C(aq) If the rate of consumption of A is 5.16x10-5 mol L-1 min-1, what is the rate of production of C?
2.58x10-5 mol L-1 min-1
What is the rate of production of product X if its concentration increases from 2.58x10-3 mol/L to 4.95x10-3 mol/L in 543.1 seconds.
2.62x10-4 M/min
The rate law for a reaction is: rate = (3.33x10-3 s-1) [R]. If the initial concentration of R is 2.99x10-2 M, calculate its concentration at 27.0 s.
2.73x10-2 M
Consider the reaction 3 A(aq) + B(aq) → 2 C(aq) If the rate of production of C is 1.91x10-4 M s-1, what is the rate of consumption of A?
2.86x10-4 M s-1
Suppose the rate law for a reaction is rate = k[X]1[Y]2 and the rate of the reaction is 0.785 M/min when [X] = 0.643 M. All other factors being equal, if [X] = 2.36 M, the rate of the reaction would be
2.88 M/min
The rate law for a reaction is: rate = (7.62x10-4 s-1)[R]. If the initial concentration of R is 1.27x10-2 M, calculate the time it takes for the concentration to drop to 1.87x10-3 M.
2510 s
The concentration of reactant A was monitored over time and the following data were obtained: t=0, [A]=5.29x10-2 M t=807 s, [A]=2.64x10-2 M t=1210 s, [A]=1.32x10-2 M Which of the following rate laws is consistent with the data?
3.28x10-5 M s-1
Consider the reaction 2 A(aq) + 3 B(aq) → C(aq) If the rate of consumption of A is 6.91x10-4 mol L-1 min-1, what is the rate of production of C?
3.46x10-4 mol L-1 min-1
Consider the reaction 2 A(aq) + 3 B(aq) → C(aq) If the rate of consumption of B is 1.06x10-3 mol L-1 min-1, what is the rate of production of C?
3.53x10-4 mol L-1 min-1
The rate law for a reaction involving reactant Q was determined to be: rate = k[A] over a range of temperatures. A plot of ln(k) vs. 1/T from 25oC to 100oC and the energy of activation was found from the slope to be 54.0 kJ/mol. If the half life at 26.6oC is found to be 891 s, calculate the half life at 79.7oC.
34.2 s
What is the rate of consumption of reactant A if its concentration decreases from 4.95x10-3 mol/L to 2.58x10-3 mol/L in 543.1 seconds.
4.36x10-6 M/s
What is the rate of consumption of reactant A if its concentration decreases from 3.08x10-3 mol/L to 1.48x10-3 mol/L in 328.4 seconds.
4.87x10-6 M/s
The rate of the reaction between X and Y was studied by using the method of isolation with the following initial concentrations: Expt 1. [X]=0.500 mol/L, [Y]=5.29x10-5 mol/L Expt 2. [X]=1.50 mol/L, [Y]=5.29x10-5 mol/L The following apparent rate constants were obtained: Expt 1. kapp = 2.77x10-3 s-1 Expt 2. kapp = 2.49x10-2 s-1 What is the rate law?
40.2 kJ/mol
The rate constant of a reaction (k) was determined over a range of temperatures. A plot of ln(k) vs. 1/T from 26.0oC to 89.0oC is linear with a slope of -4920 K. What is the energy of activation?
40.9 kJ/mol
The rate law for a reaction involving reactant Q was determined to be: rate = k[A] over a range of temperatures. A plot of ln(k) vs. 1/T from 25oC to 100oC and the energy of activation was found from the slope to be 45.9 kJ/mol. If the half life at 26.9oC is found to be 526 s, calculate the half life at 75.0oC.
41.4 s
The rate constant of a reaction (k) was determined over a range of temperatures. A plot of ln(k) vs. 1/T from 32.0oC to 87.0oC is linear with a slope of -5140 K. What is the energy of activation?
42.7 kJ/mol
The rate constant of a reaction (k) was determined over a range of temperatures. A plot of ln(k) vs. 1/T from 29.0oC to 87.0oC is linear with a slope of -5740 K. What is the energy of activation?
47.7 kJ/mol
What is the rate of production of product X if its concentration increases from 2.39x10-3 mol/L to 6.45x10-3 mol/L in 414.8 seconds.
5.87x10-4 M/min
The rate constant of a reaction (k) was determined over a range of temperatures. A plot of ln(k) vs. 1/T from 30.0oC to 83.0oC is linear with a slope of -6190 K. What is the energy of activation?
51.5 kJ/mol
What is the rate of production of product X if its concentration increases from 3.40x10-3 mol/L to 5.70x10-3 mol/L in 228.9 seconds.
6.03x10-4 M/min
What is the rate of production of product X if its concentration increases from 2.52x10-3 mol/L to 7.59x10-3 mol/L in 456.7 seconds.
6.66x10-4 M/min
The rate law for a reaction is: rate = (2.24x10-3 s-1)[R]. If the initial concentration of R is 7.17x10-3 M, calculate the time it takes for the concentration to drop to 1.86x10-3 M.
602 s
Consider the reaction 3 A(aq) + B(aq) → 2 C(aq) If the rate of consumption of A is 1.06x10-3 M s-1, what is the rate of production of C?
7.06x10-4 M s-1
The rate law for a reaction is: rate = (1.14x10-3 s-1) [R]. If the initial concentration of R is 9.54x10-3 M, calculate its concentration at 215 s.
7.47x10-3 M
Consider the reaction 3 A(aq) + B(aq) → 2 C(aq) If the rate of production of C is 5.16x10-5 M s-1, what is the rate of consumption of A?
7.74x10-5 M s-1
What is the rate of consumption of reactant A if its concentration decreases from 5.33x10-3 mol/L to 2.18x10-3 mol/L in 386.0 seconds.
8.16x10-6 M/s
The rate law for a reaction is: rate = 7.73x10-5 M s-1. If the initial concentration of R is 9.37x10-2 M, calculate its concentration at 125 s.
8.40x10-2 M
The rate law for a reaction is: rate = (1.69x10-3 s-1)[R]. If the initial concentration of R is 1.69x10-2 M, calculate the time it takes for the concentration to drop to 4.08x10-3 M.
841 s
The rate law for a reaction is: rate = (4.50x10-1 M-1 s-1)[R]2. If the initial concentration of R is 7.17x10-3 M, calculate the time it takes for the concentration to drop to 1.86x10-3 M.
885 s
The rate of the reaction between X and Y was studied by using the method of isolation with the following initial concentrations: Expt 1. [X]=0.100 mol/L, [Y]=3.00x10-6 mol/L Expt 2. [X]=0.200 mol/L, [Y]=3.00x10-6 mol/L The following apparent rate constants were obtained: Expt 1. kapp = 2.77x10-3 s-1 Expt 2. kapp = 5.54x10-3 s-1 What is the rate law?
9.47 s
Mixtures of 0.113 M A(aq) and 0.370 M B(aq) were mixed and the initial rates were measured. Expt 1. 1.00 mL A(aq) + 2.00 mL B(aq) + 7.00 mL water Expt 2. 1.00 mL A(aq) + 4.00 mL B(aq) + 7.00 mL water Expt 3. 1.00 mL A(aq) + 4.00 mL B(aq) + 5.00 mL water Which pair of experiments would allow you to determine the order of reaction with respect to B?
Expt 1 and 3
Mixtures of 0.142 M A(aq) and 0.543 M B(aq) were mixed and the initial rates were measured. Expt 1. 2.00 mL A(aq) + 1.50 mL B(aq) + 6.50 mL water Expt 2. 2.00 mL A(aq) + 3.50 mL B(aq) + 6.50 mL water Expt 3. 2.00 mL A(aq) + 3.50 mL B(aq) + 4.50 mL water Which pair of experiments would allow you to determine the order of reaction with respect to B?
Expt 1 and 3
The initial rates for a reaction A and B were studied using the following initial concentrations in mol/L. Expt 1. [A]=0.100, [B]=0.500 Expt 2. [A]=0.301, [B]=0.500 Expt 3. [A]=0.301, [B]=0.982 Which pair of experiments allows us to determine the order of reaction with respect to A?
Expts 1 and 2
The initial rates for a reaction A and B were studied using the following initial concentrations in mol/L. Expt 1. [A]=0.300, [B]=0.200 Expt 2. [A]=0.664, [B]=0.200 Expt 3. [A]=0.664, [B]=0.221 Which pair of experiments allows us to determine the order of reaction with respect to B?
Expts 2 and 3
The initial rates for a reaction A and B were studied using the following initial concentrations in mol/L. Expt 1. [A]=0.300, [B]=0.400 Expt 2. [A]=1.04, [B]=0.400 Expt 3. [A]=1.04, [B]=1.63 Which pair of experiments allows us to determine the order of reaction with respect to B?
Expts 2 and 3
If the rate law for the reaction of R and P is Rate = k [R] [P]2 then which of the following could be a unit for the rate constant (k)?
L2 mol-2 s-1
If the rate law for the reaction of R and P is Rate = k [R]2 [P] then which of the following could be a unit for the rate constant (k)?
L2 mol2- s-1
Mixtures of 0.254 M A(aq) and 0.445 M B(aq) were mixed and the initial rates were measured. Expt 1. 2.50 mL A(aq) + 2.50 mL B(aq) + 5.00 mL water Expt 2. 2.50 mL A(aq) + 4.50 mL B(aq) + 3.00 mL water Expt 3. 2.50 mL A(aq) + 4.50 mL B(aq) + 5.00 mL water Which pair of experiments would allow you to determine the order of reaction with respect to A?
None
The initial rates of a reaction between P and Q were determined in a series of experiments with the following initial concentrations: Expt 1. [P] = 3.63x10-4, [Q] = 2.83x10-4 Expt 2. [P] = 7.26x10-4, [Q] = 2.83x10-4 Expt 3. [P] = 1.82x10-3, [Q] = 2.83x10-4 Expt 4. [P] = 3.63x10-3, [Q] = 2.83x10-4 These experiments will allow us to determine the order of reaction with respect to...
P
The initial rates of a reaction between P and Q were determined in a series of experiments with the following initial concentrations: Expt 1. [P] = 3.80x10-3, [Q] = 8.87x10-6 Expt 2. [P] = 7.60x10-3, [Q] = 8.87x10-6 Expt 3. [P] = 1.90x10-2, [Q] = 8.87x10-6 Expt 4. [P] = 3.80x10-2, [Q] = 8.87x10-6 These experiments will allow us to determine the order of reaction with respect to...
P
The initial rates of a reaction between Q and P were determined in a series of experiments with the following initial concentrations: Expt 1. [Q] = 3.64x10-3, [P] = 8.89x10-4 Expt 2. [Q] = 7.28x10-3, [P] = 8.89x10-4 Expt 3. [Q] = 1.82x10-2, [P] = 8.89x10-4 Expt 4. [Q] = 3.64x10-2, [P] = 8.89x10-4 These experiments will allow us to determine the order of reaction with respect to...
Q
Consider a reaction involving reactant Z where a plot of ln[Z] vs. time can be fitted to a straight line. Two of the points on the best-fit line correspond to: (t=212 s, [Z]=2.06x10-2 M) and (t=372 s, [Z]=1.62x10
Rate = (1.50x10-3 s-1) [Z]
For a reaction involving reactant X, which rate law is consistent with the following observation: [X] = [X]o - kt, where [X]o is the initial concentration and t is time. ?
Rate = k
The rate of the reaction between X and Y was studied by using the method of isolation with the following initial concentrations: Expt 1. [X]=0.300 mol/L, [Y]=8.18x10-5 mol/L Expt 2. [X]=0.600 mol/L, [Y]=8.18x10-5 mol/L The following apparent rate constants were obtained: Expt 1. kapp = 2.77x10-3 s-1 Expt 2. kapp = 1.11x10-2 s-1 What is the rate law?
Rate = k[X]2[Y]
For a reaction involving reactant X, which rate law is consistent with the following observation: If it takes 15.0 s for [X] to drop from 0.20M to 0.10M , it takes 20.0 s to drop from 0.15 to 0.075. ?
Rate=k[X]2
The rate of the reaction between X and Y was studied by using initial concentrations of 1.69x10-5 mol/L for X and 2.00x10-1 mol/L for Y. This type of experiment will allow the determination of the order of reaction with respect to which reactant?
X
The rate of the reaction between X and Y was studied by using initial concentrations of 2.25x10-5 mol/L for X and 4.00x10-1 mol/L for Y. This type of experiment will allow the determination of the order of reaction with respect to which reactant?
X
The rate of the reaction between X and Y was studied by using initial concentrations of 5.29x10-5 mol/L for X and 5.00x10-1 mol/L for Y. This type of experiment will allow the determination of the order of reaction with respect to which reactant?
X
The rate of the reaction between X and Y was studied by using initial concentrations of 9.54x10-6 mol/L for X and 4.00x10-1 mol/L for Y. This type of experiment will allow the determination of the order of reaction with respect to which reactant?
X
The rate of the reaction between X and Y was studied by using initial concentrations of 1.00x10-1 mol/L for X and 3.00x10-6 mol/L for Y. This type of experiment will allow the determination of the order of reaction with respect to which reactant?
Y
The rate of the reaction between X and Y was studied by using initial concentrations of 2.00x10-1 mol/L for X and 1.69x10-5 mol/L for Y. This type of experiment will allow the determination of the order of reaction with respect to which reactant?
Y
The rate of the reaction between X and Y was studied by using initial concentrations of 2.00x10-1 mol/L for X and 7.17x10-6 mol/L for Y. This type of experiment will allow the determination of the order of reaction with respect to which reactant?
Y
The rate of the reaction between X and Y was studied by using initial concentrations of 4.00x10-1 mol/L for X and 2.25x10-5 mol/L for Y. This type of experiment will allow the determination of the order of reaction with respect to which reactant?
Y
The rate of the reaction between X and Y was studied by using initial concentrations of 4.00x10-1 mol/L for X and 9.54x10-6 mol/L for Y. This type of experiment will allow the determination of the order of reaction with respect to which reactant?
Y
The rate of the reaction between X and Y was studied by using initial concentrations of 5.00x10-1 mol/L for X and 1.27x10-5 mol/L for Y. This type of experiment will allow the determination of the order of reaction with respect to which reactant?
Y
Suppose the rate law for a reaction is rate = k[A]1[B]2 All other factors being equal, doubling the concentration of A causes the rate to
double
Mixtures of 0.235 M A(aq) and 0.594 M B(aq) were mixed and the initial rates were measured. Expt 1. 1.00 mL A(aq) + 2.00 mL B(aq) + 7.00 mL water Expt 2. 1.00 mL A(aq) + 3.50 mL B(aq) + 7.00 mL water Expt 3. 1.00 mL A(aq) + 3.50 mL B(aq) + 5.50 mL water Which pair of experiments would allow you to determine the order of reaction with respect to B?
expt 1 and 3
The initial rates for a reaction A and B were studied using the following initial concentrations in mol/L. Expt 1. [A]=0.100, [B]=0.500 Expt 2. [A]=0.301, [B]=0.982 Expt 3. [A]=0.301, [B]=0.500 Which pair of experiments allows us to determine the order of reaction with respect to A?
expts 1 and 3
Suppose the rate law for a reaction is rate = k[A]3[B]2 All other factors being equal, doubling the concentration of A causes the rate to
increase 8-fold
Consider a reaction involving reactant Z where a plot of ln[Z] vs. time can be fitted to a straight line. Two of the points on the best-fit line correspond to: (t=109 s, [Z]=6.76x10-3 M) and (t=348 s, [Z]=4.90x10-3 M) What is the rate law?
rate = (1.35x10-3 s-1) [Z]
The concentration of reactant A was monitored over time and the following data were obtained: t=0, [A]=1.69x10-2 M t=409 s, [A]=8.45x10-3 M t=1230 s, [A]=4.22x10-3 M Which of the following rate laws is consistent with the data?
rate = (1.45x10-1 M-1 s-1) [A]2
The concentration of reactant A was monitored over time and the following data were obtained: t=0, [A]=8.18x10-2 M t=460 s, [A]=4.09x10-2 M t=920 s, [A]=2.04x10-2 M Which of the following rate laws is consistent with the data?
rate = (1.51x10-3 s-1) [A]
The concentration of reactant A was monitored over time and the following data were obtained: t=0, [A]=3.00x10-3 M t=204 s, [A]=1.50x10-3 M t=612 s, [A]=7.50x10-4 M Which of the following rate laws is consistent with the data?
rate = (1.63x100 M-1 s-1) [A]2
Consider a reaction involving reactant Z where a plot of 1/[Z] vs. time can be fitted to a straight line. Two of the points on the best-fit line correspond to: (t=57.9 s, [Z]=2.34x10-3 M) and (t=136 s, [Z]=1.80x10-3 M)
rate = (1.64x100 M-1 s-1) [Z]2
Consider a reaction involving reactant Z where a plot of 1/[Z] vs. time can be fitted to a straight line. Two of the points on the best-fit line correspond to: (t=215 s, [Z]=7.05x10-3 M) and (t=458 s, [Z]=5.45x10-3 M) What is the rate law?
rate = (1.71x10-1 M-1 s-1) [Z]2
Consider a reaction involving reactant Z where a plot of 1/[Z] vs. time can be fitted to a straight line. Two of the points on the best-fit line correspond to: (t=125 s, [Z]=7.77x10-2 M) and (t=360 s, [Z]=5.88x10-2 M) What is the rate law?
rate = (1.76x10-2 M-1 s-1) [Z]2
The concentration of reactant A was monitored over time and the following data were obtained: t=0, [A]=6.36x10-3 M t=742 s, [A]=3.18x10-3 M t=2230 s, [A]=1.59x10-3 M Which of the following rate laws is consistent with the data?
rate = (2.12x10-1 M-1 s-1) [A]2
Consider a reaction involving reactant Z where a plot of ln[Z] vs. time can be fitted to a straight line. Two of the points on the best-fit line correspond to: (t=71.8 s, [Z]=7.00x10-2 M) and (t=204 s, [Z]=5.25x10-2 M) What is the rate law?
rate = (2.18x10-3 s-1) [Z]
Consider a reaction involving reactant Z where a plot of 1/[Z] vs. time can be fitted to a straight line. Two of the points on the best-fit line correspond to: (t=71.8 s, [Z]=7.08x10-2 M) and (t=204 s, [Z]=5.67x10-2 M) What is the rate law?
rate = (2.66x10-2 M-1 s-1) [Z]2
Consider a reaction involving reactant Z where a plot of ln[Z] vs. time can be fitted to a straight line. Two of the points on the best-fit line correspond to: (t=75.6 s, [Z]=3.61x10-3 M) and (t=127 s, [Z]=3.03x10-3 M) What is the rate law?
rate = (3.41x10-3 s-1) [Z]
The concentration of reactant A was monitored over time and the following data were obtained: t=0, [A]=4.78x10-3 M t=517 s, [A]=2.39x10-3 M t=1550 s, [A]=1.20x10-3 M Which of the following rate laws is consistent with the data?
rate = (4.05x10-1 M-1 s-1) [A]2
The concentration of reactant A was monitored over time and the following data were obtained: t=0, [A]=1.27x10-2 M t=909 s, [A]=6.35x10-3 M t=1820 s, [A]=3.18x10-3 M Which of the following rate laws is consistent with the data?
rate = (7.62x10-4 s-1) [A]
The concentration of reactant A was monitored over time and the following data were obtained: t=0, [A]=7.17x10-3 M t=310 s, [A]=3.58x10-3 M t=465 s, [A]=1.79x10-3 M Which of the following rate laws is consistent with the data?
rate = 1.16x10-5 M s-1
Consider a reaction involving reactant Z where a plot of 1/[Z] vs. time can be fitted to a straight line. Two of the points on the best-fit line correspond to: (t=134 s, [Z]=1.18x10-2 M) and (t=427 s, [Z]=9.72x10-3 M) What is the rate law?
rate = 7.10x10-6 M s-1
The concentration of reactant A was monitored over time and the following data were obtained: t=0, [A]=9.54x10-3 M t=610 s, [A]=4.77x10-3 M t=915 s, [A]=2.38x10-3 M Which of the following rate laws is consistent with the data?
rate = 7.82x10-6 M s-1
For a reaction involving reactant X, which rate law is consistent with the following observation: A plot of [X] vs. time is a straight line. ?
rate = k
For a reaction involving reactant X, which rate law is consistent with the following observation: If it takes 40 s for [X] to drop from 0.80 to 0.40M, it takes 20 s it to drop from 0.40M to 0.20 M. ?
rate = k
For a reaction involving reactant X, which rate law is consistent with the following observation: [X] = [X]o - kt, where [X]o is the initial concentration and t is time. ?
rate = k
The rate constant of a reaction (k) was determined over a range of temperatures. A plot of ln(k) vs. 1/T from 28.0oC to 94.0oC is linear with a slope of -4840 K. What is the energy of activation?
rate = k[X]2[Y]
The rate of the reaction between X and Y was studied by using the method of isolation with the following initial concentrations: Expt 1. [X]=0.100 mol/L, [Y]=3.00x10-6 mol/L Expt 2. [X]=0.200 mol/L, [Y]=3.00x10-6 mol/L The following apparent rate constants were obtained: Expt 1. kapp = 2.77x10-3 s-1 Expt 2. kapp = 1.11x10-2 s-1 What is the rate law?
rate = k[X]2[Y]
The rate of the reaction between X and Y was studied by using the method of isolation with the following initial concentrations: Expt 1. [X]=0.200 mol/L, [Y]=7.17x10-6 mol/L Expt 2. [X]=0.400 mol/L, [Y]=7.17x10-6 mol/L The following apparent rate constants were obtained: Expt 1. kapp = 2.77x10-3 s-1 Expt 2. kapp = 1.11x10-2 s-1 What is the rate law?
rate = k[X]2[Y]
The rate of the reaction between X and Y was studied by using the method of isolation with the following initial concentrations: Expt 1. [X]=0.500 mol/L, [Y]=1.27x10-5 mol/L Expt 2. [X]=1.00 mol/L, [Y]=1.27x10-5 mol/L The following apparent rate constants were obtained: Expt 1. kapp = 2.77x10-3 s-1 Expt 2. kapp = 1.11x10-2 s-1 What is the rate law?
rate = k[X]2[Y]
The rate law for a reaction involving reactant Q was determined to be: rate = k[A] over a range of temperatures. A plot of ln(k) vs. 1/T from 25oC to 100oC and the energy of activation was found from the slope to be 50.3 kJ/mol. If the half life at 26.0oC is found to be 321 s, calculate the half life at 89.1oC.
rate = k[X][Y]
The rate of the reaction between X and Y was studied by using the method of isolation with the following initial concentrations: Expt 1. [X]=0.300 mol/L, [Y]=8.18x10-5 mol/L Expt 2. [X]=0.600 mol/L, [Y]=8.18x10-5 mol/L The following apparent rate constants were obtained: Expt 1. kapp = 2.77x10-3 s-1 Expt 2. kapp = 5.54x10-3 s-1 What is the rate law?
rate = k[X][Y]
The rate of the reaction between X and Y was studied by using the method of isolation with the following initial concentrations: Expt 1. [X]=0.400 mol/L, [Y]=9.37x10-5 mol/L Expt 2. [X]=0.800 mol/L, [Y]=9.37x10-5 mol/L The following apparent rate constants were obtained: Expt 1. kapp = 2.77x10-3 s-1 Expt 2. kapp = 5.54x10-3 s-1 What is the rate law?
rate = k[X][Y]
The rate of the reaction between X and Y was studied by using the method of isolation with the following initial concentrations: Expt 1. [X]=0.300 mol/L, [Y]=8.18x10-5 mol/L Expt 2. [X]=0.600 mol/L, [Y]=8.18x10-5 mol/L The following apparent rate constants were obtained: Expt 1. kapp = 4.89x101 L mol-1 s-1 Expt 2. kapp = 9.78x101 L mol-1 s-1 What is the rate law?
rate = k[X][Y]2
The rate of the reaction between X and Y was studied by using the method of isolation with the following initial concentrations: Expt 1. [X]=0.400 mol/L, [Y]=2.25x10-5 mol/L Expt 2. [X]=1.20 mol/L, [Y]=2.25x10-5 mol/L The following apparent rate constants were obtained: Expt 1. kapp = 1.78x102 L mol-1 s-1 Expt 2. kapp = 5.34x102 L mol-1 s-1 What is the rate law?
rate = k[X][Y]2
The concentration of reactant A was monitored over time and the following data were obtained: t=0, [A]=5.16x10-2 M t=405 s, [A]=2.58x10-2 M t=608 s, [A]=1.29x10-2 M Which of the following rate laws is consistent with the data?
rate=6.37x10-5 M s-1
For a reaction involving reactant X, which rate law is consistent with the following observation: If it takes 10.0 s for [X] to drop from 0.012M to 0.06M, it takes 5.0 s for [X] to drop from 0.06M to 0.03M. ?
rate=k
For a reaction involving reactant X, which rate law is consistent with the following observation: If it takes 40 s for [X] to drop from 0.80 to 0.40M, it takes 20 s it to drop from 0.40M to 0.20 M. ?
rate=k
For a reaction involving reactant X, which rate law is consistent with the following observation: The half life of X is directly proportional to [X]. ?
rate=k
For a reaction involving reactant R, which of the rate laws below (where k is a constant) is consistent with the following observation: The rate quadruples when the concentration of R is doubled.
rate=k[R]2
For a reaction involving reactant X, which rate law is consistent with the following observation: A plot of ln[X] vs. time is a straight line. ?
rate=k[X]
For a reaction involving reactant X, which rate law is consistent with the following observation: If it takes 24 s for [X] to drop from 1.0M to 0.50M, it takes 48 s to drop from 1.0M to 0.25M. ?
rate=k[X]
For a reaction involving reactant X, which rate law is consistent with the following observation: If it takes 3.6 minutes for [X] to drop from 0.20M to 0.10M, it takes 7.2 minutes for it to drop from 0.20M to 0.05M. ?
rate=k[X]
For a reaction involving reactant X, which rate law is consistent with the following observation: If it takes 35 s for [X] to drop from 0.80 to 0.40M, it also takes 35 s it to drop from 0.60M to 0.30 M. ?
rate=k[X]
For a reaction involving reactant X, which rate law is consistent with the following observation: ln[X] = ln[X]o - kt, where [X]o is the initial concentration and t is time. ?
rate=k[X]
For a reaction involving reactant X, which rate law is consistent with the following observation: 1/[X] = 1/[X]o + kt, where [X]o is the initial concentration and t is time. ?
rate=k[X]2
For a reaction involving reactant X, which rate law is consistent with the following observation: A plot of 1/[R] vs. time is a straight line. ?
rate=k[X]2
For a reaction involving reactant X, which rate law is consistent with the following observation: If it takes 15.0 s for [X] to drop from 0.20M to 0.10M , it takes 20.0 s to drop from 0.15 to 0.075. ?
rate=k[X]2
For a reaction involving reactant X, which rate law is consistent with the following observation: If it takes 20 s for [X] to drop from 0.16M to 0.08M, it takes 80 s for it to drop from 0.04M to 0.02M. ?
rate=k[X]2
For a reaction involving reactant X, which rate law is consistent with the following observation: If it takes 24 s for [X] to drop from 0.16M to 0.08M, it takes 72 s to drop from 0.16M to 0.04M. ?
rate=k[X]2
For a reaction involving reactant X, which rate law is consistent with the following observation: The half life of X is inversely proportional to [X]. ?
rate=k[X]2
If the rate law for the reaction of R and P is Rate = k [R] then which of the following could be a unit for the rate constant (k)?
s-1
