Chem

What is the rate of consumption of reactant A if its concentration decreases from 4.58x10-3 mol/L to 1.52x10-3 mol/L in 200.1 seconds.

1.53x10-5 M/s

A+B--> C+D

(A) 25k

Rate....

M.time-1

How many H atoms are in 75.2 g of C15H30?

6.45x1024 H atoms

State whether the following is soluble or insoluble in water: HgCl2

soluble

If the rate law for the reaction of X and Y is:Rate = k [X]2then order of reaction with respect to Y is

0

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/sExpt 2. [A]=0.301, [B]=0.500, rate=3.16x10-4 M/sExpt 3. [A]=0.301, [B]=0.982, rate=6.21x10-4 M/sWhat is the value of the rate constant?

0.00210 M-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]=0.300, [B]=0.500, rate=1.10x10-3 M/sExpt 2. [A]=0.219, [B]=0.500, rate=1.10x10-3 M/sExpt 3. [A]=0.219, [B]=1.53, rate=3.37x10-3 M/sWhat is the value of the rate constant?

0.00220 s-1

How many H atoms are in 32.4 g of C10H20?

2.78x1024 H atoms

Calculate the moles of carbonate ions in a mixture of 20.2 g calcium carbonate and 22.2 g aluminum carbonate.

0.486 mol carbonate ions

How many H atoms are in 9.82 g of C12H26?

9.02x1023 H atoms

How many H atoms are in 42.5 g of C13H26?

3.65x1024 H atoms

Consider the elementary reaction: A + A → B + C. True or False: The forward reaction is bimolecular.

true

Consider the following representation for a precipitation reaction. ASSUME that filled circles and triangles represent cations and unfilled circles and triangles represent anions; cations and anions can be monatomic or polyatomic. State whether the figure would be consistent with what would occur if the following solutions are mixed:Solution I (circles): potassium chlorideSolution II (triangles): mercury(I) nitrate

yes

Consider the following representation for a precipitation reaction. ASSUME that filled circles and triangles represent cations and unfilled circles and triangles represent anions; cations and anions can be monatomic or polyatomic. State whether the figure would be consistent with what would occur if the following solutions are mixed:Solution I (circles): potassium iodideSolution II (triangles): lead(II) nitrate

yes

If the rate law for the reaction of R and P isRate = k [R]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/sExpt 2. [A]=0.219, [B]=0.500, rate=8.03x10-4 M/sExpt 3. [A]=0.219, [B]=1.53, rate=2.46x10-3 M/sWhat is the value of the rate constant?

0.00733 M-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]=0.400, rate=1.61x10-3 M/sExpt 2. [A]=0.152, [B]=0.400, rate=1.61x10-3 M/sExpt 3. [A]=0.152, [B]=1.57, rate=2.48x10-2 M/sWhat is the value of the rate constant?

0.0101 M-1 s-1

How many moles of sodium ions are in 50.0 mL of 0.400 M Na2CO3?

0.0400 mol

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

Commercially available vinegar is typically labeled as having "5% acidity". This means that a 100-mL sample of this vinegar contains 5 grams of acetic acid (HC2H3O2). How many moles of acetic acid is present in a 150-mL sample of vinegar with "5% acidity"?

0.1249 mol

Calculate the moles of carbonate ions in a mixture of 10.9 g calcium carbonate and 18.5 g aluminum carbonate.

0.346 mol carbonate ions

If the rate law for the reaction of X and Y is:Rate = k [X] [Y]then order of reaction with respect to X is

1

If the rate law for the reaction of X and Y is:Rate = k [X] [Y]then order of reaction with respect to Y is

1

If the rate law for the reaction of X and Y is:Rate = k [X]2 [Y]then order of reaction with respect to Y is

1

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/sExpt 2. [A]=1.02, [B]=0.100, rate=3.86x10-3 M/sExpt 3. [A]=0.543, [B]=0.384, rate=1.48x10-2 M/sWhat is the order of reaction with respect to B?

1

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.

1.00x10-5 M/min

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 = (7.62x10-4 s-1) [R]. If the initial concentration of R is 1.27x10-2 M, calculate its concentration at 134 s.

1.15x10-2 M

How many H atoms are in 14.9 g of C14H26?

1.20x1024 H atoms

Consider the reaction3 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 = (1.69x10-3 s-1) [R]. If the initial concentration of R is 1.69x10-2 M, calculate its concentration at 98.8 s.

1.43x10-2 M

The rate law for a reaction is: rate = (9.79x10-4 s-1) [R]. If the initial concentration of R is 2.25x10-2 M, calculate its concentration at 238 s.

1.78x10-2 M

The rate law for a reaction is: rate = (9.79x10-4 s-1)[R]. If the initial concentration of R is 2.25x10-2 M, calculate the time it takes for the concentration to drop to 7.56x10-3 M.

1110 s

The rate law for a reaction is: rate = (1.72x10-1 M-1 s-1)[R]2. If the initial concentration of R is 9.54x10-3 M, calculate the time it takes for the concentration to drop to 3.37x10-3 M.

1120 s

The rate law for a reaction is: rate = (1.51x10-3 s-1)[R]. If the initial concentration of R is 8.18x10-2 M, calculate the time it takes for the concentration to drop to 1.28x10-2 M

1230 s

The rate law for a reaction is: rate = (1.45x10-1 M-1 s-1)[R]2. 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.

1280 s

The rate law for a reaction is: rate = (8.59x10-4 s-1)[R]. If the initial concentration of R is 5.29x10-2 M, calculate the time it takes for the concentration to drop to 1.68x10-2 M.

1340 s

The rate law for a reaction is: rate = (1.14x10-3 s-1)[R]. If the initial concentration of R is 9.37x10-2 M, calculate the time it takes for the concentration to drop to 1.94x10-2 M.

1380 s

The rate law for a reaction is: rate = (1.61x10-1 M-1 s-1)[R]2. If the initial concentration of R is 2.99x10-2 M, calculate the time it takes for the concentration to drop to 3.89x10-3 M.

1390 s

The rate law for a reaction is: rate = (6.28x10-2 M-1 s-1)[R]2. If the initial concentration of R is 2.25x10-2 M, calculate the time it takes for the concentration to drop to 7.56x10-3 M

1400 s

The rate law for a reaction is: rate = (2.34x10-2 M-1 s-1)[R]2. If the initial concentration of R is 5.29x10-2 M, calculate the time it takes for the concentration to drop to 1.68x10-2 M.

1740 s

If the rate law for the reaction of X and Y is:Rate = k [X]2 [Y]then order of reaction with respect to X is

2

If the rate law for the reaction of X and Y is:Rate = k [Y]2then order of reaction with respect to Y is

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/sExpt 2. [A]=0.301, [B]=0.500, rate=3.16x10-4 M/sExpt 3. [A]=0.301, [B]=0.982, rate=1.22x10-3 M/sWhat 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/sExpt 2. [A]=0.301, [B]=0.500, rate=9.51x10-4 M/sExpt 3. [A]=0.301, [B]=0.982, rate=1.87x10-3 M/sWhat 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]=0.100, rate=6.72x10-4 M/sExpt 2. [A]=0.100, [B]=0.100, rate=1.68x10-4 M/sExpt 3. [A]=0.100, [B]=0.400, rate=6.72x10-4 M/sWhat 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]=0.200, rate=4.29x10-3 M/sExpt 2. [A]=0.397, [B]=0.200, rate=1.69x10-2 M/sExpt 3. [A]=0.397, [B]=0.409, rate=3.46x10-2 M/sWhat 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/sExpt 2. [A]=0.647, [B]=0.400, rate=1.72x10-4 M/sExpt 3. [A]=1.06, [B]=0.411, rate=1.82x10-4 M/sWhat is the order of reaction with respect to B?

2

A solution is prepared by mixing 13.1 mL of 0.440 M NH4NO3(aq) and 23.1 mL of 0.600 M NH4NO3(aq), then adding enough water to bring the total volume to 800.0 mL. Calculate the molarity of NH4NO3 in the resulting solution.

2.45x10-2 M

The rate law for a reaction is: rate = (3.40x10-3 s-1) [R]. If the initial concentration of R is 3.00x10-3 M, calculate its concentration at 57.9 s.

2.46x10-3 M

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

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

The rate law for a reaction is: rate = 7.19x10-5 M s-1. If the initial concentration of R is 2.99x10-2 M, calculate its concentration at 27.0 s.

2.80x10-2 M

The rate law for a reaction is: rate = (1.76x10-2 M-1 s-1)[R]2. If the initial concentration of R is 9.37x10-2 M, calculate the time it takes for the concentration to drop to 1.94x10-2 M.

2320 s

The rate law for a reaction is: rate = (2.66x10-2 M-1 s-1)[R]2. If the initial concentration of R is 8.18x10-2 M, calculate the time it takes for the concentration to drop to 1.28x10-2 M.

2480 s

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

What is the rate of consumption of reactant A if its concentration decreases from 3.83x10-3 mol/L to 2.14x10-3 mol/L in 514.3 seconds.

3.29x10-6 M/s

A 117.5-mL sample of aqueous solution contains 17.4 grams of sodium hydroxide. What is the molarity of the sodium hydroxide in the solution?

3.71 M

Consider the reaction3 A(aq) + B(aq) → 2 C(aq)If the rate of production of C is 3.85x10-3 M s-1, what is the rate of consumption of A?

5.76x10-3 M s-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 45.3 kJ/mol. If the half life at 28.6oC is found to be 645 s, calculate the half life at 88.3oC.

32.7 s

The rate law for a reaction is: rate = (3.40x10-3 s-1)[R]. If the initial concentration of R is 3.00x10-3 M, calculate the time it takes for the concentration to drop to 8.52x10-4 M.

370

What is the molar concentration of sodium ions in a 0.406M sodium chloride(aq) solution?

4.06x10-1 M Na+

The rate law for a reaction is: rate = (8.59x10-4 s-1) [R]. If the initial concentration of R is 5.29x10-2 M, calculate its concentration at 257 s.

4.24x10-2 M

How many H atoms are in 47.6 g of C15H32?

4.32x1024 H atoms

The rate law for a reaction is: rate = 3.28x10-5 M s-1. If the initial concentration of R is 5.29x10-2 M, calculate its concentration at 257 s.

4.45x10-2 M

What is the molar concentration of sodium ions in a 0.156M Na3PO4(aq) solution?

4.68x10-1 M Na+

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 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

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 52.8 kJ/mol. If the half life at 29.7oC is found to be 485 s, calculate the half life at 69.5oC.

42.4 s

How many H atoms are in 65.1 g of C11H20?

5.14x1024 H atoms

How many H atoms are in 70.2 g of C13H24?

5.63x1024 H atoms

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 its concentration at 80.2 s.

5.99x10-3 M

The rate constant of a reaction (k) was determined over a range of temperatures. A plot of ln(k) vs. 1/T from 33.0oC to 94.0oC is linear with a slope of -6040 K. What is the energy of activation?

50.2 kJ/mol

The rate law for a reaction is: rate = (1.63x100 M-1 s-1)[R]2. If the initial concentration of R is 3.00x10-3 M, calculate the time it takes for the concentration to drop to 8.52x10-4 M.

516 s

The rate law for a reaction is: rate = (8.66x10-2 M-1 s-1)[R]2. 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.

5260 s

Plants combine water (from the soil) and carbon dioxide (from the air) to make a simple sugar (glucose, C6H12O6). In the process, they release oxygen to the atmosphere. The best balanced equation that represents this reaction is

6 H2O(l) + 6 CO2(g) → C6H12O6(s) + 6 O2(g)

The rate law for a reaction is: rate = 1.16x10-5 M s-1. If the initial concentration of R is 7.17x10-3 M, calculate its concentration at 80.2 s.

6.24x10-3 M

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

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 the time it takes for the concentration to drop to 3.89x10-3 M.

612 s

A 105.6-mL sample of aqueous solution contains 98.1 grams of ammonium sulfate. What is the molarity of the ammonium sulfate in the solution?

7.03 M

The rate law for a reaction is: rate = 7.82x10-6 M s-1. If the initial concentration of R is 9.54x10-3 M, calculate its concentration at 215 s.

7.05x10-3 M

The rate law for a reaction is: rate = (1.51x10-3 s-1) [R]. If the initial concentration of R is 8.18x10-2 M, calculate its concentration at 71.8 s.

7.34x10-2 M

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

The rate law for a reaction is: rate = 8.89x10-5 M s-1. If the initial concentration of R is 8.18x10-2 M, calculate its concentration at 71.8 s.

7.54x10-2 M

What is the rate of production of product X if its concentration increases from 1.39x10-3 mol/L to 3.26x10-3 mol/L in 243.3 seconds.

7.68x10-6 M/min

What is the rate of consumption of reactant A if its concentration decreases from 3.26x10-3 mol/L to 1.39x10-3 mol/L in 243.3 seconds.

7.68x10-6 M/s

The rate law for a reaction is: rate = (1.14x10-3 s-1) [R]. If the initial concentration of R is 9.37x10-2 M, calculate its concentration at 125 s.

8.12x10-2 M

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

A solution is prepared by mixing 37.2 mL of 0.389 M C6H12O6(aq) and 43.0 mL of 0.490 M C6H12O6(aq), then adding 319.8 mL of water. Assuming the liquid volumes are additive, calculate the molarity of C6H12O6 in the resulting solution.

8.88x10-2 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

How many moles of H atoms are in 70.2 g of C13H24?

9.34 mol H

What is the rate of consumption of reactant A if its concentration decreases from 6.45x10-3 mol/L to 2.39x10-3 mol/L in 414.8 seconds.

9.79x10-6 M/s

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 the time it takes for the concentration to drop to 3.37x10-3 M.

913 s

rate limiting

C

The souring of wine is due to the conversion of ethyl alcohol (C2H5OH, the intoxicating ingredient) into acetic acid (CH3COOH, the sour ingredient of vinegar). In this process, oxygen molecules (from air) react with ethyl alcohol molecules to produce acetic acid and water molecules. The best balanced equation that represents this reaction is

C2H5OH(aq) + O2(g) → CH3COOH(aq) + H2O(l)

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 waterExpt 2. 2.00 mL A(aq) + 3.50 mL B(aq) + 4.50 mL waterExpt 3. 2.00 mL A(aq) + 3.50 mL B(aq) + 6.50 mL waterWhich pair of experiments would allow you to determine the order of reaction with respect to B?

Expt 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]=0.200, [B]=0.100Expt 2. [A]=0.100, [B]=0.100Expt 3. [A]=0.100, [B]=0.400Which 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]=0.200, [B]=0.100Expt 2. [A]=0.100, [B]=0.400Expt 3. [A]=0.100, [B]=0.100Which pair of experiments allows us to determine the order of reaction with respect to A?

Expts 1 and 3

Consider the elementary reaction: A → B + C. True or False: The forward reaction is second order with respect to A.

False

Consider the elementary reaction: A + A → B + C. True or False: The forward reaction is first order with respect to A.

False

Consider the elementary reaction: A + B → C. True or False: The reverse reaction is second order overall.

False

Consider the elementary reaction: A + B → C. True or False: The reverse reaction is second order with respect to C.

False

Consider the elementary reaction: A → B + C. True or False: The forward reaction is bimolecular.

False

Which of the potential energy diagrams shown below represent a reaction with no intermediate.?

I

Which of the potential energy diagrams shown below represent a reaction with product C.?

I

Which of the potential energy diagrams shown below represent an elementary reaction?

I

Which of the potential energy diagrams shown below represent an endothermic reaction with a two step mechanism and a slower first step?

II

Which of the potential energy diagrams shown below represent a two-step mechanism that is exothermic?

III

Which of the potential energy diagrams shown below represent a two step mechanism with a slow second step?

IV

Which of the following represents a precipitation reaction?

KCl(aq) + AgNO3(aq) → AgCl(s) + KNO3(aq)

If the rate law for the reaction of R and P isRate = k [R] [P]then which of the following could be a unit for the rate constant (k)?

L mol-1 hr-1

If the rate law for the reaction of R and P isRate = k [P]2then which of the following could be a unit for the rate constant (k)? Select one:

L mol-1 s-1

If the rate law for the reaction of R and P isRate = k [R]2then 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 isRate = k [R] [P]2 then which of the following could be a unit for the rate constant (k)?

L2 mol-2 min-1

If the rate law for the reaction of R and P isRate = k [R] [P]2then which of the following could be a unit for the rate constant (k)?

L2 mol-2 min-1

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 mol-2 s-1

If the rate law for the reaction of R and P isRate = k [R]2 [P]then which of the following could be a unit for the rate constant (k)?

L2 mol-2 s-1

Which of the following is soluble in water?

MgSO4

Which of the following is a precipitation reaction?

Na2CO3(aq) + 2 AgNO3(aq) → Ag2CO3(s) + 2 NaNO3(aq)

weird graph thing

The correct answer is: (C)

The rate law for a reaction is: rate = 1.59x10-5 M s-1. If the initial concentration of R is 2.25x10-2 M, calculate its concentration at 238 s.

The correct answer is: 1.87x10-2 M

Consider the following representation for the precipitation reaction that occurs when solutions of lead(II) nitrate and potassium iodide are mixed. The lead(II) ions are represented by

The correct answer is: filled triangles

If the rate law for the reaction of R and P isRate = k [R]then which of the following could be a unit for the rate constant (k)?

The correct answer is: s-1

Classify the following: Mg(OH)2(s) + HCl(aq) → MgCl2(aq) + H2O(l)

acid-base neutralization reaction

Classify the following: HC2H3O2 + NaOH(aq) → NaC2H3O2(aq) + H2O(l)

acid-base neutralization reaction

Consider the elementary reaction: A + A → B + C. True or False: The reverse reaction is bimolecular.

True

Consider the elementary reaction: A + B → C. True or False: The forward reaction is bimolecular.

True

Consider the elementary reaction: A + B → C. True or False: The forward reaction is first order with respect to B.

True

Consider the elementary reaction: A + B → C. True or False: The forward reaction is second order overall.

True

Consider the elementary reaction: A → B + C. True or False: The reverse reaction is first order with respect to B.

True

Consider the elementary reaction: A + B → C. True or False: The forward reaction is first order with respect to A.

True

Consider the elementary reaction: A → B + C. True or False: The reverse reaction is second order overall.

True

Consider the elementary reaction: A → B + C. True or False: The forward reaction is first order with respect to A.

True

Consider the precipitation reactions that could occur when the following pairs of aqueous solutions are mixed:Reaction 1. iron(II) nitrate + sodium carbonateReaction 2. calcium nitrate + sodium carbonateThe formula Fe2+ will

appear in the net ionic equation for reaction 1 only.

A chlorine atom becomes an ion by

by gaining electron(s)

A magnesium atom becomes an ion by

by losing electron(s)

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 9.37x10-5 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 3.00x10-1 mol/L for X and 8.18x10-5 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 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

Consider the following representation for the precipitation reaction that occurs when solutions of lead(II) nitrate and potassium iodide are mixed. The potassium ions are represented by

filled circles

State whether the following is soluble or insoluble in water: Hg2Cl2

insoluble

State whether the following is soluble or insoluble in water: Zn3(PO4)2

insoluble

State whether the following is soluble or insoluble in water: barium sulfate

insoluble

State whether the following is soluble or insoluble in water: cadmium phosphate

insoluble

State whether the following is soluble or insoluble in water: chromium(III) hydroxide

insoluble

State whether the following is soluble or insoluble in water: silver chloride

insoluble

State whether the following is soluble or insoluble in water:silver bromide

insoluble

If the rate law for the reaction of R and P isRate = kthen which of the following could be a unit for the rate constant (k)?

mol L-1 hr-1

Classify the following:HNO3(aq) + ZnCl2(aq) → Zn(NO3)2(aq) + HCl(aq)

no reaction

For the precipitation reaction that occurs when BaBr2(aq) and MgSO4(aq) are mixed, state whether the following appear in the net ionic equation: Ba+, SO4-.

no, no

For the precipitation reaction that occurs when K3PO3(aq) and CaCl2(aq) are mixed, state whether the following appear in the net ionic equation: K3+, PO43-.

no, yes

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 waterExpt 2. 2.50 mL A(aq) + 4.50 mL B(aq) + 3.00 mL waterExpt 3. 2.50 mL A(aq) + 4.50 mL B(aq) + 5.00 mL waterWhich pair of experiments would allow you to determine the order of reaction with respect to A?

none

Consider the precipitation reactions that could occur when the following pairs of aqueous solutions are mixed:Reaction 1. iron(II) nitrate + sodium carbonateReaction 2. calcium nitrate + sodium carbonateThe formula NO3- will

not appear in the net ionic equation for either reaction because it is a spectator ion or because it is not a precipitate

Classify the following: H2SO4(aq) + Ba(OH)2(aq) → H2O(l) + BaSO4(s)

precipitation and acid-base neutralization

Classify the following: Zn(NO3)2(aq) + (NH4)2S(aq) → ZnS(s) + NH4NO3(aq)

precipitation reaction

Classify the following:H2SO4(aq) + Ba(NO3)2(aq) → HNO3(aq) + BaSO4(s)

precipitation reaction

The concentration of reactant A was monitored over time and the following data were obtained:t=0, [A]=3.34x10-2 Mt=665 s, [A]=1.67x10-2 Mt=1330 s, [A]=8.35x10-3 M Which of the following rate laws is consistent with the data?

rate = (1.04x10-3 s-1) [A]

The concentration of reactant A was monitored over time and the following data were obtained:t=0, [A]=9.37x10-2 Mt=606 s, [A]=4.68x10-2 Mt=1210 s, [A]=2.34x10-2 MWhich of the following rate laws is consistent with the data?

rate = (1.14x10-3 s-1) [A]

The concentration of reactant A was monitored over time and the following data were obtained:t=0, [A]=8.18x10-2 Mt=460 s, [A]=4.09x10-2 Mt=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]=2.99x10-2 Mt=208 s, [A]=1.50x10-2 Mt=624 s, [A]=7.48x10-3 M Which of the following rate laws is consistent with the data?

rate = (1.61x10-1 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=215 s, [Z]=6.71x10-3 M) and (t=458 s, [Z]=4.50x10-3 M)

rate = (1.64x10-3 s-1) [Z]

The concentration of reactant A was monitored over time and the following data were obtained:t=0, [A]=1.69x10-2 Mt=409 s, [A]=8.45x10-3 Mt=818 s, [A]=4.22x10-3 M Which of the following rate laws is consistent with the data?

rate = (1.69x10-3 s-1) [A]

The concentration of reactant A was monitored over time and the following data were obtained:t=0, [A]=4.70x10-2 Mt=514 s, [A]=2.35x10-2 Mt=1540 s, [A]=1.18x10-2 M Which of the following rate laws is consistent with the data?

rate = (4.14x10-2 M-1 s-1) [A]2

The concentration of reactant A was monitored over time and the following data were obtained:t=0, [A]=2.65x10-2 Mt=665 s, [A]=1.32x10-2 Mt=2000 s, [A]=6.62x10-3 M Which of the following rate laws is consistent with the data?

rate = (5.67x10-2 M-1 s-1) [A]2

The concentration of reactant A was monitored over time and the following data were obtained:t=0, [A]=5.29x10-2 Mt=807 s, [A]=2.64x10-2 Mt=1610 s, [A]=1.32x10-2 M Which of the following rate laws is consistent with the data?

rate = (8.59x10-4 s-1) [A]

The concentration of reactant A was monitored over time and the following data were obtained:t=0, [A]=3.60x10-3 Mt=292 s, [A]=1.80x10-3 Mt=876 s, [A]=9.00x10-4 M Which of the following rate laws is consistent with the data?

rate = (9.51x10-1 M-1 s-1) [A]2

Consider a reaction involving reactant Z where a plot of [Z] vs. time can be fitted to a straight line. Two of the points on the best-fit line correspond to:(t=80.2 s, [Z]=6.24x10-3 M) and (t=135 s, [Z]=5.61x10-3 M)

rate = 1.15x10-5 M s-1

The concentration of reactant A was monitored over time and the following data were obtained:t=0, [A]=1.07x10-2 Mt=366 s, [A]=5.35x10-3 Mt=549 s, [A]=2.68x10-3 M Which of the following rate laws is consistent with the data?

rate = 1.46x10-5 M s-1

The concentration of reactant A was monitored over time and the following data were obtained:t=0, [A]=2.25x10-2 Mt=708 s, [A]=1.12x10-2 Mt=1060 s, [A]=5.62x10-3 M Which of the following rate laws is consistent with the data?

rate = 1.59x10-5 M s-1

The concentration of reactant A was monitored over time and the following data were obtained:t=0, [A]=3.34x10-2 Mt=665 s, [A]=1.67x10-2 Mt=998 s, [A]=8.35x10-3 M Which of the following rate laws is consistent with the data?

rate = 2.51x10-5 M s-1

The concentration of reactant A was monitored over time and the following data were obtained:t=0, [A]=8.01x10-3 Mt=742 s, [A]=4.00x10-3 Mt=1110 s, [A]=2.00x10-3 M Which of the following rate laws is consistent with the data?

rate = 5.40x10-6 M s-1

The concentration of reactant A was monitored over time and the following data were obtained:t=0, [A]=5.91x10-2 Mt=514 s, [A]=2.96x10-2 Mt=771 s, [A]=1.48x10-2 M Which of the following rate laws is consistent with the data?

rate = 5.75x10-5 M s-1

The concentration of reactant A was monitored over time and the following data were obtained:t=0, [A]=4.53x10-3 Mt=292 s, [A]=2.26x10-3 Mt=438 s, [A]=1.13x10-3 M Which of the following rate laws is consistent with the data?

rate = 7.76x10-6 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:The half life of X is directly proportional to [X].?

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

Consider the following fictitious mechanism: Step 1. R + S → T, slow Step 2. T + U → W + S, fast Which would be the observe experimental rate law?

rate = k[R]

Consider the following fictitious mechanism:Step 1. R + S → T, slowStep 2. T + U → W + S, fastWhich would be the observed rate law for the reaction?

rate = k[R][S]

Consider the following fictitious mechanism:Step 1. R + S → T, (fast, reversible)Step 2. T + U → W + S, slowWhich is the rate law for the reaction?

rate = k[R][U]

Consider the following fictitious mechanism: Step 1. R + S → T, (fast, reversible) Step 2. T + U → W + S, slow Which is the rate law for the reaction?

rate = k[R][U][S]

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:The half life of X is constant.?

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:The half life of X is inversely proportional to [X].?

rate=k[X]2

State whether the following is soluble or insoluble in water: MgCl2

soluble

State whether the following is soluble or insoluble in water: Na2CrO4

soluble

State whether the following is soluble or insoluble in water: potassium chromate

soluble

State whether the following is soluble or insoluble in water: ammonium sulfate

soluble