Chem. Chapter 13 Test

derive an expression for a "1/3-life" for a first-order reaction

1.099/k

given the following balanced equation, determine the rate of reaction with respect to [O₂]. If the rate of formation of O₂ is 7.78*10⁻¹ M/s, what is the rate of the loss of O₃ (2O₃(g)→3O₂(g))

1.17 M/s

if the activation energy for a given compound is found to be 103 kJ/mol, with a frequency factor of 4.0*10¹³s⁻¹, what is the rate constant for this reaction at 398K

1.2 s⁻¹

the second-order reaction 2Mn(CO)₅→Mn₂(CO)₁₀, has a rate constant equal to 3.0*10⁹ M⁻¹s⁻¹ at 25°C. if the initial concentration of Mn(CO)₅ is 2.0*10⁻⁵M, how long will it take for 90%of the reactant to disappear

1.5*10⁻⁴s

a particular first-order reaction has a rate constant of 1.35*10² s⁻¹ at 25.0°c. what is the magnitude of k at 75.0°C if Ea= 85.6 kJ/mol

1.92*10⁴s⁻¹

what are the units of k in the following rate law (Rate= k[X]

1/Ms

what are the units of k in the following rate law (Rate= k[X][Y]

1/Ms

what are the units of k in the following rate law (Rate=k[X]²[Y]²

1/M³s

which of the following represents the integrated rate law for a second-order reaction

1/[A]t - 1/[A]₀ =kt

what data should be plotted to show that experimental concentration data fits a second-order reaction

1/[reactant] vs. time

what are the units of k in the first order reaction

1/s

the following reaction is first order, C₂H₆→2CH₃. if the rate constant is equal to 5.5*10⁻⁴s⁻¹ at 1000K, how long will it take for 0.35 mol of C₂H₆ in a 1.00L container to decrease to 0.20 mol in the same container

17 min

how many half-lives are required for the concentration of reactant to decrease to 25% of its original value

2

the first-order reaction, 2N₂O(g)→2N₂(g)+O₂(g), has a rate constant equal to 0.76 s⁻¹ at 1000K. how long will it take for the concentration of N₂O to decrease to 12% of its initial concentration

2.8s

for a particular first-order reaction, it takes 24 minutes for the concentration of the reactant to decrease to 25% of its initial value. what is the value for rate constant (in s⁻¹) for the reaction

9.6*10⁻⁴s⁻¹

the isomerization of methylisonitrile to acetonitrile (CH₃NC(g)→CH₃CN(g)) is first order in CH₃NC. the half life of the reaction is 5.20*101s at 545 K. the rate constant when the initial [CH₃NC] is 0.030 M is

0.0133 s⁻¹

hydrogen iodide decomposes at 800K via a second-order process to produce hydrogen and iodine according to the following chemical equation (2HI(g)→H₂(g)+I₂(g) at 800K it take 142 seconds for the initial concentration of HI to decrease from 6.75*10⁻²M to 3.50*10⁻²M. what is the rate constant for the reaction at this temperature

9.69*10⁻²M⁻¹s⁻¹

the half-life for the second-order decomposition of HI is 15.4 s. when the initial concentration of HI is 0.67M. what is the rate constant for this reaction

9.7 *10⁻² M⁻¹s⁻¹

the rate of disappearance of HBr in the gas phase reaction (2HBr(g)→H₂(g)+Br₂(g)) is 0.130 Ms⁻¹ at 150°C. the rate of reaction is

0.0650 Ms⁻¹

the combustion of ethylene proceeds by the reaction (C₂H₄(g)+3O₂(g)→2CO₂(g)+2H₂O(g), when the rate of disappearance of O₂IS 0.23 M s⁻¹, the rate of disappearance of C₂H₄ is

0.077 Ms⁻¹

the rate constant for a first-order reaction is 0.54 M⁻¹s⁻¹. what is the half-life of this reaction if the initial concentration is 0.33M

0.089s

the decomposition of dinitrogen pentoxide is described by the chemical equation (2N₂O₅(g)→ 4NO₂(g)+O₂(g)). if the rate of appearance of NO₂ is equal to 0.560 mol/min at a particular moment, what is the rate of appearance of O₂ at that moment

0.140 mol/min

the combustion of ethylene proceeds by the reaction C₂H₄(g)+3O₂(g)→2CO₂+2H₂O(g) when the rate of disappearance of O₂ IS 0.28 Ms⁻¹, the rate of appearance of CO₂ is

0.19 Ms⁻¹

the rate constant for a zero-order reaction is 0.54 M⁻¹s⁻¹. what is the half-life of this reaction if the initial concentration is 0.33M

0.31s

the decomposition of dinitrogen pentoxide is described by the chemical equation (2N₂O₅(g)→4NO₂(g)+O₂. if the rate of appearance of O₂ is equal to 3.00 mol/min at a particular moment, what is the rate of disappearance of N₂O₅ at that moment

0.750 mol/min

the second-order decomposition of NO₂ has a rate constant of 0.255M⁻¹s⁻¹. how much NO₂ decomposes in 4.00s if the initial concentration of NO₂(1.00L volume) is 1.33M

0.77mol

the decomposition of dinitrogen pentaoxide is described by the chemical equation (2N₂O₅(g)→4NO₂(g)+O₂)). if the rate of disappearance of N₂O₅ is equal to 1.60mol/min at a particular moment, what is the rate of appearance of NO₂ at the moment

0.800 mol/min

the first-order decomposition of N₂O₅ at 328K has a rate constant of 1.70*10⁻³ s⁻¹. if the initial concentration of N₂O₅ is 2.88M, what is the concentration of N₂O₅ after 12.5 minutes

0.805M

the first-order decomposition of cyclopropane has a rate constant of 6.7*10⁻⁴ s⁻¹. if the initial concentration of cyclopropane is 1.33M, what is the concentration of cyclopropane after 644s?

0.86M

SO₂Cl₂ decomposes in the gas phase by the reaction (SO₂Cl₂(g)→ SO₂(g)+Cl₂) the reaction is first order in SO₂Cl₂ and the rate constant 3.0*10⁻⁶ s⁻¹ at 600K. a vessel is charged with 2.4 atm of SO₂Cl₂ at 600K. the partial pressure of SO₂Cl₂ at 3.0*10⁵ s is

0.98 atm

in the hydrogenation of double bonds, a catalyst is needed. in the first step, the reactant must come into contact with a metal surface. this step is known as

adsorption

biological catalysts that increase the rates of biochemical reactions are known as

enzymes

for a reaction that follows the general rate law, Rate= k[A][B]², what will happen to the rate of reaction if the concentration of B is increased by a factor of 3.00? the rate will

increase by a factor of 9.00

what data should be plotted to show that experimental concentration data fits a first-order reaction

ln[reactant] vs. time

which of the following statement is true

rate constants are temperature dependent

which rate law is bimolecular

rate= k[A][B]

what is the overall reaction order for the reaction that has the rate law: Rate= k[O₂][NO]H

second order

which of the following statements if FALSE

the half life of a first order reaction is dependent on the initial concentration of reactant

which of the following statements is FALSE

the half life of a second order reaction is not dependent on concentration

given the following rate law, how does the rate of reaction change if the concentration of X is doubled (Rate= k[X]²[Y]³)

the rate of reaction will increase by a factor of 4

give the characteristic of a first order reaction having only one reactant

the rate of the reaction is directly proportional to the concentration of the reactant

give the characteristic of a zero order reaction having only one reactant

the rate of the reaction is not proportional to the concentration of the reactant

give the characteristics of a second order reaction having only one reactant

the rate of the reaction is proportional to the square of the concentration of the reactant

identify the rate-determining step

the slowest step

which of the following represents the equation for a second-order half-life

t₁/₂ = 1/k[A]₀

which of the following represents the equation for a first-order half-life

t₁/₂ = 2k[A]₀/1

what are the units of k in the following rate law (Rate= k[X]⁰[Y]⁰

M-1 s-1

what are the units of k in the zero order reaction

M/s

what are the units of k in the following rate law (Rate=k[X][Y]¹/²

M⁻¹/² s⁻¹

what are the units of k in a second order reaction

M⁻¹s⁻¹

what are the units of k in the following rate law (Rate= k[X]²

M⁻¹s⁻¹

given the following balanced equation, determine the rate of reaction with respect to [NOCl] (2NO(g)+Cl₂(g) →2NOCl (g)

Rate = +1/2 [delta NOCl] / deltal t

given the following balanced equation, determine the rate of reaction with respect to [N₂] :(N₂(g)+3H₂→2NH₃(g)

Rate= +1/2 [delta NH₂]/delta t

given the following balanced equation, determine the rate of reaction with respect to [NH₃]: N₂(g)+2H₂(g)→2NH₃(g)

Rate= +1/2 [delta NH₃]/ delta t

given the following balanced equation, determine the rate of reaction with respect to [SO₂]: (2SO₂(g)+O₂→2SO₃(g)

Rate= -1/2 [delta SO₂]/Dt

given the following balanced equation, determine the rate of reaction with respect to [H₂]: (N₂(g)+3H₂(g)→2NH₃(g)

Rate= -1/3[delta H₂]/ delta t

determine the rate law and the value of k for the following reaction using the data provided

Rate= 5.2*10⁻³s⁻¹ [N₂O₅]

what is the overall order of the following reaction, given the rate law (X+2Y →4Z , Rate= k[X][Y]

2nd order

how many half lives-are required for the concentration of reactant to decrease to 12.5% of its original value

3

what is the overall order of the following reaction, given the rate law (2NO(g)+H₂(g)→N₂(g)+2H₂O(g), Rate= k[NO]²[H₂]

3rd order

if the concentration of a reactant is 6.25%, how many half-lives has it gone through

4

a reaction is found to have an activation energy of 38.0kJ/mol. if the rate constant for this reaction is 1.60*10² M⁻¹s⁻¹ at 249K, what is the rate constant at 436K

4.20*10⁵ M⁻¹s⁻¹

given the following balanced equation, determine the rate of reaction with respect to [O₂]. if the rate of O₂ loss is 2.64*10⁻³ M/s, what is the rate of formation of SO₃

5.28*10⁻³M/s

for the first-order reaction, 2N₂O(g)→2N₂(g)+O₂(g), what is the concentration of N₂O after 3 half-lives of 0.25 mol of N₂O is initially placed into a 1.00-L reaction vessel

6.2*10⁻²M

the first-order reaction, SO₂Cl₂→SO₂+Cl₂, has the rate constant equal to 2.20*10⁻⁵ s⁻¹ at 593K. what percentage of the initial amount of SO₂Cl₂ will remain after 6.00 hours

62.2%

the first-order decay of radon has a half-life of 3.823 days. how many grams of radon remain after 7.22 days if the sample initially weighs 250.0grams

67.5g

the isomerization of methylisonitrile to acetonitrile (CH₃NC(g)→CH₃CN(g) is first order in CH₃NC.

7.33*10³

identify an homogeneous catalyst

H₂SO₄ with concentrated HCl

in the hydrogenation of double bonds, a catalyst is needed. in the last step, the reactants must escape from the surface into the gas phase. this step is known as

desorption