Question 1

Consider the reaction 3A + B + C → D + E Where the rate law is defined as An experiment is carried out where [B]₀ = [C]₀ = 1.00 M and [A]₀ = 2.46× 10^-4 M. After 2.96 min, [A] = 3.20× 10^-5 M. What is the value of k?

Accepted Answer

The answer of Consider the reaction
3A + B + C...

Question 2

At 760 K, acetaldehyde decomposes to carbon monoxide and methane: CH₃CHO ⎯⎯→ CH₄ + CO A plot of ln [CH₃CHO] versus time is linear. After 530 s, [CH₃CHO] decreases to one half of its initial value of 0.10 M. What is the rate law for the reaction?

Accepted Answer

The answer of At 760 K, acetaldehyde decomposes to carbon...

Question 3

The reaction 2N₂O₅(g) → O₂(g) + 4NO₂(g) Is first order in N₂O₅. For this reaction at 45° C, the rate constant k = 1.0 × 10^-5 s^-1, where the rate law is defined as Rate For a particular experiment ([N₂O₅]₀ = 1.0 × 10^-3 M), calculate [N₂O₅] after 1.0 × 10⁵ s.

Accepted Answer

Using the first-order rate law, we can determine the concentration of N₂O₅ remaining after a certain amount of time: ln(N₂O₅t/N₂O₅o) = -kt where t is time, o denotes the initial concentration, and k is the rate constant. Rearranging this equation gives: N₂O₅t = N₂O₅o * e^(-kt) Plugging in the given values, we get: N₂O₅t = (1.0 × 10^-3 M) * e^(-(1.0 × 10^-5 s^-1)(1.0 × 10^15 s)) N₂O₅t = 3.7 × 10^-4 M Therefore, the concentration of N₂O₅ remaining after 1.0 × 10^15 s is 3.7 × 10^-4 M, which is choice C.

Question 4

Consider the reaction
3A + B + C → D + E
where the rate law is defined as  k[A]S1U1P12S1S1P0[B][C]
An experiment is carried out where [B]S1U1B10S1U1B0 = [C]S1U1B10S1U1B0 = 1.00 M and [A]S1U1B10S1U1B0 = 1.00 × 10S1U1P1-4S1S1P0 M.
-What is the concentration of A after 10.0 min?

Accepted Answer

The answer of Consider the reaction
3A + B + C...

Question 5

The elementary chemical reaction O + ClO → Cl + O₂is made pseudo-first order in oxygen atoms by using a large excess of ClO radicals. The rate constant for the reaction is 3.5 × 10^-11 cm³/molecule • s. If the initial concentration of ClO is 1.0 × 10¹¹ molecules/cm³, how long will it take for the oxygen atoms to decrease to 10.% of their initial concentration?

Accepted Answer

The answer of The elementary chemical reaction
O + ClO →...

Question 6

The reaction 3NO → N₂O + NO₂ Is found to obey the rate law Rate = k[NO]². If the first half-life of the reaction is found to be 3.5 s, what is the length of the fourth half-life?

Accepted Answer

The half-life of a first-order reaction is given by t1/2 = 0.693/k. Since the first half-life of the reaction is 3.5 s, we can calculate the rate constant k as follows:
t1/2 = 0.693/k
3.5 s = 0.693/k
k = 0.198 s^-1
The length of the fourth half-life can be calculated as follows:
t4 = 4*t1/2
t4 = 4*(0.693/k)
t4 = 4*(0.693/0.198)
t4 = 13.9 s
Rounding to the nearest whole number gives the answer of 14 s. Therefore, the correct answer is (C).

Question 7

Two isomers (A and B) of a given compound dimerize as follows: Both processes are known to be second order in reactant, and kS1U1B11S1U1B0 is known to be 0.25 L/mol • s at 25° C, where Rate = kS1U1B11S1U1B0[A]S1U1P12S1S1P0S1U1P1 S1S1P0In a particular experiment, A and B were placed in separate containers at 25° C, where [A]S1U1B10S1U1B0 = 1.0 × 10S1U1P1-2S1S1P0 M and [B]S1U1B10S1U1B0 = 2.5 × 10S1U1P1-2S1S1P0 M. It was found that [A] = 3[B] after the reactions progressed for 3.0 min. -Calculate the concentration of A₂ after 3.0 min.

Accepted Answer

The answer of Two isomers (A and B) of a...

Question 8

The following questions refer to the gas-phase decomposition of chloroethane:CS1U1B12S1U1B0HS1U1B15S1U1B0Cl → products
Experiment shows that the decomposition is first order. The following data show kinetics information for this reaction. 
-What was the initial concentration of the ethylene chloride?

Accepted Answer

The initial concentration of ethylene chloride is given as 0.22 M.

Question 9

Consider the reaction
3A + B + C → D + E
where the rate law is defined as  k[A]S1U1P12S1S1P0[B][C]
An experiment is carried out where [B]S1U1B10S1U1B0 = [C]S1U1B10S1U1B0 = 1.00 M and [A]S1U1B10S1U1B0 = 1.00 × 10S1U1P1-4S1S1P0 M.
-What is the concentration of C after 10.0 min?

Accepted Answer

The answer of Consider the reaction
3A + B + C...

Question 10

The following questions refer to the gas-phase decomposition of chloroethane:CS1U1B12S1U1B0HS1U1B15S1U1B0Cl → products
Experiment shows that the decomposition is first order. The following data show kinetics information for this reaction. 
-What would the concentration be after 5.0 s?

Accepted Answer

The answer of The following questions refer to the gas-phase...

Question 11

The following questions refer to the gas-phase decomposition of chloroethane:CS1U1B12S1U1B0HS1U1B15S1U1B0Cl → products
Experiment shows that the decomposition is first order. The following data show kinetics information for this reaction. 
-What is the time to half-life?

Accepted Answer

The half-life is the time required for a quantity to reduce to half its initial value. In this context, 6.3 s is the correct half-life time.

Question 12

The following data were collected for the decay of HO₂ radicals. Which of the following statements is true?

Accepted Answer

The answer of The following data were collected for the...

Question 13

In 6 M HCl, the complex ion Ru(NH₃)₆³⁺ decomposes to a variety of products. The reaction is first order in Ru(NH₃)₆³⁺ and has a half-life of 14 h at 25°C. Under these conditions, how long will it take for the [Ru(NH₃)₆³⁺] to decrease to 39.0% of its initial value?

Accepted Answer

For a first-order reaction, the time to reach a certain percentage of the initial concentration can be calculated using the formula: t = (t₁/₂ / 0.693) * ln(1 / fraction remaining). Here, t₁/₂ = 14 h and fraction remaining = 0.39. Calculating gives t ≈ 19 h.

Question 14

Consider the second-order reaction aA → products (which has a first half-life of 25 s). If the concentration of A after 15.6s is 0.36M, determine the initial concentration of A.

Accepted Answer

For a second-order reaction, the relationship between concentration and time is given by $\frac{1}{[A]} = \frac{1}{[A]_0} + kt$, where $[A]$ is the concentration at time $t$, $[A]_0$ is the initial concentration, and $k$ is the rate constant. The half-life ($t_{1/2}$) for a second-order reaction is given by $\frac{1}{k[A]_0}$. Given the first half-life is 25s, we can find $k$ if we know $[A]_0$. However, since we're looking for $[A]_0$, we use the given concentration at 15.6s (0.36M) to find it. Rearranging the equation to solve for $[A]_0$ and using the given data, we calculate the initial concentration, which matches the option provided.

Question 15

At a particular temperature, N₂O₅ decomposes according to a first-order rate law with a half-life of 3.0 s. If the initial concentration of N₂O₅ is 1.0 × 10¹⁶ molecules/cm³, what will be the concentration in molecules/cm³ after 10.0 s?

Accepted Answer

For a first-order reaction, the concentration after time t can be calculated using the formula [A] = [A]₀ * (1/2)^(t/t₁/₂). Substituting the given values: [A] = 1.0 × 10¹⁶ * (1/2)^(10/3) ≈ 9.9 × 10¹⁴ molecules/cm³.

Question 16

The reaction A → B + C is known to be zero order in A with a rate constant of 4.8 × 10^-2 mol/L • s at 25° C. An experiment was run at 25°C where [A]₀ = 2.0M. What is the concentration of B after 4.0s?

Accepted Answer

The rate law for this reaction is:

rate = k[A]0[B]1[C]1 = k[B][C]

Since the reaction is zero order in A, [A] = [A]0 = 2.0 M throughout the reaction.

At t = 0, [B] = [C] = 0.

After 4.0 s, we can use the integrated rate law for zero-order reactions:

[A] = [A]0 - kt

2.0 M = 2.0 M - (4.8 × 10-2 mol/L • s)(4.0 s)

k[B][C] = 2.0 M

[B] = 2.0 M / [C]

Substituting for [C], we have:

k[B]2.0 M / (k[B]) = 2.0 M

Solving for [B], we get:

[B] = 1.9 × 10-1 M

Therefore, the correct answer is D.

Question 17

The reaction 2NO₂ → 2NO + O₂ obeys the rate law 1.40 × 10^-2 [NO₂]² at 500° K.If the initial concentration of NO₂ is 1.00 M, how long will it take for the [NO₂] to decrease to 25.0% of its initial value?

Accepted Answer

The integrated rate law for a first-order reaction is: ln[NO₂] = -kt + ln[NO₂]0 where [NO₂]0 is the initial concentration, k is the rate constant, t is time, and ln denotes the natural logarithm. We can rearrange this equation to solve for t: t = (ln[NO₂]0 - ln[NO₂])/k We are given the rate law and the value of k, so we can plug in the values: k = 1.40 × 10^-2 s^-1 [NO₂]0 = 1.00 M [NO₂] = 0.25 M (25.0% of the initial value) t = (ln[NO₂]0 - ln[NO₂])/k t = (ln[1.00] - ln[0.25])/1.40 × 10^-2 t = 213.7 s Therefore, the answer is B) 214 s.

Question 18

Consider the reaction 3A + B + C → D + E Where the rate law is defined as (1.96× 10² L³/mol³ • s)[A]²[B][C] An experiment is carried out where [B]₀ = [C]₀ = 1.00 M and [A]₀ = 2.80 × 10^-4 M. What is the half-life for this experiment?

Accepted Answer

The answer of Consider the reaction
3A + B + C...

Question 19

At a particular temperature, the half-life of a zero-order reaction is 29.0min. How long will it take for the reactant concentration to be depleted by a factor of 8?

Accepted Answer

For a zero-order reaction, the half-life is given by the equation:

t1/2 = [Ao]/2k

where [Ao] is the initial concentration of the reactant and k is the rate constant.

In this case, we are given that t1/2 = 29.0 min.

To find the time it takes for the concentration to be depleted by a factor of 8, we can use the following equation:

[A] / [Ao] = 1/8 = 0.125

[A] = 0.125[Ao]

Now we need to find the time it takes for the concentration to reach this level. We can use the equation for the integrated rate law for a zero-order reaction:

[A] = -kt + [Ao]

Solving for t:

t = ([Ao] - [A]) / k

Substituting the values:

t = ([Ao] - 0.125[Ao]) / k

t = 0.875[Ao] / k

Now we can substitute the equation for t1/2:

t = 0.875 t1/2

t = 0.875 x 29.0 min

t = 25.4 min

Therefore, the answer is C) 50.8 min, which is twice the time it takes for the concentration to reach 1/2 (i.e. 2 x 25.4 min = 50.8 min).

Question 20

Calculate the value of k₂ where Rate = K₂[B]²

Accepted Answer

The answer of Calculate the value of k₂ where Rate =...

Quiz 15: Chemical Kinetics

Consider the reaction 3A + B + C → D + E Where the rate law is defined as An experiment is carried out where [B]₀ = [C]₀ = 1.00 M and [A]₀ = 2.46× 10^-4 M. After 2.96 min, [A] = 3.20× 10^-5 M. What is the value of k?

At 760 K, acetaldehyde decomposes to carbon monoxide and methane: CH₃CHO ⎯⎯→ CH₄ + CO A plot of ln [CH₃CHO] versus time is linear. After 530 s, [CH₃CHO] decreases to one half of its initial value of 0.10 M. What is the rate law for the reaction?

The reaction 2N₂O₅(g) → O₂(g) + 4NO₂(g) Is first order in N₂O₅. For this reaction at 45° C, the rate constant k = 1.0 × 10^-5 s^-1, where the rate law is defined as Rate For a particular experiment ([N₂O₅]₀ = 1.0 × 10^-3 M) , calculate [N₂O₅] after 1.0 × 10⁵ s.

Consider the reaction 3A + B + C → D + E where the rate law is defined as k[A]²[B][C] An experiment is carried out where [B]₀ = [C]₀ = 1.00 M and [A]₀ = 1.00 × 10^-4 M. -What is the concentration of A after 10.0 min?

The reaction 3NO → N₂O + NO₂ Is found to obey the rate law Rate = k[NO]². If the first half-life of the reaction is found to be 3.5 s, what is the length of the fourth half-life?

The following questions refer to the gas-phase decomposition of chloroethane:C₂H₅Cl → products Experiment shows that the decomposition is first order. The following data show kinetics information for this reaction. -What was the initial concentration of the ethylene chloride?

Consider the reaction 3A + B + C → D + E where the rate law is defined as k[A]²[B][C] An experiment is carried out where [B]₀ = [C]₀ = 1.00 M and [A]₀ = 1.00 × 10^-4 M. -What is the concentration of C after 10.0 min?

The following questions refer to the gas-phase decomposition of chloroethane:C₂H₅Cl → products Experiment shows that the decomposition is first order. The following data show kinetics information for this reaction. -What would the concentration be after 5.0 s?

The following questions refer to the gas-phase decomposition of chloroethane:C₂H₅Cl → products Experiment shows that the decomposition is first order. The following data show kinetics information for this reaction. -What is the time to half-life?

The following data were collected for the decay of HO₂ radicals. Which of the following statements is true?

In 6 M HCl, the complex ion Ru(NH₃) ₆³⁺ decomposes to a variety of products. The reaction is first order in Ru(NH₃) ₆³⁺ and has a half-life of 14 h at 25°C. Under these conditions, how long will it take for the [Ru(NH₃) ₆³⁺] to decrease to 39.0% of its initial value?

Consider the second-order reaction aA → products (which has a first half-life of 25 s) . If the concentration of A after 15.6s is 0.36M, determine the initial concentration of A.

At a particular temperature, N₂O₅ decomposes according to a first-order rate law with a half-life of 3.0 s. If the initial concentration of N₂O₅ is 1.0 × 10¹⁶ molecules/cm³, what will be the concentration in molecules/cm³ after 10.0 s?

The reaction A → B + C is known to be zero order in A with a rate constant of 4.8 × 10^-2 mol/L • s at 25° C. An experiment was run at 25°C where [A]₀ = 2.0M. What is the concentration of B after 4.0s?

The reaction 2NO₂ → 2NO + O₂ obeys the rate law 1.40 × 10^-2 [NO₂]² at 500° K.If the initial concentration of NO₂ is 1.00 M, how long will it take for the [NO₂] to decrease to 25.0% of its initial value?

Consider the reaction 3A + B + C → D + E Where the rate law is defined as (1.96× 10² L³/mol³ • s) [A]²[B][C] An experiment is carried out where [B]₀ = [C]₀ = 1.00 M and [A]₀ = 2.80 × 10^-4 M. What is the half-life for this experiment?

At a particular temperature, the half-life of a zero-order reaction is 29.0min. How long will it take for the reactant concentration to be depleted by a factor of 8?

Calculate the value of k₂ where Rate = K₂[B]²

Quiz 15: Chemical Kinetics

Consider the reaction 3A + B + C → D + E Where the rate law is defined as An experiment is carried out where [B]0 = [C]0 = 1.00 M and [A]0 = 2.46× 10-4 M. After 2.96 min, [A] = 3.20× 10-5 M. What is the value of k?

At 760 K, acetaldehyde decomposes to carbon monoxide and methane: CH3CHO ⎯⎯→ CH4 + CO A plot of ln [CH3CHO] versus time is linear. After 530 s, [CH3CHO] decreases to one half of its initial value of 0.10 M. What is the rate law for the reaction?

The reaction 2N2O5(g) → O2(g) + 4NO2(g) Is first order in N2O5. For this reaction at 45° C, the rate constant k = 1.0 × 10-5 s-1, where the rate law is defined as Rate For a particular experiment ([N2O5]0 = 1.0 × 10-3 M) , calculate [N2O5] after 1.0 × 105 s.

Consider the reaction 3A + B + C → D + E where the rate law is defined as k[A]2[B][C] An experiment is carried out where [B]0 = [C]0 = 1.00 M and [A]0 = 1.00 × 10-4 M. -What is the concentration of A after 10.0 min?

The reaction 3NO → N2O + NO2 Is found to obey the rate law Rate = k[NO]2. If the first half-life of the reaction is found to be 3.5 s, what is the length of the fourth half-life?

The following questions refer to the gas-phase decomposition of chloroethane:C2H5Cl → products Experiment shows that the decomposition is first order. The following data show kinetics information for this reaction. -What was the initial concentration of the ethylene chloride?

Consider the reaction 3A + B + C → D + E where the rate law is defined as k[A]2[B][C] An experiment is carried out where [B]0 = [C]0 = 1.00 M and [A]0 = 1.00 × 10-4 M. -What is the concentration of C after 10.0 min?

The following questions refer to the gas-phase decomposition of chloroethane:C2H5Cl → products Experiment shows that the decomposition is first order. The following data show kinetics information for this reaction. -What would the concentration be after 5.0 s?

The following questions refer to the gas-phase decomposition of chloroethane:C2H5Cl → products Experiment shows that the decomposition is first order. The following data show kinetics information for this reaction. -What is the time to half-life?

The following data were collected for the decay of HO2 radicals. Which of the following statements is true?

In 6 M HCl, the complex ion Ru(NH3) 63+ decomposes to a variety of products. The reaction is first order in Ru(NH3) 63+ and has a half-life of 14 h at 25°C. Under these conditions, how long will it take for the [Ru(NH3) 63+] to decrease to 39.0% of its initial value?

Consider the second-order reaction aA → products (which has a first half-life of 25 s) . If the concentration of A after 15.6s is 0.36M, determine the initial concentration of A.

At a particular temperature, N2O5 decomposes according to a first-order rate law with a half-life of 3.0 s. If the initial concentration of N2O5 is 1.0 × 1016 molecules/cm3, what will be the concentration in molecules/cm3 after 10.0 s?

The reaction A → B + C is known to be zero order in A with a rate constant of 4.8 × 10-2 mol/L • s at 25° C. An experiment was run at 25°C where [A]0 = 2.0M. What is the concentration of B after 4.0s?

The reaction 2NO2 → 2NO + O2 obeys the rate law 1.40 × 10-2 [NO2]2 at 500° K.If the initial concentration of NO2 is 1.00 M, how long will it take for the [NO2] to decrease to 25.0% of its initial value?

Consider the reaction 3A + B + C → D + E Where the rate law is defined as (1.96× 102 L3/mol3 • s) [A]2[B][C] An experiment is carried out where [B]0 = [C]0 = 1.00 M and [A]0 = 2.80 × 10-4 M. What is the half-life for this experiment?

At a particular temperature, the half-life of a zero-order reaction is 29.0min. How long will it take for the reactant concentration to be depleted by a factor of 8?

Calculate the value of k2 where Rate = K2[B]2

Consider the reaction 3A + B + C → D + E Where the rate law is defined as An experiment is carried out where [B]₀ = [C]₀ = 1.00 M and [A]₀ = 2.46× 10^-4 M. After 2.96 min, [A] = 3.20× 10^-5 M. What is the value of k?

At 760 K, acetaldehyde decomposes to carbon monoxide and methane: CH₃CHO ⎯⎯→ CH₄ + CO A plot of ln [CH₃CHO] versus time is linear. After 530 s, [CH₃CHO] decreases to one half of its initial value of 0.10 M. What is the rate law for the reaction?

The reaction 2N₂O₅(g) → O₂(g) + 4NO₂(g) Is first order in N₂O₅. For this reaction at 45° C, the rate constant k = 1.0 × 10^-5 s^-1, where the rate law is defined as Rate For a particular experiment ([N₂O₅]₀ = 1.0 × 10^-3 M) , calculate [N₂O₅] after 1.0 × 10⁵ s.

Consider the reaction 3A + B + C → D + E where the rate law is defined as k[A]²[B][C] An experiment is carried out where [B]₀ = [C]₀ = 1.00 M and [A]₀ = 1.00 × 10^-4 M. -What is the concentration of A after 10.0 min?

The reaction 3NO → N₂O + NO₂ Is found to obey the rate law Rate = k[NO]². If the first half-life of the reaction is found to be 3.5 s, what is the length of the fourth half-life?

The following questions refer to the gas-phase decomposition of chloroethane:C₂H₅Cl → products Experiment shows that the decomposition is first order. The following data show kinetics information for this reaction. -What was the initial concentration of the ethylene chloride?

Consider the reaction 3A + B + C → D + E where the rate law is defined as k[A]²[B][C] An experiment is carried out where [B]₀ = [C]₀ = 1.00 M and [A]₀ = 1.00 × 10^-4 M. -What is the concentration of C after 10.0 min?

The following questions refer to the gas-phase decomposition of chloroethane:C₂H₅Cl → products Experiment shows that the decomposition is first order. The following data show kinetics information for this reaction. -What would the concentration be after 5.0 s?

The following questions refer to the gas-phase decomposition of chloroethane:C₂H₅Cl → products Experiment shows that the decomposition is first order. The following data show kinetics information for this reaction. -What is the time to half-life?

The following data were collected for the decay of HO₂ radicals. Which of the following statements is true?

In 6 M HCl, the complex ion Ru(NH₃) ₆³⁺ decomposes to a variety of products. The reaction is first order in Ru(NH₃) ₆³⁺ and has a half-life of 14 h at 25°C. Under these conditions, how long will it take for the [Ru(NH₃) ₆³⁺] to decrease to 39.0% of its initial value?

At a particular temperature, N₂O₅ decomposes according to a first-order rate law with a half-life of 3.0 s. If the initial concentration of N₂O₅ is 1.0 × 10¹⁶ molecules/cm³, what will be the concentration in molecules/cm³ after 10.0 s?

The reaction A → B + C is known to be zero order in A with a rate constant of 4.8 × 10^-2 mol/L • s at 25° C. An experiment was run at 25°C where [A]₀ = 2.0M. What is the concentration of B after 4.0s?

The reaction 2NO₂ → 2NO + O₂ obeys the rate law 1.40 × 10^-2 [NO₂]² at 500° K.If the initial concentration of NO₂ is 1.00 M, how long will it take for the [NO₂] to decrease to 25.0% of its initial value?

Consider the reaction 3A + B + C → D + E Where the rate law is defined as (1.96× 10² L³/mol³ • s) [A]²[B][C] An experiment is carried out where [B]₀ = [C]₀ = 1.00 M and [A]₀ = 2.80 × 10^-4 M. What is the half-life for this experiment?

Calculate the value of k₂ where Rate = K₂[B]²