Question 1

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

Accepted Answer

The answer of Given the following balanced equation,determine the rate...

Question 2

Identify an heterogeneous catalyst.

Accepted Answer

Pd in H₂ gas is an example of a heterogeneous catalyst because the Pd is a solid and the reactants (probably gases) are present in the gas phase. The other choices involve either a homogeneous catalyst (KI dissolved in solution) or a chemical reaction without a catalyst (CFCs with ozone, HCl with organic solvent, alcohol with an organic compound).

Question 3

If the activation energy for a given compound is found to be 42.0 kJ/mol,with a frequency factor of 8.0 × 10¹⁰ s^-1,what is the rate constant for this reaction at 298 K?

Accepted Answer

The rate constant can be calculated using the Arrhenius equation:

k = Ae^(-Ea/RT)

where k is the rate constant, A is the frequency factor, Ea is the activation energy, R is the gas constant (8.314 J/mol*K), and T is the temperature in Kelvin.

Plugging in the values given:

k = (8.0 × 10^13 s^-1) * e^(-42000 J/mol / (8.314 J/mol*K * 298 K))

k = 3.5 × 10^-13 s^-1

Therefore, the best choice is E.

Question 4

Which rate law has a molecularity of three?

Accepted Answer

The molecularity of a reaction refers to the number of particles involved in the rate-determining step of the reaction. In the given rate law, option B has a molecularity of three as it involves the concentration of two molecules (A and B) and the power of the concentration of the products. All other options have a molecularity of one or two.

Question 5

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

Accepted Answer

Enzymes are biological catalysts that increase the rates of biochemical reactions, by lowering the activation energy needed for reactions to occur. Substrates are the molecules that enzymes act on, while inhibitors are molecules that decrease enzyme activity. "Binders" and "trumanettes" are not commonly used terms in biochemistry or biology.

Question 6

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

Accepted Answer

The rate constant (k) can be calculated using the Arrhenius equation: $k = A \exp\left(-\frac{E_a}{RT}\right)$, where $A$ is the frequency factor, $E_a$ is the activation energy in J/mol (103 kJ/mol = 103,000 J/mol), $R$ is the gas constant (8.314 J/mol·K), and $T$ is the temperature in Kelvin (398 K). Plugging in the values: $k = 4.0 \times 10^{13} \exp\left(-\frac{103,000}{8.314 \times 398}\right)$, which calculates to approximately 1.2 s^-1, making option A correct.

Question 7

In the hydrogenation of double bonds,a catalyst is needed.In the third step,the reactants react to form the product.This step is known as

Accepted Answer

The third step, where the reactants react to form the product, is known as the reaction step. The other options - adsorption, diffusion, and desorption - are steps that may occur before or after the reaction step but are not the actual reaction itself.

Question 8

A reaction is followed and found to have a rate constant of 3.36 × 10⁴ M^-1s^-1 at 344 K and a rate constant of 7.69 M^-1s^-1 at 219 K.Determine the activation energy for this reaction.

Accepted Answer

Using the Arrhenius equation, we have:

ln(k2/k1) = (Ea/R)(1/T1 - 1/T2)

where k1 and T1 are the rate constant and temperature at the first condition, and k2 and T2 are the rate constant and temperature at the second condition.

Substituting the given values and solving for Ea, we obtain:

Ea = (ln(k2/k1))/(1/T1 - 1/T2) x R

= [(ln 7.69 - ln 3.36) / (1/219 - 1/344)] x 8.314 J/mol/K

= 42.0 kJ/mol

Therefore, the activation energy for this reaction is 42.0 kJ/mol, which corresponds to choice B.

Question 9

In the hydrogenation of double bonds,a catalyst is needed.In the first step,the reactants must come into contact with a metal surface.This step is known as

Accepted Answer

In the first step of the hydrogenation of double bonds, the reactants must come into contact with a metal surface, which is known as adsorption. Adsorption is the process by which atoms or molecules adhere to the surface of a solid or liquid. This step is important because it brings the reactants into close proximity with the hydrogen atoms on the metal surface, which is necessary for the reaction to occur.

Question 10

Which rate law has a molecularity of one?

Accepted Answer

A rate law with a molecularity of one only involves one reactant, and therefore only one concentration term in the rate law. The only option with one concentration term is D, which has a rate law of only k[A].

Question 11

In the hydrogenation of double bonds,a catalyst is needed.In the second step,the reactants diffuse on the surface until they approach each other.This step is known as

Accepted Answer

The step where the reactants diffuse on the surface until they approach each other is known as diffusion. This is the second step in the hydrogenation of double bonds, after the initial adsorption of the reactants onto the catalyst surface. The other options (adsorption, reaction, desorption) do not accurately describe this specific step in the process.

Question 12

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

Accepted Answer

Desorption is the process of molecules leaving a surface and returning to the gas phase. In the hydrogenation of double bonds, the reactants (such as hydrogen) must desorb from the catalyst surface to complete the reaction. Therefore, the correct answer is D) desorption.

Question 13

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

Accepted Answer

The rate of reaction with respect to [SO₂] would be the rate at which the concentration of SO₂ changes during the reaction. In the balanced equation, we can see that 2 molecules of SO₂ react to form 2 molecules of SO₃. Therefore, the rate of reaction with respect to [SO₂] would be negative, as the concentration of SO₂ decreases during the reaction. The correct answer is A, which gives the negative sign in the rate expression.

Question 14

A reaction is found to have an activation energy of 108 kJ/mol.If the rate constant for this reaction is 4.60 × 10^-6s^-1 at 275 K,what is the rate constant at 366 K?

Accepted Answer

We can use the Arrhenius equation to relate the rate constants at two temperatures:

k2 = A * exp(-Ea/R * (1/T2 - 1/T1))

where k1 and T1 are given, Ea is the activation energy (108 kJ/mol), R is the gas constant (8.31 J/mol*K), and T2 is the new temperature (366 K).

Plugging in the values, we get:

k2 = (4.60 × 10^-6) * exp(-108000/(8.31 * 366) * (1/366 - 1/275))

k2 = 0.58 s^-1

Therefore, the answer is C, 0.58 s^-1.

Question 15

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

Accepted Answer

The answer of Given the following balanced equation,determine the rate...

Question 16

Which of the following statements is TRUE?

Accepted Answer

The rate constant is influenced by temperature through the Arrhenius equation, which states that k=Ae^(-Ea/RT), where k is the rate constant, Ea is the activation energy, R is the gas constant, T is the temperature in Kelvin, and A is the pre-exponential factor. Thus, as temperature increases, the rate constant also increases. A, B, and D are all false statements.

Question 17

Which rate law has a molecularity of three?

Accepted Answer

The rate law is of molecularity three because it contains the concentrations of three different reactants, [A], [B], and [C]. Molecularity refers to the number of molecules or ions participating in the rate-determining step of a reaction. In this case, the rate-determining step involves the collision of three molecules or ions, hence the molecularity of 3.

Question 18

Which rate law is unimolecular?

Accepted Answer

A unimolecular rate law has only one reactant in the rate determining step, and its rate is proportional to the concentration of that reactant raised to the first power. In this case, option D is the only rate law that has only one reactant (A) and its rate is proportional to [A]1.

Question 19

Which rate law has a molecularity of two?

Accepted Answer

The rate law that has a molecularity of two is one that involves the collision of two molecules. The rate law that meets this criterion is option B, which involves the concentration of two reactant molecules, A and B. A reaction with a molecularity of two is a second-order reaction.

Question 20

A reaction is found to have an activation energy of 38.0 kJ/mol.If the rate constant for this reaction is 1.60 × 10² M^-1s^-1 at 249 K,what is the rate constant at 436 K?

Accepted Answer

The answer of A reaction is found to have an...

Quiz 14: Chemical Kinetics

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

Identify an heterogeneous catalyst.

If the activation energy for a given compound is found to be 42.0 kJ/mol,with a frequency factor of 8.0 × 10¹⁰ s^-1,what is the rate constant for this reaction at 298 K?

Which rate law has a molecularity of three?

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

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

In the hydrogenation of double bonds,a catalyst is needed.In the third step,the reactants react to form the product.This step is known as

A reaction is followed and found to have a rate constant of 3.36 × 10⁴ M^-1s^-1 at 344 K and a rate constant of 7.69 M^-1s^-1 at 219 K.Determine the activation energy for this reaction.

In the hydrogenation of double bonds,a catalyst is needed.In the first step,the reactants must come into contact with a metal surface.This step is known as

Which rate law has a molecularity of one?

In the hydrogenation of double bonds,a catalyst is needed.In the second step,the reactants diffuse on the surface until they approach each other.This step is known as

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

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

A reaction is found to have an activation energy of 108 kJ/mol.If the rate constant for this reaction is 4.60 × 10^-6s^-1 at 275 K,what is the rate constant at 366 K?

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

Which of the following statements is TRUE?

Which rate law has a molecularity of three?

Which rate law is unimolecular?

Which rate law has a molecularity of two?

A reaction is found to have an activation energy of 38.0 kJ/mol.If the rate constant for this reaction is 1.60 × 10² M^-1s^-1 at 249 K,what is the rate constant at 436 K?

Quiz 14: Chemical Kinetics

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

Identify an heterogeneous catalyst.

If the activation energy for a given compound is found to be 42.0 kJ/mol,with a frequency factor of 8.0 × 1010 s-1,what is the rate constant for this reaction at 298 K?

Which rate law has a molecularity of three?

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

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

In the hydrogenation of double bonds,a catalyst is needed.In the third step,the reactants react to form the product.This step is known as

A reaction is followed and found to have a rate constant of 3.36 × 104 M-1s-1 at 344 K and a rate constant of 7.69 M-1s-1 at 219 K.Determine the activation energy for this reaction.

In the hydrogenation of double bonds,a catalyst is needed.In the first step,the reactants must come into contact with a metal surface.This step is known as

Which rate law has a molecularity of one?

In the hydrogenation of double bonds,a catalyst is needed.In the second step,the reactants diffuse on the surface until they approach each other.This step is known as

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

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

A reaction is found to have an activation energy of 108 kJ/mol.If the rate constant for this reaction is 4.60 × 10-6 s-1 at 275 K,what is the rate constant at 366 K?

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

Which of the following statements is TRUE?

Which rate law has a molecularity of three?

Which rate law is unimolecular?

Which rate law has a molecularity of two?

A reaction is found to have an activation energy of 38.0 kJ/mol.If the rate constant for this reaction is 1.60 × 102 M-1s-1 at 249 K,what is the rate constant at 436 K?

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

If the activation energy for a given compound is found to be 42.0 kJ/mol,with a frequency factor of 8.0 × 10¹⁰ s^-1,what is the rate constant for this reaction at 298 K?

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

A reaction is followed and found to have a rate constant of 3.36 × 10⁴ M^-1s^-1 at 344 K and a rate constant of 7.69 M^-1s^-1 at 219 K.Determine the activation energy for this reaction.

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

A reaction is found to have an activation energy of 108 kJ/mol.If the rate constant for this reaction is 4.60 × 10^-6s^-1 at 275 K,what is the rate constant at 366 K?

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

A reaction is found to have an activation energy of 38.0 kJ/mol.If the rate constant for this reaction is 1.60 × 10² M^-1s^-1 at 249 K,what is the rate constant at 436 K?