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Exam 14: Chemical Kinetics

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Question 61

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The rate constant for a first-order decomposition reaction is 0.0111 min^-1. What is the half-life of the reaction?

A) 111 min
B) 62.4 min
C) 5000 sec
D) 31.25 min
E) 27.1 min

F) C) and E)
G) A) and D)

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Question 62

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For the reaction, 2M + 2N $\rarr$ 2P + Q, studies on how the initial rate of the reaction varied with concentration were carried out. Some data is given below.

A) the rate law is therefore: rate = k[N]²
B) the rate law is therefore: rate = k[M][N]²
C) the rate law is therefore: rate = k[M][N]
D) the rate law is therefore: rate = k[M]²
E) the rate law is therefore: rate = k[M]²[N]²

F) All of the above
G) A) and D)

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Question 63

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The data shown below was determined for the reaction A + B $\rarr$ Products.What is the missing value in the table, for the initial rate of the reaction in Experiment 5?

Describe, in words, the effects of a catalyst on a chemical reaction.

The fact that granulated sugar dissolves faster than a sugar cube of the same mass can best be explained by which of the following statements?

An isomerization reaction of a substance, A, is first order. In a laboratory class, one student group found that 28.5% of A had isomerized after a period of 15.0 minutes, when the temperature was maintained at 84.5 °C. What is the half-life of substance A at that temperature?

The fastest step in a multistep reaction mechanism is the net reaction.

The reaction A + 2B → products was found to follow the rate law, rate = k[A]²[B]. The rate of reaction will increase by a factor of ________ when the concentration of A is tripled, the concentration of B is doubled, and the temperature remains constant.

The step in a multistep reaction mechanism that has the highest activation energy is the rate-determining step.

If a reaction was found to be 4^th order overall, what would be the units for the rate constant, in terms of M and s?

For the reaction A + B → products, the rate law was determined experimentally to be:Rate = k[B]²Using this information, could the reaction happen in a single step, or would it require multiple steps? Explain.

The half-life of a first order chemical reaction is 24.0 minutes at 55.0^°C and 16.4 minutes at 63.5°C. What will be the half-life, in minutes, at 70.0°C?________Hint: Use the given information to solve for activation energy, then find the missing equilibrium constant. Remember t_1/2 = .

The average reaction rate over a time period in graph b can be found by

Concentration vs. time data for a first-order reaction is shown in the graph below. What should be done to determine the half-life of the reaction?

The activation energy is the energy required to initiate a reaction, and the reaction will continue without additional outside energy.

The initial concentration of a reactant in a first order reaction is 0.620 M. What will be its concentration after 3 half-lives?

Given the reaction, aA + bB $\rarr$ dD + eE If we try rate = k[A]^q[B]^r for a generic rate law statement, which one of the statements below is false?

The decomposition of ozone to oxygen has the following proposed mechanism: What is the rate determining step?

Heterogeneous catalysis often takes place at transition metal surfaces. Which would be a better choice for a catalyst-a gold sphere with a radius of 18Å, or 15 gold spheres, each with a radius of 5 Å?Hint: The surface area of a sphere is given by: A = 4πr^2.

The decomposition of a compound is known to be a first-order reaction. If the half-life of the reaction is 6.25 minutes at 65 °C, what is the value of the rate constant for the reaction at this temperature?