AP Chem 5.1

2NO(g) + 2H₂(g) → N₂(g) + 2H₂O(g)

The information in the data table above represents two different trials for an experiment to study the rate of the reaction between NO(g) and H₂(g), as represented by the balanced equation above the table. Which of the following statements provides the correct explanation for why the initial rate of formation of N₂ is greater in trial 2 than in trial 1 ? Assume that each trial is carried out at the same constant temperature.

• The activation energy of the reaction is smaller in trial 2 than it is in trial 1.

• The frequency of collisions between reactant molecules is greater in trial 2 than it is in trial 1.

• The value of the rate constant for the reaction is smaller in trial 2 than it is in trial 1.

• The value of the rate constant for the reaction is greater in trial 2 than it is in trial 1.

Tags

NGSS.HS-PS1-5

Zn(s)+2⁢ HCl(aq)→ZnCl₂(aq)+H₂(g)

Zn(s) reacts with HCl(aq) according to the equation shown above. In trial 1 of a kinetics experiment, a 5.0g piece of Zn(s) is added to 100mL of 0.10MHCl(aq). The rate of reaction between Zn(s) and HCl(aq) is determined by measuring the volume of H2(g) produced over time. In trial 2 of the experiment, 5.0g of powdered Zn(s) is added to 100mL of 0.10MHCl(aq). Which trial will have a faster initial rate of reaction and why?

• Trial 1, because there is a higher concentration of Zn(s) in the reaction mixture.

• Trial 1, because the sample of Zn(s) has less surface area for the reaction to take place.

• Trial 2, because there is a higher concentration of HCl(aq) in the reaction mixture.

• Trial 2, because the sample of Zn(s) has a greater surface area for the reaction to take place.

Tags

NGSS.HS-PS1-5

CH₃I+NaOH→CH₃OH+NaI

The rate of the reaction represented by the chemical equation shown above is expressed as rate=k[CH₃I][NaOH]. Based on this information, which of the following claims is correct?

• The reaction will proceed at a slower rate with increasing temperature.

• The rate of the reaction will double when the concentrations of both CH₃I and NaOH are doubled.

• The rate of the reaction will double if the concentration of CH₃I is doubled while keeping the concentration of NaOH constant.

• A larger amount of CH₃OH will be produced if the concentrations of CH₃I and NaOH are halved.

Tags

NGSS.HS-PS1-5

2N₂O₅(g)→4NO₂(g)+O₂(g)

For the reaction represented by the equation above, the concentration of N₂O₅ was measured over time. The following graphs were created using the data.

Based on the graphs, what is the order of the reaction with respect to N₂O₅ ?

• Zeroth order

• First order

• Second order

• Third order

Tags

NGSS.HS-PS1-5

Bismuth-214 undergoes first-order radioactive decay to polonium-214 by the release of a beta particle, as represented by the nuclear equation above.

Which of the following quantities plotted versus time will produce a straight line?

• [Bi]

• [Po]

• ln[Bi]

• 1/[Bi]

Tags

NGSS.HS-PS1-8

• Rate=k

• Rate=k[NH₃]²

• Rate=k[N₂][H₂]

Tags

NGSS.HS-PS1-5

What would be my the overall order of this rate law? 
Rate=[A]²[B]¹

• 0 Order
• 1st Order
• 2nd Order
• 3rd Order

Given the following balanced equation :

2NO(g) + Cl₂(g) → 2NOCl(g)

If the rate of disappearance of Cl₂ is 4.84 x 10^-2 Ms^-1, what is the rate of disappearance of NO?

• 1.45 x 10^-2 Ms^-1

• 2.42 x 10^-2 Ms^-1

• 3.67 x 10^-2 Ms^-1

• 9.68 x 10^-2 Ms^-1

Tags

NGSS.HS-PS1-5

Consider the following rate law: Rate = k[A]ⁿ[B]^m
How are the exponents n and m determined?

• by using balanced chemical equation
• By using the subscripts for the formulas
• By educated guess
• By experiment 

When you double the concentration of this reactant the rate of the reaction doesn't change.  It is ______ order

• First
• Second
• Zero

Tags

NGSS.HS-PS1-5