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Worksheets10-1 Chemical Kinetics
Total questions: 17
Worksheet time: 9mins
Which sample of HCl(aq) reacts at the fastest rate with a 1.0-gram sample of iron filings?
10 mL of 1 M HCl(aq) at 10°C
10 mL of 1 M HCl(aq) at 25°C
10 mL of 3 M HCl(aq) at 10°C
10 mL of 3 M HCl(aq) at 25°C
During a laboratory activity to investigate reaction rate, a student reacts 1.0-gram samples of solid zinc with 10.0-milliliter samples of HCl(aq). The table below shows information about the variables in five experiments the student performed. Which two experiments can be used to investigate the effect of the concentration of HCl(aq) on the reaction rate?
1 and 3
1 and 5
4 and 2
4 and 3
For a given chemical reaction, the addition of a catalyst provides a different reaction pathway that
decreases the reaction rate and has a higher activation energy
decreases the reaction rate and has a lower activation energy
increases the reaction rate and has a higher activation energy
increases the reaction rate and has a lower activation energy
Each of four test tubes contains a different concentration of HCl(aq) at 25°C. A 1-gram cube of Zn is added to each test tube. In which test tube is the reaction occurring at the fastest rate?
1
2
3
4
A 5.0-gram sample of zinc and a 50.-milliliter sample of hydrochloric acid are used in a chemical reaction. Which combination of these samples has the fastest reaction rate?
a zinc strip and 1.0 M HCl(aq)
a zinc strip and 3.0 M HCl(aq)
zinc powder and 1.0 M HCl(aq)
zinc powder and 3.0 M HCl(aq)
Adding a catalyst to a chemical reaction results in
a decrease in activation energy and a decrease in the reaction rate
a decrease in activation energy and an increase in the reaction rate
an increase in activation energy and a decrease in the reaction rate
an increase in activation energy and an increase in the reaction rate
Which conditions will increase the rate of a chemical reaction?
decreased temperature and decreased concentration of reactants
decreased temperature and increased concentration of reactants
increased temperature and decreased concentration of reactants
increased temperature and increased concentration of reactants
Given the reaction at equilibrium: N2(g) + 3H2(g) ⇌ 2NH3(g). Increasing the concentration of N2(g) will increase the forward reaction rate due to
an increase in the number of effective collisions
a decrease in the number of effective collisions
a decrease in the activation energy
an increase in the activation energy
A 1-cubic-centimeter cube of sodium reacts more rapidly in water at 25°C than does a 1-cubic-centimeter cube of calcium at 25°C. The difference in rate of reaction is most closely associated with the different
surface area of the metal cubes
nature of the metals
density of the metals
concentration of the metals
A chemical reaction occurs when reactant particles
are separated by great distances
have no attractive forces between them
collide with proper energy and proper orientation
convert chemical energy into nuclear energy
A reaction is most likely to occur when the colliding particles have proper orientation and
mass
volume
half-life
energy
An effective collision between reactant particles requires the particles to have the proper
charge and mass
charge and orientation
energy and mass
energy and orientation
What is required for a chemical reaction to occur?
standard temperature and pressure
a catalyst added to the reaction system
effective collisions between reactant particles
an equal number of moles of reactants and products
A chemical reaction between iron atoms and oxygen molecules can only occur if
the particles are heated
the atmospheric pressure decreases
there is a catalyst present
there are effective collisions between the particles
As the concentration of reacting particles increases, the rate of reaction generally
decreases
increases
remains the same
Increasing the temperature increases the rate of a reaction by
lowering the activation energy
increasing the activation energy
lowering the frequency of effective collisions between reacting molecules
increasing the frequency of effective collisions between reacting molecules
Given the balanced equation representing a reaction:
2HCl(aq) + Na2S2O3(aq) → S(s) + H2SO3(aq) + 2NaCl(aq)
Decreasing the concentration of Na2S2O3(aq) decreases the rate of reaction because the:
activation energy decreases
activation energy increases
frequency of effective collisions decreases
frequency of effective collisions increases
