Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Transcribed Image Text:True or False. If false, correct to make a true statement.
1. The rate constant for a reaction which follows 2nd order kinetics does not depend on
concentration.
2. The half life of a reaction (for the cases we've studied) is always inversely
proportional to the rate constant.
3. If graphed over time, the concentration of a reactant will be linear for a reaction
which follows first order kinetics.
4. A reaction with a constant half-life of 25 seconds is being studied. There is only one
reactant with an initial concentration of 0.800 M. After 75 seconds, the molarity is
found to be 0.200 M.
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- A particular reactant decomposes with a half‑life of 153 s when its initial concentration is 0.360 M. The same reactant decomposes with a half‑life of 231 s when its initial concentration is 0.238 M. Determine the reaction order. 2 1 0 What is the value and units of the rate constant for this reaction? K= ???arrow_forwardA particular reaction is proposed to be first order. What plot would support this conclusion? a. a linear plot of [reactant] versus time b. an exponential decay of [reactant] versus time c. a linear plot of ln [reactant] versus time d. an exponential decay of ln [reactant] versus timearrow_forwardWrite true if the statement is true, otherwise change the underlined word to make the statement true. 1. Metal A has a higher specific heat than metal B. If the two metals are independently applied with equal heat, it is expected that metal A will have a higher change in temperature. 2. The units for the rate constant of an over-all 1st order reaction is s', when the reaction time is measured in seconds. 3. If K is much greater than 1 (that is, K>>1), the equilibrium will favor the formation of reactants. 4. In the iron-thiocyanate system, increasing the pH would produce a dark orange solution. 5. For a weak acid HA, the equilibrium concentration of H3O* is equal to [HA]i. 6. The buffer region is the pH range where a buffer effectively neutralizes added acids and bases, while maintaining a relatively constant pH. A buffer can be expressed by the Henderson-Hasselbaich equation. 7. 8. Diluting a concentrated weak base, results to an increase in pH. 9. The plot of absorbance versus…arrow_forward
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