consider the following reaction at 25 o C (CH3)3COH +HI ---> (CH3)3Cl + H20 The
ID: 835316 • Letter: C
Question
consider the following reaction at 25oC
(CH3)3COH +HI ---> (CH3)3Cl + H20
The experimentally determined rate law for this reaction indicates that the reaction is first order in (CH3)3COH and that the reation is first order overall. Which of the following would produce an increase in the rate of this reaction?
. a. decrease concentration of HI
b. increase concentratin of HI
c. increase concetration of (CH3)3COH
d. decrease the concentration of (CH3)Cl
e. it is impossible ot tell
2. which of these substances either appears or disappears the fastes?
4NH3 + 7O2 ----> 4NO2 +6H2O
3. Which of the follwoing is a key reason why chemists generally measure the INITIAL reaction rate?
a. one knows the concentration of reactants one puts in the test tubes
b one can ignore the rate of back-reactionfrom products to reactants when studying initial reaction rates as product concetrations are zero
c. all of the above are reasons to measure the initial rate
d. none of the above are reasons to measure the initial rate
4. the rate law for a given reaction is rate = k[reactant]2 , with k = 2.64x104 M-1min-1. If the initial concentration is 0.250M, what is the initial rate, with correct units?
5. What will happen when the pressure increase by decreasing the volume of the system in the reaction
3H2 + N2 <----> 2NH3
Explanation / Answer
consider the following reaction at 25oC
(CH3)3COH +HI ---> (CH3)3Cl + H20
1.)
The experimentally determined rate law for this reaction indicates that the reaction is first order in (CH3)3COH and that the reation is first order overall. Which of the following would produce an increase in the rate of this reaction?
. a. decrease concentration of HI
b. increase concentratin of HI
c. increase concetration of (CH3)3COH
d. decrease the concentration of (CH3)Cl
e. it is impossible ot tell
2. which of these substances either appears or disappears the fastes?
4NH3 + 7O2 ----> 4NO2 +6H2O
Answer = O2 (maximum no of moles in balanced equation)
3. Which of the follwoing is a key reason why chemists generally measure the INITIAL reaction rate?
a. one knows the concentration of reactants one puts in the test tubes
b one can ignore the rate of back-reactionfrom products to reactants when studying initial reaction rates as product concetrations are zero
c. all of the above are reasons to measure the initial rate
d. none of the above are reasons to measure the initial rate
4. the rate law for a given reaction is rate = k[reactant]2 , with k = 2.64x104 M-1min-1. If the initial concentration is 0.250M, what is the initial rate, with correct units?
rate = k[reactant]2 = 2.64x104 * 0.250 * 0.250 = 0.165 x104 = 1.65 x103 M min-1
5. What will happen when the pressure increase by decreasing the volume of the system in the reaction
3H2 + N 2 <----> 2NH3
(total 4 moles of gas) ( 2 moles of gas)
When volume is decreased or pressure is increased, equilibruim tries to occupy less volume , so less no of moles, so the equilbrium will shift in forward direction in reaction, more NH3 will be produced.
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