consider the following reaction at 25oC
(CH3)3COH +HI ---> (CH3)3Cl + H20
The experimentally determined rate law for this reactionindicates that the reaction is first order in (CH3)3COH and thatthe reation is first order overall. Which of the following wouldproduce 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 thefastes?
4NH3 + 7O2 ----> 4NO2 +6H2O
3. Which of the follwoing is a key reason why chemists generallymeasure the INITIAL reaction rate?
a. one knows the concentration of reactants one puts in the testtubes
b one can ignore the rate of back-reactionfrom products toreactants when studying initial reaction rates as productconcetrations 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 = 2.64x104M-1min-1. If the initial concentration is0.250M, what is the initial rate, with correct units?
5. What will happen when the pressure increase by decreasing thevolume of the system in the reaction
3H2 + N2 <----> 2NH3
consider the following reaction at 25oC
(CH3)3COH +HI ---> (CH3)3Cl + H20
The experimentally determined rate law for this reactionindicates that the reaction is first order in (CH3)3COH and thatthe reation is first order overall. Which of the following wouldproduce 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 thefastes?
4NH3 + 7O2 ----> 4NO2 +6H2O
3. Which of the follwoing is a key reason why chemists generallymeasure the INITIAL reaction rate?
a. one knows the concentration of reactants one puts in the testtubes
b one can ignore the rate of back-reactionfrom products toreactants when studying initial reaction rates as productconcetrations 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 = 2.64x104M-1min-1. If the initial concentration is0.250M, what is the initial rate, with correct units?
5. What will happen when the pressure increase by decreasing thevolume of the system in the reaction
3H2 + N2 <----> 2NH3
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