9. A completely hypothetical reaction at a constant temperature has the mechanism shown below. Step 1: A(g) + B(g) C(g) + D(g) (slow) Step 2: C(g) + E(g) → F(g) (fast) Step 3: F(g) + A(g) → G(g) (fast) a) Write the equation for the overall reaction. 2A(g)+B(g)+E(g) → D(g)+G(g) b) Write the rate law for the overall reaction. Rate = k[A][B] c) How will doubling the concentration of A affect the overall reaction rate? Why? The rate law for the reaction is Rate = k[A][B] and therefore, the overall order of the reaction is second. Thus, doubling the concentration will increase the rate by a factor of 4. d) How will doubling the concentration of E affect the overall reaction rate? Why? e) List the intermediate(s). f) A catalyst is discovered which increases the rate of Step 3. How will this affect the rate of the overall reaction? g) A catalyst is discovered which increases the rate of Step 1. How will this affect the rate of the overall reaction?

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9. A completely hypothetical reaction at a constant temperature has the mechanism
shown below.
Step 1:
A(g) + B(g)
C(g) + D(g)
(slow)
Step 2:
C(g) + E(g) → F(g)
(fast)
Step 3:
F(g) + A(g) → G(g)
(fast)
a) Write the equation for the overall reaction.
2A(g)+B(g)+E(g) → D(g)+G(g)
b) Write the rate law for the overall reaction.
Rate = k[A][B]
c) How will doubling the concentration of A affect the overall reaction rate? Why?
The rate law for the reaction is Rate = k[A][B] and therefore, the overall order of the
reaction is second. Thus, doubling the concentration will increase the rate by a factor of
4.
d) How will doubling the concentration of E affect the overall reaction rate? Why?
e) List the intermediate(s).
f) A catalyst is discovered which increases the rate of Step 3. How will this affect
the rate of the overall reaction?
Transcribed Image Text:9. A completely hypothetical reaction at a constant temperature has the mechanism shown below. Step 1: A(g) + B(g) C(g) + D(g) (slow) Step 2: C(g) + E(g) → F(g) (fast) Step 3: F(g) + A(g) → G(g) (fast) a) Write the equation for the overall reaction. 2A(g)+B(g)+E(g) → D(g)+G(g) b) Write the rate law for the overall reaction. Rate = k[A][B] c) How will doubling the concentration of A affect the overall reaction rate? Why? The rate law for the reaction is Rate = k[A][B] and therefore, the overall order of the reaction is second. Thus, doubling the concentration will increase the rate by a factor of 4. d) How will doubling the concentration of E affect the overall reaction rate? Why? e) List the intermediate(s). f) A catalyst is discovered which increases the rate of Step 3. How will this affect the rate of the overall reaction?
g) A catalyst is discovered which increases the rate of Step 1. How will this affect
the rate of the overall reaction?
Transcribed Image Text:g) A catalyst is discovered which increases the rate of Step 1. How will this affect the rate of the overall reaction?
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