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chemistry 2 Test 5
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Terms in this set (19)
Consider the general reaction:
A(g) + 2B(g) →→ C(g)
Which of the following relative rates of change is true?
-deltaB/2deltat= deltaC/deltaT
-deltaA/deltaT=-deltaB/2deltaT
-deltaA/deltaT=deltaC/deltaT
Consider the general reaction:
A(g) + 2B(g) →→ C(g)
If rate of consumption for A is−Δ[A]Δt= -0.1 M s-1 , What is the rate of consumption of B, −Δ[B]Δt?
-0.2 M s-1
For the reaction:
O2(g) + 2NO(g) ⟶⟶ 2NO2(g)
Using the data below, what is the value and units of the rate constant, k?
find m and n by doing initial concentrations over concentrations then initial rate over initial rate and then find the number of powers that go into it. add the powers together then divide 1 from the overall order to get the M
Consider a first order reaction:
A --> B
If the initial concentration of A is 0.75 M and the rate constant, k = 0.556 s-1, how many seconds until it reaches one-half of its original concentration?
.693/0.556=1.25
Consider a second order reaction:
A --> B
If the initial concentration of A is 0.75 M and the rate constant, k = 0.556 M-1 s-1, how many seconds until it reaches one-half of its original concentration?
1/initial concentration (.75) then divide that by 0.556
Consider a zeroth order reaction:
A --> B
If the initial concentration of A is 0.75 M and the rate constant, k = 0.556 M s-1, how many seconds until it reaches one-half of its original concentration?
.75/2(.556)=.67
initial/2(k)
Consider a first order reaction:
A --> B
If the initial concentration of A is 0.75 M and the rate constant, k = 0.951 s-1, how many seconds until it reaches one-third of its original concentration?
1.099/k
Consider a zeroth order reaction:
A --> B
If the initial concentration of A is 0.75 M and the rate constant, k = 0.951 M s-1, how many seconds until it reaches one-third of its original concentration?
2A/3K
Consider a second order reaction:
2A + B ⟶⟶ C
If the rate constant at 300 K is 3.25 x 10-6 M-1 s-1and
the rate constant at 500 K is 1.58 x 10-3 M-1 s-1 . What is the activation energy, Ea?
Ea=-R(ln(k2/k1))/1/t2- 1/t1
plug in numbers
R equals 8.314 but make sure to change it to 8.314*10^-3 if it asks for kJ
Consider a second order reaction:
2A + B ⟶⟶ C
If the rate constant at 600 K is 0.211 M-1 s-1 and the activation energy, Ea , is 77 kJ/mol, what is the rate constant when the temperature is 500∘∘C ?
k2=k1 e^Ea/R(1/t2 - 1/t1)
6.69= (.211)e^(77/8.314*10^-3)(1/600 - 1/773.15)
500+273.15=K
Consider a zeroth order reaction:
A + B ⟶⟶ C
If the rate constant at 350 K is 0.290 M s-1 and the activation energy, Ea , is 2 kJ/mol, at what temperature (in K) would the rate constant be 0.180 M s-1?
1/ ((1/t1 + R*ln(k1/k2))/Ea)
1/ 1/350 + 8.314
10^-3
ln(.290/.180)/2
206.6 or 207
What are the correct units for the rate constant in a second order overall reaction rate?
M-1 S-1
What are the correct units for the rate constant in a zeroth order overall reaction rate?
M S-1
What are the correct units for the rate constant in a first order overall reaction rate?
s-1
Consider a second order reaction:
A --> B
If the initial concentration of A is 0.5 M and the rate constant, k = 0.422 M-1 s-1, how many seconds until it reaches one-third of its original concentration?
2/ initial * K
2/(.5)(0.422)
Consider the following proposed reaction mechanism:
Ignoring the phases of matter, what is the global equation for the mechanism shown here?
ClO + I > IO + Cl
Consider the following proposed reaction mechanism:
Ignoring water, how many reaction intermediates are present?
H2O, OH, and all other long combinations are intermediates
Which of the following reactions would not be a reasonable elementary step for the reaction?
termolecular are not reasonable
If a catalyst is added to a reversible reaction, what should changes should we expect compared to the non-catalyzed reaction?
Non-equilibrium concentrations will reach equilibrium in less time.
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