Question

a.)For the gas phase decomposition of hydrogen iodide at 700 K

2 HI---->H2 + I2

the following data have been obtained: [HI], M 0.530 0.187 0.114 8.16×10-2 time, s 0 48.0 96.0 144 The average rate of disappearance of HI over the time period from t = 48.0 s to t = 96.0 s is M s-1.

b.)For the gas phase decomposition of phosphine at 120 °C

4 PH3(g)----->P4(g) + 6 H2(g)

the following data have been obtained: [PH3], M 8.04×10-2 4.69×10-2 2.73×10-2 1.59×10-2 time, s 0 30.0 60.0 90.0 The average rate of disappearance of PH3 over the time period from t = 60.0 s to t = 90.0 s is M s-1.

Answer #1

The decomposition of hydrogen iodide in the gas phase goes as
follows at 600 K. 2 HI (g)->H2 (g) + I2 (g) Rate = k[HI]2 k =
9.7x10-6 M-1 s -1
a) Starting with an HI concentration of 0.030 M, what is the
concentration of HI after 6.00 days?
b) What is the concentration of H2 in the flask after 6.00
days?
c) How much time would it take to drop the concentration from
0.030 M to 0.025 M?
d)...

The gas-phase decomposition of HI HI (g) → ½ H2 (g) + ½ I2 (g)
has k = 30. L/mol⋅min at 443°C. What is the concentration after 3.3
minutes if the initial concentration of HI was 0.010 M? Write the
rate law for the reaction.

The decomposition of HI (g) into its elements in the gas phase
at 800 K is found to proceed by a second order process.
A) Please write a balanced equation for the reaction (smallest
integer ratio of coefficients, please).
B) Please write the rate law for the reaction:
C) Given that it takes 142 s for the [HI (g)] to change from 6.75 x
10-2 M to 3.50 x 10-2 M, please calculate the value of the rate
constant (and...

In a study of the gas phase decomposition of hydrogen
peroxide at 400 °C
H2O2(g)H2O(g)
+ ½ O2(g)
the following data were obtained:
[H2O2], M
0.133
6.65×10-2
3.33×10-2
1.67×10-2
seconds
0
16.1
48.2
112
Hint: It is not necessary to graph these
data.
(1)
The observed half life for this reaction when the starting
concentration is 0.133 M is s and
when the starting concentration is
6.65×10-2 M is
s.
(2)
The average (1/[H2O2]) / t
from t = 0...

Hydrogen iodide undergoes decomposition according to the
equation 2HI(g) H2(g) + I2(g) The equilibrium constant Kp at 500 K
for this equilibrium is 0.060. Suppose 0.898 mol of HI is placed in
a 1.00-L container at 500 K. What is the equilibrium concentration
of H2(g)?
(R = 0.0821 L · atm/(K · mol))
A. 7.3 M
B. 0.40 M
C. 0.15 M
D. 0.18 M
E. 0.043 M

Hydrogen iodide decomposes slowly to H2 and I2 at 600 K. The
reaction is second order in HI and the rate constant is 9.7×10^−6
M^−1s^−1. If the initial concentration of HI is 0.130 M...
What is its molarity after a reaction time of 7.00 days?
What is the time (in days) when the HI concentration reaches a
value of 7.5×10^−2 M ?

1) The gas phase decomposition of dinitrogen pentoxide at 335
K
N2O5(g) 2
NO2(g) + ½ O2(g)
is first order in
N2O5 with a rate constant of
4.70×10-3
s-1.
If the initial concentration of
N2O5 is
0.105 M, the concentration of
N2O5 will
be Mafter 391 s have
passed.
2) The gas phase decomposition of dinitrogen pentoxide at 335
K
N2O5(g)2
NO2(g) + ½ O2(g)
is first order in
N2O5 with a rate constant of
4.70×10-3
s-1.
If the initial concentration of...

Hydrogen iodide decomposes according to the following reaction.
2 HI(g) equilibrium reaction arrow H2(g) + I2(g) A sealed 1.5 L
container initially holds 0.00615 mol H2, 0.00445 mol I2, and
0.0163 mol HI at 703 K. When equilibrium is reached, the
equilibrium concentration of H2(g) is 0.00364 M. What are the
equilibrium concentrations of HI(g) and I2(g)?

Consider the following reaction: H2 (g) + I2 (g) ⇌ 2 HI (g)
Complete the following table. Assume that all concentrations are
equilibrium concentrations in M.
T(∘C)
[H2]
[I2]
[HI]
[Kc]
25
0.0355
0.0388
0.922
−
340
−
4.50×10−2 M
0.394 M
9.6
445
4.90×10−2 M
4.76×10−2 M
−
50.2
Find [H2] at 340 ∘C.
Find [HI] at 445 ∘C.

Hydrogen iodide decomposes slowly to H2 and I2 at 600 K. The
reaction is second order in HI and the rate constant is
9.7×10−6M−1s−1. If the initial concentration of HI is 0.100 M .
What is its molarity after a reaction time of 5.00 days?

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