Question

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?

Answer #1

The reaction of decomposition of HI can be written as follows:

2HI -----> H2 + I2

The reaction is second order in HI. The Integrated second order rate law equation for this reaction can be given as follows:

1/[HI] = 1/[HI]_{o} + kt

Where, [HI] = molarity of HI after time t

[HI]_{o} = initial molarity of HI = 0.100 M

k = rate constant = 9.7×10^{−6}
M^{−1}s^{−1}

t = time = 5.00days = 5.00 x 24 x 60 x 60 seconds = 432,000 seconds

Thus, molarity after 5.00days [HI] can be calculated as follows:

1/[HI] = 1/(0.100 M) +
9.7×10^{−6}M^{−1}s^{−1} x 432,000 s

1/[HI] = 10M^{-1} + 4.2 M^{-1}

1/[HI] = 14.2M^{-1}

[HI] = (1/14.2)M

[HI] = 0.070 M

Thus, molarity of [HI] after five days of reaction will be
**0.070 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 ?

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)?

Hydrogen iodide decomposes according to the equation 2HI
(g)<---> H2 (g) + I2 (g) for which K= .0156 at 400 degrees
celsius. If 0.550 mol of HI was injected into 2.00L reaction vessel
at 400 degrees celsuis. Calculate the concentration of H2 at
equilibrium?

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)...

Kc for the reaction of hydrogen and
iodine to produce hydrogen iodide.
H2(g) + I2(g) ⇌
2HI(g)
is 54.3 at 430°C. Calculate the
equilibrium concentrations of H2,
I2, and HI at 430°C if
the initial concentrations are [H2] =
[I2] = 0 M,
and [HI] = 0.483 M.

Kc for the reaction of hydrogen and iodine to produce hydrogen
iodide. H2(g) + I2(g) ⇌ 2HI(g) is 54.3 at 430 ° C. Calculate the
equilibrium concentrations of H2, I2, and HI at 430 ° C if the
initial concentrations are [H2] = [I2] = 0 M, and [HI] = 0.445
M.

The equation for the formation of hydrogen iodide from
H2 and I2 is:
H2(g) + I2(g) <--> 2HI(g)
The value of Kp for the reaction is 69.0 at 730.0C.
What is the equilibrium partial pressure of HI in a sealed reaction
vessel at 730.0C if the initial partial pressures of H2
and I2 are both 0.1600 atm and initially there is no HI
present?

Hydrogen iodide, HI, decomposes at moderate temperature
according to the equation 2HI (g) H2 (g) + I2 (g) When 4.00 mol HI
was placed in a 5.00-L vessel at 458C, the equilibrium mixture was
found to contain 0.442 mol I2. What is the value of Kc for the
decomposition of HI at this temperature?

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

Be sure to answer all parts.
The rate constant for the gaseous reaction
H2(g) + I2(g)
→2HI(g)
is 2.42 ×10−2/(M·s) at 400°C. Initially an
equimolar sample of H2 and I2 is placed in a
vessel at 400°
C and the total pressure is 1694 mmHg.
(a) What is the initial rate (M/min) of formation of
HI?
_____ (M/min)
(b) What are the rate of formation of HI and the concentration
of HI (in molarity) after 13.6 min?
Rate of formation...

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