Question

The half-life for the first-order decomposition of sulfuryl chloride at 320 °C is 8.75 hours.

SOCl2 (g) → SO2 (g) + Cl2 (g)

a. What is the value of the rate constant k (in hours)?

**b.** What is the pressure of sulfuryl chloride
3.00 hours after the start of the reaction if its initial pressure
is 722 mmHg?

**c.** How long after the start of the reaction
will the pressure of sulfuryl chloride become 125 mmHg?

Answer #1

Sulfuryl chloride undergoes first-order decomposition at 320.ºC
with a half-life of 8.75 h (k = 2.20 × 10-5
s-1).
SO2Cl2(g) → SO2(g) +
Cl2(g)
If the initial pressure of SO2Cl2 is 786
torr and the decomposition occurs in a 1.25-L container, how many
molecules of SO2Cl2 remain after 11.8 h?

The first order reaction, SO2Cl2 --> SO2 + Cl2, has a half
life of 8.75 hours at 593 K.?
How long will it take for the concentration of SO2CL2 to fall to
12.5% of its initial value?

The decomposition of sulfuryl chloride
(SO2Cl2) is a first order process. The rate
constant at 660 K is 4.5 x 10-2s-1.
a) If the initial pressure of sulfuryl chloride is 375 torr,
what is the pressure of the substance after 65 sec?
b) At what time will the pressure of sulfuryl chloride decline
to one tenth of its original value?

The decomposition of sulfuryl chloride (SO2Cl2) is a first-order
process. The rate constant for the decomposition at 660 K is
4.5×10−2s−1.
If we begin with an initial SO2Cl2 pressure of 450 torr , what
is the partial pressure of this substance after 68 s?
At what time will the partial pressure of SO2Cl2 decline to
one-third its initial value?

- As described in Exercise 14.43, the decomposition of sulfuryl
chloride (SO2Cl2) is a first-order process.
The rate constant for the decomposition at 660 K is 4.5 ×
10–2 s–1.
(a) If we begin with an initial
SO2Cl2 pressure of 450 torr, what is the
pressure of this substance after 60 s?
(b) At what time will the pressure of
SO2Cl2 decline to one-tenth its initial
value?

The decomposition of sulfuryl chloride (SO2Cl2) is a first-order
process. The rate constant for the decomposition at 660 K is
4.5

The decomposition of N2O to N2 and O2 is a first-order reaction.
At 730°C the half-life of the reaction is 3.58 × 103 min. If the
initial pressure of N2O is 4.50 atm at 730°C, calculate the total
gas pressure after one half-life. Assume that the volume remains
constant.

Sulfuryl chloride decomposes to sulfur dioxide and chlorine by
the following reaction: SO2Cl2(g) ⇌ SO2(g) + Cl2(g) Kc = 0.045 at
648 K If an initial concentration of 6.76 x 10-2 M SO2Cl2 is
allowed to equilibrate, what is the equilibrium concentration of
Cl2?

The decomposition of chloroform at 504°C is first order with a
half-life of 1570 seconds. What percent of any initial amount of
chloroform remains after 1.25 hours?

The decomposition of N2O to N2 and O2 is a first-order reaction.
At 730°C, the rate constant of the reaction is 1.94 × 10-4 min-1.
If the initial pressure of N2O is 4.70 atm at 730°C, calculate the
total gas pressure after one half-life. Assume that the volume
remains constant.

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