Question

Sulfuryl chloride undergoes first-order decomposition at 320.ºC
with a half-life of 8.75 h (k = 2.20 × 10^{-5}
s^{-1}).

SO_{2}Cl_{2}(g) → SO_{2}(g) +
Cl_{2}(g)

If the initial pressure of SO_{2}Cl_{2} is 786
torr and the decomposition occurs in a 1.25-L container, how many
molecules of SO_{2}Cl_{2} remain after 11.8 h?

Answer #1

K = 2.20 * 10^-5 s-1

looking at the value of the rate constant it is first-order reaction

11.8 hr = 42480 sec

initial pressure = 786 torr

ln(initial pressure / final pressure) = rate constant * time ( in sec)

= ln (786 / final pressure) = 42480 * 2.20 * 10^-5

final pressure = 308.71 torr or 0.4062 atm

moles of SO2Cl2 = Pressure * volume ( in L) / R * temperature

= 0.4062 * 1.25 / 0.082 * 593.15 (320 in Kelvin)

= 0.01044

molecules = avagadro number * moles

= 6.022*10^23 * 0.01044

= 6.287*10^21

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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?

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 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?

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