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the following data were obtained during the first...

Question:
The following data were obtained during the first order thermal decomposition of SO₂Cl₂at a constant volume.

SO₂Cl₂₍g) → SO₂₍g) + Cl₂(g)

Experiment
Time/s^{- 1}
Total pressure/atm

1 0 0.5

2 100 0.6

Calculate the rate of the reaction when total pressure is 0.65 atm.

Answer:

The thermal decomposition of SO₂Cl₂at a constant volume is represented by the following equation.

After time, t, total pressure,P_t = (P_º - p) + p + p

⇒ P_t = (P_º + p)

⇒ p = P_t - P_º

therefore, P_º - p = P_º- P_t - P_º

= 2 P_º- P_t

For a first order reaction,

k = 2.303/t Log P_º/ P_º- p

= 2.303/t Log P_º/ 2 P_º- P_t

When t= 100 s,

k = 2.303 / 100s log 0.5 / 2x0.5 - 0.6

= 2.231 × 10^{- 3}s^{- 1}

When Pt= 0.65 atm,

P₀+ p= 0.65

⇒ p= 0.65 - P₀

= 0.65 - 0.5

= 0.15 atm

Therefore, when the total pressure is 0.65 atm, pressure of SOCl₂ is

p_SOCL2 = P₀ - p

= 0.5 - 0.15

= 0.35 atm

Therefore, the rate of equation, when total pressure is 0.65 atm, is given by,

Rate = k(p_SOCL2)

= (2.23 × 10 ^{- 3}s ^{- 1}) (0.35 atm)

= 7.8 × 10 ^{- 4}atm s^{- 1}

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Question:
The following data were obtained during the first order thermal decomposition of SO₂Cl₂at a constant volume.

SO₂Cl₂₍g) → SO₂₍g) + Cl₂(g)

Experiment
Time/s^{- 1}
Total pressure/atm

1 0 0.5

2 100 0.6

Calculate the rate of the reaction when total pressure is 0.65 atm.

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Question: The following data were obtained during the first order thermal decomposition of SO2Cl2at a constant volume. SO2Cl2(g) → SO2(g) + Cl2(g) Experiment Time/s - 1 Total pressure/atm 1 0 0.5 2 100 0.6 Calculate the rate of the reaction when total pressure is 0.65 atm.

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Question:
The following data were obtained during the first order thermal decomposition of SO₂Cl₂at a constant volume.

SO₂Cl₂₍g) → SO₂₍g) + Cl₂(g)

Experiment
Time/s^{- 1}
Total pressure/atm

1 0 0.5

2 100 0.6

Calculate the rate of the reaction when total pressure is 0.65 atm.