Question

For the reaction Alg) -
be
B(g) + C(g), if initial pressure of Ais 200 mm of Hg and total pressure at equilibrium is 300 mm of Hg the value of
050 mm of Hg
O 100 mm of Hg
0 150 mm of Hg
o 300 mm of Hg​

Answer 1

Answer:

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Answer 2

Complete question : In the following gaseous phase first order reaction

A(g) → B(g) + C(g)

Initial pressure was observed to be 200 mmHg and after 20 minutes, it changed to 300 mmHg. The rate constant for the reaction is

1) 0.035 min⁻¹

2) 0.055 min⁻¹

3) 0.693 min⁻¹

4) 0.115 min⁻¹

Given :

Equation : A(g) → B(g) + C(g)

Initial Pressure (P₀) = 200 mmHg

Final pressure (Pt) = 300 mmHg

Time (t) = 20 min

To find :

The rate constant for the reaction (k)

Solution :

          A(g)       →       B(g)     +     C(g)

Initial  P₀=200             0               0

Final   P₀-P=200-P      P               P

Total Pressure (Pt) = 200-P + P + P

300 = 200 + P

P = 300 - 200

P = 100 mmHg

$k = \frac{2.303}{t} log(\frac{P_0}{P_0 - P} )$

$k = \frac{2.303}{20} log(\frac{200}{200 - 100} )$

$k = \frac{2.303}{20} log(\frac{200}{100} )$

k = 0.11515 × log(2)

k = 0.03466 min⁻¹

k = 0.035 min⁻¹

Therefore, the rate constant for the reaction is 0.035 min⁻¹.