For the following reaction:

The rate of reaction is $\frac{d P}{d t} = k [X]$ . Two moles of X are mixed with one mole of Y to make 1.0 L of solution.
At 50 s, 0.5 mole of Y is left in the reaction mixture. The correct statement(s) about the reaction is(are): (Use $ln 2 = 0.693$ )

Question

For the following reaction:

The rate of reaction is $\frac{d P}{d t} = k [X]$ . Two moles of X are mixed with one mole of Y to make 1.0 L of solution.

At 50 s, 0.5 mole of Y is left in the reaction mixture. The correct statement(s) about the reaction is(are): (Use $ln 2 = 0.693$ )

TestHub · Accepted Answer

dt dB ​ = k [ x ] 1 2 X + Y → P t = 0 2 1 t = 50 s ( 2 − 1 ) ( 1 − 0.5 ) 0.5 − 2 1 ​ dt dX ​ = dt dP ​ = k [ X ] 1 − dt dX ​ = 2 k [ X ] 1 2 k = 50 ℓ n 2 ​ ⇒ k = 100 ℓ n 2 ​ At t = 50 sec , dt − dX ​ = 2 k × ( 1 ) 1 = 50 ℓ n 2 ​ At t = 100 sec ; 2 − 1 ​ dt dX ​ = dt − dY ​ ⇒ − dt dY ​ = 100 ℓ n 2 ​ × 2 1 ​ { dx − dY ​ = k [ X ] 1 }

Chemistry - Chemical Kinetics Question with Solution | TestHub

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