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Consider the following simple reaction at equilibrium:

$${ H }_{ 2 }(g) + ICl(g) \overset { { k }_{ 1 } }{ \underset { { k }_{ -1 } }{ \rightleftarrows } } HI(g) + HCl(g)$$

...where ${ k }_{ 1 }$ and ${ k }_{ -1 }$ are the rate constants for the forward and reverse reaction, respectively.

Which of the following equality holds true at equilibrium?

A

${ k }_{ 1 } = { k }_{ -1 }$

B

$[{ H }_{ 2 }][ICl] = [HI][HCl]$

C

$[{ H }_{ 2 }] + [ICl] = [HI] + [HCl]$

D

${k}_{1}[{ H }_{ 2 }][ICl] = {k}_{-1}[HI][HCl]$

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