At Equilibrium

Chemistry Level 1

What is the effect of halving \text{halving} the p r e s s u r e \color{#3D99F6}{pressure} by doubling \text{doubling} the v o l u m e \color{#20A900}{volume} on the following system,

H 2 ( g ) + I 2 ( g ) ⇌ 2 H I ( g ) \large H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}

Details: \text{ Details: }

  • System is in equilibrium \text{equilibrium} at 500℃.

  • X ( g ) X_{(g)} means substance X is in gaseous phase \text{gaseous phase} .

Shift to product side Liquefaction of HI No effect Shift to product formation

Akhil Bansal by Akhil Bansal , 22, India

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1 solution

Raj Magesh
Sep 11, 2015

Changing the pressure of an equilibrium mixture affects the position of equilibrium only when there are an unequal number of moles of gaseous products and reactants. In this case, there are the same number of moles of gaseous products and reactants, 2. Hence, no effect is observed.

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