Consider the following reaction that is occurring inside a sealed container: CH4(g) + NH3(g) <-- -->...

Consider the following reaction that is occurring inside a sealed container:

CH₄(g) + NH₃(g) <-- --> HCN(g) + 3H₂(g)

If we increase the volume of the sealed container without changing the temperature, will this affect the amounts of product and reactant in this container? If so, will the amounts of products increase or decrease? Briefly EXPLAIN!

Solutions

Expert Solution

The concentration of component decreases as we increase the volume of container. So for decreased concentration rate of reaction for forward reaction and for backward reaction decreases. This decrease in reaction rate depends on a number of molecules associated.

For given reaction, product side that is for HCN and H2 have more no. of mole(4 mole) than CH4 and NH3. According to Le Chatelier's principle, if we decrease the pressure, the equilibrium will shift in such a way as to increase the pressure. If we can increase the number of gas molecules in the container, then the pressure will increase. If the position of equilibrium shifts to the right, we get more gas molecules in the mixture.

Therefore, If we increase the volume of the sealed container without changing the temperature, this will affect the amounts of product and reactant in this container, according to Le Chatelier principle.

The amounts of products will increase.

queen_honey_blossom answered 1 year ago

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