Suppose you have the following reaction at equilibrium: C(s) + 2H2(g) = CH4(g), ΔH = −74.8 kJ .

Suppose you have the following reaction at equilibrium:

C(s) + 2H₂(g) = CH₄(g), ΔH = −74.8 kJ

What changes are expected to occur if the pressure of the system was increased? You may select multiple answers.

		The temperature would increase above the expected temperature increase resulting from the increased pressure.
		The concentration of H₂(g) would decrease
		The amount of C(s) present would decrease
		The concentration of CH₄(g) would increase
		No change in the equilibrium would occur.
		The concentration of CH₄(g) would decrease

Expert Solution

The correct answer is The concentration of CH₄(g) would increase

Reasons:

According to Le Châtelier, if the pressure is increased, the position of equilibrium will shift so that the pressure is reduced once again. Pressure is originated by gas molecules hitting the sides of their container. The extra molecules in the container, the higher the pressure will be.

For the following reaction; two moles on the left-hand side of the equation, but only one on the right. By forming more CH₄(g), the system causes the pressure to reduce. Thus increasing the pressure on this gas reaction shifts the position of equilibrium towards the side with fewer moles of gas molecules means the formation of methane. As the result of this concentration of CH₄(g) will increase.

C(s) + 2H₂(g) = CH₄(g), ΔH = −74.8 kJ

queen_honey_blossom answered 2 years ago

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Question

Suppose you have the following reaction at equilibrium: C(s) + 2H2(g) = CH4(g), ΔH = −74.8 kJ .

Solutions

Expert Solution

Related Solutions

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