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Consider the following reaction at equilibrium. What effect will reducing the volume have on the system?...

Consider the following reaction at equilibrium. What effect will reducing the volume have on the system?

C3H8(g) + 5 O2(g) ⇌ 3 CO2(g) + 4 H2O(l) ΔH° = -2220 kJ

The reaction will shift to the left in the direction of reactants.

The equilibrium constant will increase.

No effect will be observed.

The equilibrium constant will decrease.

The reaction will shift to the right in the direction of products.
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Answer #2

C3H8(g) + 5O2(g) 3CO2(g) + 4 H2O(l)

Here, one of the product is a liquid.

Number of moles of gaseous reactants = 6

Number of moles of gaseous product = 3

Therefore, according to the Le chatliers principle, reducing the volume of the system will increase the pressure of the system. The system will try to reduce the pressure by shifting the equilibrium to the lower moles of gas (which occupy most space). Therefore, equilibrium will shift right (in the direction of products)

Answer: The reaction will shift to the right in the direction of products.

answered by: anonymous
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