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Sulfur trioxide (SO3) can be produced using the reversible reaction shown.

Which change would keep this reaction from shifting to form more of the
product?

User Brielle
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2 Answers

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Final Answer:

Adding more sulfur trioxide (SO3) would prevent the reaction from shifting towards it, as it would oppose the forward reaction and push the equilibrium back towards the reactants.

Step-by-step explanation:

Le Chatelier's principle states that a system at equilibrium will adjust to oppose any changes in its conditions. In this reversible reaction, adding more SO3 (product) would increase its concentration, driving the reaction backwards to decrease its concentration and maintain equilibrium. Therefore, adding more SO3 would prevent the reaction from shifting further towards forming it.

Other options might seem appealing but are incorrect:

Removing SO3: This would directly shift the equilibrium towards forming more SO3 to replenish the removed product.

Adding sulfur dioxide (SO2): This is a reactant, and adding more would drive the reaction forward, producing more SO3.

Increasing the temperature: This reaction is exothermic, meaning it releases heat. Increasing the temperature would favor the reverse reaction, consuming SO3 and forming SO2.

Decreasing the pressure: The reaction involves a decrease in moles (from 2 to 1), so decreasing pressure would favor the forward reaction, producing more SO3 to increase pressure.

Therefore, adding more SO3 is the only option that would prevent the reaction from shifting towards forming more of the product.

User Brandon Kuczenski
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18 votes
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If
SO3(g)
is removed from the following reaction, will the equilibrium shift to the left, shift to the right, or stay the same? Explain.

2SO2(g)+O2(g)⇋2SO3(g);ΔH

Explanation: The reaction shown in the question is a combination reaction between sulfur dioxide gas and oxygen gas, forming sulfur trioxide gas by the two gases combining into one product. The question's objective is to determine the direction in which the equilibrium will shift if sulfur trioxide is removed. Removing the products from the container during a reversible chemical reaction means that only the forward reaction will proceed right after the products are removed. Once more of the products are formed, the reverse reaction will start to occur.

But, when the product is removed, the system will compensate for the removal of the product by increasing the production of the product, which is done by increasing the rate of the forward reaction and shifting the equilibrium to the right.

User Pelo
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