Quiz 2 -Shifting Equilibrium - Chemistry - Grade 12- W9

If a system that is at equilibrium is disturbed, then it will change in a way that will oppose the

• decomposition of reactants.

• re-formation of reactants.

• stress on the system.

• synthesis of products.

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By applying Le Châtelier’s principle to a reaction that has come to equilibrium, you can make the reaction

• produce more reactants.

• run to completion.

• reach a new chemical equilibrium.

• All of the above

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Which of the following is not a stress on an equilibrium reaction involving gases?

• increasing pressure

• raising temperature

• maintaining volume

• varying the concentrations

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Consider the reaction represented by the equation 
CO(g) + 3 H2 (g)   $\longleftrightarrow$ CH4(g)  +  H2O(l)

Which of the following could you add to the system without affecting the reaction? 

• CO(g)

• H2

• CH2(g)

• H2O(l)

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Write the equilibrium constant expression for the following equation: Fe(s) + 5CO(g)   $\longleftrightarrow$  Fe(CO)3 (g)

• [Fe]

• 5[CO][Fe(CO)3]

•  $\frac{\text{[Fe] [5CO]}}{\text{[ Fe(OH)]3}}$  

•  $\frac{\left[Fe\left(CO\right)_3\right]}{\left[CO\right]^5}$  

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Explain why changes in the concentrations of the reactants and products at equilibrium have no effect on the value of the equilibrium constant.

In the space provided, predict the effect that decreasing pressure would have on each of the following reaction systems at equilibrium .
1- H2(g)     +  Cl2(g)      $\longleftrightarrow$    2HCl(g)

2- 3O2(g)      $\longleftrightarrow$    2O3(g)

3- CaCO3(s)    $\longleftrightarrow$   CaO(S)   +  CO2(g)