Consider the following heterogeneous reaction: Mg(s) + 2H_3O^+ (aq) rightleftarr

Question

Consider the following heterogeneous reaction: Mg(s) + 2H_3O^+ (aq) rightleftarrow Mg^2+ (aq) + H_2 (g) + 2H_2O(l) Which of the following statements is false? The amount of magnesium present does not affect the equilibrium position. Adding 1.0 atm of N_2 to the system would cause the reverse reaction to be favored. Increasing P_H_2 causes the forward reaction to be favored Increasing [H_3O^+] causes the forward reaction to be favored. Decreasing [Mg^2+] causes the forward reaction to be favored. 31.5 kJ 16.1 kJ QUESTION 3 Consider the following heterogeneous reaction: Mg(s) 2H30 (aq) (aq) H2 (g) 2H20 2+, Which of the following statements is false? O The amount of magnesium present does not affect the equilibrium position. O Adding 1.0 atm of N2 to the system would cause the reverse reaction to be favored. Increasing PH, causes the forward reaction to be favored Increasing DH30 causes the forward reaction to be favored. Decreasing [Mg2+] causes the forward reaction to be favored.

Explanation / Answer

Mg is solid and its amount will not effect the equilibrium position

Adding N2 will increase pressure. So reaction will move to side containing less gases. that is , it will move to reactant side. Reverse reaction is favoured

adding H2 will favour reverse reaction as H2 is a product

adding [H3o+] favours forward reaction as it is reactant

decreasing Mg2+ will favour forward reaction as it is a product

So, 3rd option is false

Answer: Increasing PH2 causes the forward reaction to be favoured

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