Consider the following equilibrium system for the high-temperature reduction of

Question

Consider the following equilibrium system for the high-temperature reduction of tin(lI) oxide (SnO) by dihydrogen (H2). Which of the following changes wi result in an increased yield of Sn(s) at equilibrium, and why? Sno(s) + H2(g) Sn(s) + H20(g) O Increasing the pressure of H2(9), because this makes reaction quotient Q smaller than K. O Increasing the pressure of H2(g), because this makes reaction quotient Q larger than K O Increasing the pressure of H20(9), because this makes reaction quotient Q smaller than K. O The yield of Sn will not change, because Sn is a solid that does not appear in the expression for Q.

Explanation / Answer

we want to increase yield of Sn(s) which is a product
So, we must increase concentration of reactant

Increasing pressure of H2(g) will make Q smaller than K and hence reaction will move in forward direction increasing yield of Sn(s)

Answer: option 1

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