Consider the following equilibrium for which H = -10.37 kJ: H2(g) + I2(g) 2 HI(g

Question

Consider the following equilibrium for which H = -10.37 kJ: H2(g) + I2(g) 2 HI(g) If a mixture of the gases involved in this reaction is allowed to come to equilibrium, and the reaction mixture is heated, what will the reaction do in response to this change, and how will the value of K (the equilibrium constant) be affected? The reaction will shift toward reactants with a decrease in K. The reaction will shift toward products with an increase in K. The reaction will shift toward reactants with an increase in K. The reaction will shift toward products with a decrease in K. The reaction will not shift and the value of K will not change.

Explanation / Answer

) The reaction will shift toward reactants with a decrease in K.

because the increase in temperature favours endothermic reaction the back ward reaction is endothermic.as result of this the concentration of the reactants increases,kvalue cdecreases

Related Questions

Navigate

• Browse (All)
• Browse C
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.