Question

What reactant concentrations, pressure and temperature conditions would favor the production of the substance that is underlined in each of the following equations. Make sure you address all three of the factors listed above for each equilibrium.

a) 2CO(g) + O2(g) <--> 2CO2 (g) + 167 kJ
b) Cu2+(aq) + 4NH3(aq) <--> Cu(NH3)42+(aq) + 42 kJ
c) 2HI(g) + 12.6 kJ <--> H2(g) + I2(g)
d) 4HCl(g) + O2(g) <--> 2H2O(g) + 2Cl2(g) + 113 kJ
e) PCl5(g) + 88 kJ <--> PCl3(g) + Cl2(g)

Answer 1

a) Increase the pressure, Increase the reactants, Decrease the temperature

b) No effect on pressure, Increase the reactants, Decrease the temperature

c) No effect on pressure, Increase the reactants, Increase the temperature

d) No effect on pressure, Increase the reactants, Decrease the temperature

e) Decrease the pressure, Increase the reactants, Increase the temperature

I had to look up the questions online because you did not underline them properly, but yeah these should be the respective conditions for each equation

Increasing pressure shifts equilibrium to the side with the least amount of gas moles, decreasing pressure does the opposite

Increasing Reactants will cause more products to be made

Increasing temperature in an endothermic reaction will shift equilibrium to the right, and in the opposite direction if the reaction is exothermic (left)

Decreasing temperature in an endothermic reaction will shift equilibrium to the left, and in the opposite direction if the reaction is exothermic (right)