Question

QUESTION 16 The following balanced chemical equation is in equilibrium Which of the following changes will shift the equilibrium towards forming more products? 2A(g) + B(g) = 30g) 20(g) Increase the pressure of B Double the pressure of both reactants and products Decrease the volume of the reaction vessel, while the total mass and the temperature remain constant Add a catalyst Decrease the pressure of A QUESTION 17 You seal 10.0 moles of solid NH4NO3 into an empty 5.00 L container, The Ko for the following reaction is 245 104 What is the equilibrium pressure of the steam (H2O)? Assume there is an excess of NH4NO3(s). NH4NO3(s) = N20(g) 2H2003) 4.00 atm 0.394 atm 0.0788 atm 0.125 atm 0.0626 atm

Answer 1

2A19) + Big) = 3(g) + 2.Dig) According to he Chatelier's Principle The change in condition by any means results by shifting equilibrium te that side so that it oppose the changes. If we increase the pressure, the equilibrium shift towards the the side where least maeleonter molecules are present (A) If we increase the pressure of B, the equilibrium shift towards reactant Side because of least mole üles © Even if we double the pressure on both seachante and products, the equilibrium Shift according to number of molecules. In the's case, the equilibrium sheft to the deactant side. (c) Since the total mass and the temperature remain constant and it we decrease the volume then the pressure needs to be increased to Therefore the equilibrium Shift to the reactant side (0) there is absolutely no effect of cataty catalyst in the equilibrium. E) If we decrease the pressure y A then the equilibrium will more in such a way that the pressure increases again which is done by producing molecules therefore the equilibrium Shift to more number of molecules or to the product side. Correct option is (E)