Consider the decomposition of limestone: CaCO 3 (s) <--> CaO(s) + CO 2 (g) for w
ID: 484414 • Letter: C
Question
Consider the decomposition of limestone: CaCO3(s) <--> CaO(s) + CO2(g) for which the forward reaction is endothermic. If the reaction takes place in a closed container what will be the effect of decreasing the pressure?
the reaction will go in the forward direction until all reactants are gone more slowly.
the reaction will go in the forward direction until all reactants are gone more quickly.
the equilibrium will shift towards the products
the equilibrium will not be affected
the equilibrium will shift towards the reactants
A.the reaction will go in the forward direction until all reactants are gone more slowly.
B.the reaction will go in the forward direction until all reactants are gone more quickly.
C.the equilibrium will shift towards the products
D.the equilibrium will not be affected
E.the equilibrium will shift towards the reactants
Explanation / Answer
the answer is equilibrium will shift towards the products (option C)
decreasing the pressure will drives the reaction towards more molecules here calcium carbonate decompose in calcium oxide and carbon dioxide therefore by decreasing the pressure allow more molecule in the system, it will favour the equlibrium towards the product.