Q1 If 1.00 mol each of carbon dioxide and hydrogen is initially injected into a 10.0-L reaction chamber at 986°C, what would be the concentrations of each entity at equilibrium?
CO2(g) +H2(g)→CO(g) +H2O(g) K = 1.60 for 986°C
( temperature is just to confuse you. Ignore it)
Step1:Convert the concentration into mol/l( if the concentration is already given in mol/l skip this step)
To get mol/l divide the number of moles with total volume given.1 mol/10 l=0.1 mol/l
Step2: Construct ICE chart by writing the equation.
|Concentration(mol/l)||CO2(g) +H2(g) →CO(g) +H2O(g)|
|Initial||0.1 0.1 0 0|
|Change||-x* -x +x +x|
|Equilibrium||(0.1-x) (0.1-x) x x|
*Reactant's concentration goes down and product concentration goes up as the reaction proceeds.So for change in concentration we need to use -x for reactants and +x for products.
Step3: Write the equilibrium expression and solve it.
Step 4:Square toot on both sides.
Hint: the answer should be less than the initial concentration.If you get x value greater than the initial concentration then use negative value for K after square rooting it.
"Rate This article