Question

1. Carbon Monoxide gas reacts with diatomic hydrogen gas to form CH3OH gas at 298K in a 1.00L container.

a. Write a balanced chemical equation for this reaction.

b. If 3.00g of H2 reacts with 3.00g of CO, determine the theoretical yield (in moles) and limiting reactant.

c. Determine the amount of excess reactant left over. (In moles.)

d. Determine the partial pressure for each species in the container after the reaction is complete and the total pressure in the container (there will be no limiting reactant left over.)

Please show all work.

Answer 1

a)

reaction

CO + H2 = CH3OH

balance

CO + 2H2 = CH3OH

b)

mol of H2 = mass/MW = 3/2 = 1.5

mol of CO = mass/MW = 3/28 = 0.10714

1 mol of CO =1 mol of CH3OH

then

0.10714 mol of CO = 0.10714 mol of CH3OH

limiting reactants is CO since it has less moles than H2

c)

exces = mol of H2 initially - mol of H2 reacted = 1.5 -0.10714*2 = 1.28572 mol

d)

Pgas

PV = nRT

mol of H2 = 1.28572 , mol of CO = 0, mol of CH3COOH = 0.10714

mol total = 0.10714 + 1.28572 = 1.39286

P = nRT/V = (1.39286)(0.082)(298)/1 =

P = 34.035 atm