41. Methanol (CH,OH) is used in the production of many chemicals. Methanol is made by reacting carbon monoxide and hydrogen at high temperature and pressure.
CO(g) + 2H, (g) → > CH30H(g)
a. How many moles of each reactant are needed to produce 3.60 X 102 g CH,OH?
b. Calculate the number of grams of each reactant needed to produce 4.00 mol CHOH.
c. How many grams of hydrogen are necessary to react with 2.85 mol of Co?
a. To determine the moles of each reactant needed, we need to use their molar masses.
The molar mass of CO is 28.01 g/mol.
The molar mass of H2 is 2.02 g/mol.
From the balanced equation, we can see that the mole ratio between CO and CH3OH is 1:1, and the mole ratio between H2 and CH3OH is 2:1.
So, to produce 1 mole of CH3OH, we need 1 mole of CO and 2 moles of H2.
To produce 3.60 x 10^2 g of CH3OH, we can use the following calculations:
(3.60 x 10^2 g CH3OH) x (1 mol CH3OH / 32.04 g CH3OH) = 11.24 mol CH3OH
Therefore, we need 11.24 moles of CO and 22.48 moles of H2 to produce 3.60 x 10^2 g CH3OH.
b. To determine the grams of each reactant needed, we need to use their molar masses.
To produce 1 mole of CH3OH, we need 1 mole of CO and 2 moles of H2.
So, to produce 4.00 mol CH3OH, we would need:
- 4.00 mol CO x (28.01 g CO / 1 mol CO) = 112.04 g CO
- 4.00 mol H2 x (2.02 g H2 / 1 mol H2) = 8.08 g H2
Therefore, we would need 112.04 grams of CO and 8.08 grams of H2 to produce 4.00 mol CH3OH.
c. Again, the mole ratio between CO and H2 in the balanced equation is 1:2. This means that for every 1 mole of CO, we need 2 moles of H2.
To determine the grams of hydrogen necessary to react with 2.85 mol of CO, we can use the following calculation:
2.85 mol CO x (2 mol H2 / 1 mol CO) x (2.02 g H2 / 1 mol H2) = 11.55 g H2
Therefore, we would need 11.55 grams of hydrogen to react with 2.85 mol of CO.