Ch 8, #12
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Consider the balanced equation below:
C(s)+H2O(g) à CO(g)+H2(g)
a.) How many mol of hydrogen can be produced from 120.g of carbon?
C-12g/mol
H2 -2g/mol ß MOLECULAR WEIGHT
O-16g/mol
STEP 1: 120.g C * (1 mol C/12 g C) = 10 mol C
STEP 2: 16 g/mol O +2 g/mol H2 = 18 g/mol H2O
STEP 3: 10 mol H2O * (18 g H2O/1 mol H2O) = 180 g H2O = 160 g O + 20 g H2
STEP 4: 20 g H2 * (1 mol/2 g H+) = 10 mol H2
EXPLANATION
step 1: The total grams of carbon (120g) is divided by the molecular
weight of carbon (12 g/mol).
step 2: The molecular weights of oxygen (16 g/mol) and hydrogen (2 g/mol)
are added together to get the molecular weight of water.
step 3: Because there is a 1 to 1 ratio between carbon and water, 10 mol
of water is multiplied by the molecular weight of water. The
answer is divided to show how many grams of both hydrogen and
oxygen are produced.
step 4: 20 grams of hydogen is divided by the molecular weight of
hydrogen. This gives us the final solution.
SOLUTION
10 MOL OF HYDROGEN CAN BE PRODUCED FROM 120.GRAMS OF CARBON.