Consider the following chemical reaction: |
Part A How many liters of hydrogen gas is formed from the complete reaction of 18.8 g C? Assume that the hydrogen gas is collected at a pressure of 1.0 atm and a temperature of 360 K . Express your answer using two significant figures. |
A)
Molar mass of C = 12.01 g/mol
mass of C = 18.8 g
mol of C = (mass)/(molar mass)
= 18.8/12.01
= 1.5654 mol
From balanced chemical reaction, we see that
when 1 mol of C reacts, 1 mol of H2 is formed
mol of H2 formed = moles of C
= 1.5654 mol
we have:
P = 1.0 atm
n = 1.5654 mol
T = 360.0 K
we have below equation to be used:
P * V = n*R*T
1 atm * V = 1.5654 mol* 0.08206 atm.L/mol.K * 360 K
V = 46 L
Answer: 46 L
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