Molar mass of CH4,
MM = 1*MM(C) + 4*MM(H)
= 1*12.01 + 4*1.008
= 16.042 g/mol
mass(CH4)= 1.12 g
use:
number of mol of CH4,
n = mass of CH4/molar mass of CH4
=(1.12 g)/(16.04 g/mol)
= 6.982*10^-2 mol
Molar mass of O2 = 32 g/mol
mass(O2)= 1.7 g
use:
number of mol of O2,
n = mass of O2/molar mass of O2
=(1.7 g)/(32 g/mol)
= 5.312*10^-2 mol
Balanced chemical equation is:
CH4 + 2 O2 ---> 2 H2O + CO2
1 mol of CH4 reacts with 2 mol of O2
for 6.982*10^-2 mol of CH4, 0.1396 mol of O2 is required
But we have 5.312*10^-2 mol of O2
so, O2 is limiting reagent
we will use O2 in further calculation
Molar mass of H2O,
MM = 2*MM(H) + 1*MM(O)
= 2*1.008 + 1*16.0
= 18.016 g/mol
According to balanced equation
mol of H2O formed = (2/2)* moles of O2
= (2/2)*5.312*10^-2
= 5.312*10^-2 mol
use:
mass of H2O = number of mol * molar mass
= 5.312*10^-2*18.02
= 0.9571 g
Answer: 0.957 g
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