Question

From the following balanced equation, CH,(g) +20,(g) — CO2(g) + 2 H2O(g) how many grams of H, O can be formed from 1.25 g CH ? • Your answer should have three significant figures.

Answer 1

Molar mass of CH4,

MM = 1*MM(C) + 4*MM(H)

= 1*12.01 + 4*1.008

= 16.042 g/mol

mass of CH4 = 1.25 g

mol of CH4 = (mass)/(molar mass)

= 1.25/16.04

= 7.792*10^-2 mol

According to balanced equation

mol of H2O formed = (2/1)* moles of CH4

= (2/1)*7.792*10^-2

= 0.1558 mol

Molar mass of H2O,

MM = 2*MM(H) + 1*MM(O)

= 2*1.008 + 1*16.0

= 18.016 g/mol

mass of H2O = number of mol * molar mass

= 0.1558*18.02

= 2.808 g

Answer: 2.81 g