How many grams of water are obtained when 16 g of hydrogen are burned? Ar (H) = 1, Mr (H2O) = 18

To solve this problem, we perform the following actions:
we compose the equation of reactions, which looks as follows:
2H2 + O2 = 2 H2O
From the conditions it follows that the mass of hydrogen is 16 g, Substitute in the equation of reactions, also since there is 2 in front of hydrogen, then we put 2 mol under hydrogen, under water also 2 mol.
16g xg
2H2 + O2 = 2 H2O
2mol 2mol
The molar mass of hydrogen is M (n) = 1 × 2 × 2 = 4 g / mol
Molar water is M (H2O) = (2 + 16) × 2 = 36
16g H2 – 4g / mol H2
x g – 36g / mol H2O
We calculate the value of the unknown number x
x = 36 × 16 ÷ 4 = 144 g
Answer: the mass is 144 grams.