Using the equaation 2h2+o2-->2h2o if 10.0g of hydrogen are used in the presence of excess oxygen how many grams of water will e produced

90g of H2O

Explanation:

2H2 + O2 —> 2H2O

First, we calculate the molar masses of H2 And H20.

Molar Mass of H2 = 2g/mol

Mass conc of H2 from the balanced equation = 2 x 2 = 4g

Molar Mass of H2O = 2 + 16 = 18g/mol

Mass conc of H2O from the balanced equation = 2x18 = 36g

From the equation,

4g of H2 produced 36g of H2O

Therefore, 10g of H2 will be produce = (10x36)/4 = 90g of H2O

every chemical equation adheres to the law of conservation of mass, which states that matter cannot be created or destroyed. therefore, there must be the same number of atoms of each element on each side of a chemical equation.