If you burn 50.4 g of hydrogen and produce 4.50 × 102 g of water, how much oxygen reacted?

The amount of O₂ reacted to give 4.50 × 10² g H₂O = 400 g

Explanation:

Reaction involved: 2H₂ + O₂ → 2H₂O

In this reaction, 2 moles (2 g/mol) of H₂ reacts with 1 mole (32 g/mol) of O₂ to give 2 moles of H₂O (18 g/mol).

Given: 50.4 g H₂ reacts to give 4.50 × 10² g water.

Number of moles of H₂ burned = 50.4 g ÷ 2 g/mol = 25.2 moles

Number of moles of H₂O formed = 4.50 × 10² g ÷ 18 g/mol = 25 moles

∵ 2 moles H₂O is formed from 1 mole O₂

∴ The number of moles of O₂ that reacts to give 25 moles H₂O =  25 moles ÷ 2 moles = 12.5 moles

Therefore, the amount of O₂ reacted to give 4.50 × 10² g H₂O = 12.5 mole × 32 g/mol = 400 g

the density of gold = 19.3 g/cm3

the relation between density and mass and volume is

density = mass / volume

given :

mass of gold = 13 g

density = 13g / volume = 19.3

volume = 13 /19.3 = 0.67 cm^3

thus volume of gold nugget = 0.67 cm^3

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