How many grams of H2O will be produced from 32.0 grams of O2?

Answer 1

Start with the balanced equation of the formation of water:

2 H2 + O2 --> 2 H2O

It takes one mole of oxygen to produce 2 moles of water.

32.0 g O2 * (1 mol O2/32.00 g O2) * (2 mol H2O/1 mol O2) * (18.02 g H2O/1 mol H2O) = 36.04 g

Therefore, about 36.04 grams of water will be produced from 32.0 grams of oxygen gas, assuming that it can react with unlimited amounts of hydrogen gas.

Answer 2

To the justified number of significant digits, the masses given correspond to one mole of diatomic oxygen and two moles of diatomic hydrogen. The formula of water is H2O; therefore, these numbers of moles produce two moles of water molecules, and the number of the latter is twice Avogadro's number = 1.2 X 1024.

Answer 3

32g of oxygen is 2 moles oxygen (O) atoms. To make this react completely you require 4 moles of hydrogen (H) atoms which weighs 4g.

Added:

Not by atoms but by molecules, like the balanced equation will give:

O2 + 2H2 --> 2H2O

Reactant [O2:H2] molecular ratio = reactant molar ratio = 1 : 2

O2 = 32 g O2 = 32g / (2*16.0) g/mol O2 = 1.0 mol O2

2H2 = 2.0 mol H2 = 2.0 * (2*1.008) g/mol H2 = 4.03 = 4.0 g H2

Answer 4

The balanced chemical equation for the reaction is 2 H2 + O2 -> 2 H2O. From the equation, we can see that 2 moles of H2O are produced for every mole of O2 consumed. First, we need to convert 32.0 grams of O2 to moles, then use the mole ratio from the balanced equation to find the moles of H2O produced, and finally convert those moles to grams of H2O.

Answer 5

36 grams of water

Answer 6

8 grams

Answer 7

4

Answer 8

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