How many liters of water can be made from 34 grams of oxygen gas and 6.0 grams of hydrogen gas at STP?

Answer 1

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Answer 2

At STP

1mol O2 = 22.4L

1mol O2 = 6.022 x 1023 molecules O2

22.4L O2 = 6.022 x 1023 molecules O2

Convert liters O2 to moles O2

3.36L O2 X (6.022 x 1023 molecules O2/22.4L O2) = 9.03 x 1022 molecules O2

Answer 3

Using the ideal gas law, we can calculate that 34 grams of oxygen gas is equivalent to approximately 1.5 moles, and 6.0 grams of hydrogen gas is approximately 3 moles. The balanced chemical equation for the reaction between oxygen and hydrogen to form water is 2H2 + O2 -> 2H2O. Since 2 moles of H2 produce 2 moles of H2O, 3 moles of H2 can produce 3 moles of H2O. At STP, 3 moles of water corresponds to 67.2 liters.

Answer 4

The chemical reaction of O2 with H2 to form water is O2 + 2 H2 = 2 H2O. 2.4 liters of H2 is equal to 107 millimoles. This means it reacts with 53.5 millimoles of O2, or 1.2 liters.

Answer 5

The synthesis reaction for water is 2 H2 + O2 = 2 H2O. 1.2 liters of hydrogen is equal to 53.5 millimoles, which means 26.75 millimoles of oxygen is needed. This is equal to 0.599 liters.

Answer 6

1.8

Answer 7

1 (one)

Answer 8

90.98 L