3.3k views
1 vote
A hydrogen-filled balloon is ignited and 1.50 g of hydrogen reacts with 12.0 g of oxygen. How many grams of water vapor form? (assume that water vapor is the only product.)

User Alexey F
by
7.0k points

1 Answer

4 votes

The balanced chemical reaction between hydrogen and oxygen to form water is given as:


H_2(g)+(1)/(2)O_2(g)\rightarrow H_2O(g)

From the balanced chemical equation it is clear that one mole of hydrogen reacts to give 1 mole of water.

Since, number of moles =
(mass of the substance)/(Molar Mass)

So, number of moles of hydrogen =
(mass of the hydrogen)/(Molar Mass of hydrogen)

Mass of hydrogen =
1.50 g (given)

Molar mass of hydrogen,
H_2 = 2* 1 = 2 g/mol

Substituting the values:

Number of moles of hydrogen =
(1.5)/(2) = 0.75 mol

Number of moles of water formed on reacting with
0.75 mol of hydrogen is:

Number of moles of water =
0.75 mol

Mass of water can be calculated by:

Number of moles of water =
(mass of water)/(Molar Mass of water)

Molar mass of water =
2* 1+16 = 18 g/mol

Substituting the values:


0.75 mol = (mass of water)/(18 g/mol)


mass of water = 13.5 g

Hence, the mass of water vapor forms is
13.5 g.

User Jimkberry
by
8.3k points