A hydrogen filled balloon was ignited and 1.30 of hydrogen reacted with 10.4 of oxygen. How many grams of water vapor were formed?
A hydrogen filled balloon is ignited and 1.30 g of hydrogen reacted with 10.4 g of oxygen.
When oxygen reacts with hydrogen, the chemical reaction that takes place is given by the equation:
2H2 + O2 --> 2H2O
From the equation it is seen that 2 moles of hydrogen (H2) reacts with one mole of oxygen (O2) to form 2 moles of water.
The molar mass of hydrogen is 2. 1.3 g of hydrogen is equivalent to .65 moles. The molar mass of oxygen is 32. 10.4 g of oxygen is equivalent to 10.4/32 = 0.325 moles.
When 0.325 moles of oxygen reacts with 0.325 moles of oxygen, 0.65 moles of water is formed. The molar mass of water is 18. The mass of 0.65 moles of water is 11.7 g
Two moles of hydrogen gas react with one mole of oxygen gas to form two moles of water.
1.3 grams of hydrogen is 1.3/2 = 0.65 moles of hydrogen.
10.4 grams of oxygen is 10.4/32 = 0.325 moles of oxygen.
If alll of the hydrogen reacts with all of the oxygen to produce 0.65 moles of water, then 0.66 moles of water is
0.65 x 18 = 11.7 grams of water