Question

A hydrogen-filled balloon was ignited and 1.80 g of hydrogen reacted with 14.4 g of oxygen. How many grams of water vapor were formed?

Answer 1

1.80 g of hydrogen reacts with 14.4 g of oxygen to form water vapor. The grams of water vapor formed is 32.08 g.

Step-by-step explanation:

In the given reaction, 1.80 g of hydrogen reacts with 14.4 g of oxygen to form water vapor. To find the grams of water vapor formed, we need to determine the limiting reactant and use stoichiometry.

First, we calculate the moles of hydrogen and oxygen using their respective molar masses:

• Moles of hydrogen: 1.80 g / 2.02 g/mol = 0.891 mol
• Moles of oxygen: 14.4 g / 32.00 g/mol = 0.450 mol

Since hydrogen is the limiting reactant (it has fewer moles than oxygen), we can use its moles to calculate the moles of water formed:

• Moles of water vapor: 0.891 mol (hydrogen) × 2 mol (water) = 1.782 mol

Finally, we convert the moles of water vapor to grams:

• Grams of water vapor: 1.782 mol × 18.02 g/mol = 32.08 g

Answer 2

Hydrogen reacts with water according to the following equation:
2H2 + O2 ..............> 2H2O

From the periodic table:
molar mass of hydrogen = 1 gram
molar mass of oxygen = 16 grams

Therefore:
4 grams of hydrogen react with 32 grams of oxygen to produce 36 grams of water vapor.

Now, we need to determine the limiting reactant in the equation. By comparing, we can deduce that hydrogen is the limiting reactant (because half of that amount is less than how much O2 you have).
This means that, once the amount of the reacting hydrogen is consumed, the reaction will stop. So, our calculations will be based on the amount of reacting hydrogen.

Now, back to our calculations:
we know that 4 grams of hydrogen are needed to produce 36 grams of water vapor.
To know how many grams of water vapor were produced from 1.8 grams of hydrogen, we will use cross multiplication as follows:
mass of water vapor = (1.8 x 36) / 4 = 16.2 grams