How many liters of hydrogen will be produced by the decomposition of 59 grams of dihydrogen dioxide at STP?
To calculate the number of liters of hydrogen produced by the decomposition of dihydrogen dioxide at STP (Standard Temperature and Pressure), we need to follow a step-by-step approach.
Step 1: Find the molar mass of dihydrogen dioxide (H2O2).
The molar mass of dihydrogen dioxide (H2O2) is calculated by summing up the atomic masses of its constituent atoms.
H2O2:
2 Hydrogen (H) atoms x atomic mass of hydrogen (1.008 g/mol) = 2.016 g/mol
2 Oxygen (O) atoms x atomic mass of oxygen (15.999 g/mol) = 31.998 g/mol
Total molar mass of H2O2 = 2.016 + 31.998 = 34.014 g/mol
Step 2: Calculate the number of moles of dihydrogen dioxide.
To find the number of moles of a substance, we divide the given mass of the substance by its molar mass.
Number of moles = Mass / Molar mass
Number of moles of H2O2 = 59 g / 34.014 g/mol
Step 3: Use the balanced chemical equation to determine the number of moles of hydrogen produced.
The balanced chemical equation for the decomposition of dihydrogen dioxide (H2O2) is:
2 H2O2 → 2 H2O + O2
From the equation, we can see that for every 2 moles of H2O2, we obtain 2 moles of H2.
Therefore, the number of moles of H2 produced is equal to the number of moles of H2O2.
Number of moles of H2 = Number of moles of H2O2
Step 4: Convert moles of hydrogen to liters.
At STP, one mole of gas occupies 22.4 liters.
Number of liters of H2 = Number of moles of H2 x 22.4 liters/mol
Plug in the value for the number of moles of H2 from Step 3 into the equation to calculate the answer.
Overall, the number of liters of hydrogen produced by the decomposition of 59 grams of dihydrogen dioxide at STP can be obtained by following these steps.