Electrolysis of water occurs according to the following equation:2H2O → 2H2 + O2If electrolysis is performed with 100% efficiency on 100 grams of water, how many grams of hydrogen gas will be produced?A.100 gramsB.11 gramsC.50 gramsD.4 gramsSUBMITarrow_backPREVIOUS

To solve this problem, we need to use the concept of stoichiometry, which is a section of chemistry that involves using relationships between reactants and/or products in a chemical reaction to determine desired quantitative data.

1. First, we need to know the molar mass of water (H2O). The molar mass of hydrogen (H) is approximately 1 gram/mole, and there are two of them in water, so that's 2 grams/mole. The molar mass of oxygen (O) is approximately 16 grams/mole. So, the molar mass of water is 2 + 16 = 18 grams/mole.

2. We have 100 grams of water. To find out how many moles of water we have, we divide the mass of the water by the molar mass of water. So, 100 grams / 18 grams/mole = 5.56 moles of water.

3. According to the balanced chemical equation, 2 moles of water produce 2 moles of hydrogen gas. Therefore, 5.56 moles of water will produce 5.56 moles of hydrogen gas.

4. To find out how many grams of hydrogen gas this is, we multiply the number of moles by the molar mass of hydrogen gas (H2). The molar mass of H2 is 2 * 1 = 2 grams/mole. So, 5.56 moles * 2 grams/mole = 11.11 grams of hydrogen gas.

So, the answer is B. 11 grams.