Question

A mixture of 0.0375 g of hydrogen and 0.0185 mol of oxygen in a closed container is sparked to initiate a reaction. How many grams of water can form? Which reactant is in excess, and how many grams of it remain after the reaction? 2H₂(g) + O₂(g) → 2H₂O(l).

Answer 1

0.324 g of water can form from the reaction. Oxygen is the reactant in excess, and 0.0005 g of it remains after the reaction.

Step-by-step explanation:

To determine how many grams of water can form from the given reactants, we first need to determine which reactant is in excess.

From the information provided, we can calculate the number of moles of each reactant. The molar mass of hydrogen (H₂) is 2.02 g/mol and the molar mass of oxygen (O₂) is 32.0 g/mol.

Using the given masses and molar masses, we find that there are 0.018 mol of hydrogen and 0.0185 mol of oxygen. Since the ratio of hydrogen to oxygen in the balanced equation is 2:1, we can see that there is excess oxygen, and all the hydrogen will react.

To determine the grams of water formed, we use the molar mass of water (18.02 g/mol). Since 2 mol of water is formed for every 2 mol of hydrogen, the number of moles of water formed is equal to the number of moles of hydrogen.

Therefore, 0.018 mol of water can form, which is equal to 0.018 x 18.02 = 0.324 g of water.

Since all the hydrogen will react, 0 g of hydrogen will remain after the reaction. The excess oxygen, 0.0185 - 0.018 = 0.0005 mol, remains after the reaction.