How many moles of water can be made from 4 moles of oxygen gas and

16 moles of hydrogen gas? What is the limiting reagent?

Same problem as you posted earlier.

To find out how many moles of water can be made from the given amounts of oxygen gas and hydrogen gas, we need to determine the limiting reagent first.

The limiting reagent is the reactant that will be completely consumed, thus limiting the amount of product formed. To determine the limiting reagent, you can use the concept of stoichiometry, which involves comparing the mole ratio of the reactants to the balanced chemical equation.

The balanced chemical equation for the reaction between oxygen gas (O2) and hydrogen gas (H2) to form water (H2O) is:

2H2 + O2 -> 2H2O

According to the equation, 2 moles of hydrogen gas react with 1 mole of oxygen gas to produce 2 moles of water.

Given that we have 4 moles of oxygen gas and 16 moles of hydrogen gas, we can calculate the moles of water that can be formed based on the limiting reagent.

For oxygen gas (O2):
- According to the equation, 1 mole of O2 reacts with 2 moles of H2O.
- Therefore, based on the given amount of oxygen gas, we would expect to produce (4/1) x 2 = 8 moles of water.

For hydrogen gas (H2):
- According to the equation, 2 moles of H2 react with 2 moles of H2O.
- Therefore, based on the given amount of hydrogen gas, we would expect to produce (16/2) x 2 = 16 moles of water.

Comparing the calculated values, we can see that the maximum yield of water is limited by the amount of oxygen gas. Thus, the limiting reagent is oxygen gas (O2).

In summary, from 4 moles of oxygen gas and 16 moles of hydrogen gas, the limiting reagent is oxygen gas. The maximum amount of water that can be formed is 8 moles.