How many grams of hydrogen are needed to produce 1.80 g of water according to this equation?
2H₂ + O₂ → 2H₂O

Question

How many grams of hydrogen are needed to produce 1.80 g of water according to this equation? 2H₂ + O₂ → 2H₂O

Quizplus · Accepted Answer

In the balanced equation, we can see that 2 moles of hydrogen (2H) react with 1 mole of oxygen (O) to produce 2 moles of water (2H2O).

This means that 1 mole of water (H2O) requires 2 moles of hydrogen (2H).

First, we need to find the number of moles of water produced from 1.80 g. We can use the molar mass of water to do this:

Molar mass of H2O = 18.015 g/mol

Number of moles of H2O = mass / molar mass = 1.80 g / 18.015 g/mol = 0.0999 mol

So, 0.0999 mol of water requires 2 * 0.0999 mol = 0.1998 mol of hydrogen.

Finally, we can convert moles of hydrogen to grams:

Molar mass of H2 = 2.016 g/mol

Mass of hydrogen required = number of moles * molar mass = 0.1998 mol * 2.016 g/mol = 0.402 g

Rounded to two significant figures, the answer is 0.20 g of hydrogen. Therefore, the best choice is C.

How Many Grams of Hydrogen Are Needed to Produce 1