QuestionGrams A $\mathbf{M M}_{\mathrm{A}}$ Moles A mole ratio Moles B $\mathrm{MM}_{\mathrm{B}}$ Grams
What steps would you use to solve the following problem? Hydrogen and oxygen react to produce water as shown in the reaction below. $$2 \mathrm{H}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \rightarrow 2 \mathrm{H}_{2} \mathrm{O}(\mathrm{~g})$$
How many moles of water would be produced if 50.00 grams cf hydrogen reacted with excess oxygen gas? a. Step 1: Convert grams of hydrogen to moles of hydrogen with the molar mass of hydrogen.
Step 2: Convert moles of hydrogen to moles of water using the mole ratio from the balanced equation. Step 3: Convert moles of water to grams of water using the molar mass of water. b. Step 1: Convert grams of hydrogen to moles of hydrogen with the molar mass of hydrogen.
Step 2: Convert moles of hydrogen to moles of water using the mole ratio from the balanced equation. Step 3: Do not do this step. Problem is already done with correct units. c. Step 1: Skip this step and go directly to step 2.
Step 2: Convert moles of hydrogen to moles of water using the mole ratio from the balanced equation. Step 3: Convert moles of water to grams of water using the molar mass of water.
How many grams of oxygen will react with excess hydrogen to produce 25.0 grams of water in the synthesis of water reaction