For the reaction 2 Na + 2 H2O -------> 2 NaOH + H2, how many grams of hydrogen gas are produced when 133.6 g of water are reacted?
I tired it like the steps to the last one and I still got answer wrong can you please show steps you would perform?
This 4-step procedure will work all simple stoichiometry problems. Limiting reagent problems take an addition one or two steps.
1. Write and balance the equation. You have that.
2. Convert what you have (in this case H2O) to mols. mol = g/molar mass = 133.6/18 = approx 7.5 but you need go through this and the other calculations and do them more accurately.
3. Using the coefficients in the balanced equation, convert mols of what you have (H2O) to mols of what you want (in this case H2).
7.5 mols H2O x (1 mol H2/2 mol H2O) = 7.5 x 1/2 = approx 3.75.
4. Now convert mols of what you want to grams. g = mols x molar mass
approx 3.75 mol H2 x (2 grams/mol H2) = approx 7.5 g H2.