when 50 g of H2S reacts with 50 g of O2, how much SO2 will it produce?
This is a limiting reagent problem. I know that because BOTH reactants are given. The scheme for solving these problems is to work a simple stoichiometry problem twice, once with one reactant and a second time with the other reactant. You will obtain two answers for the moles of the product, the correct answer in limiting reagent problems is ALWAYS the smaller one. Here is a worked example of a simple stoichiometry problem. Just follow the steps. Post your work if you get stuck.
http://www.jiskha.com/science/chemistry/stoichiometry.html
To determine the amount of SO2 produced when 50 g of H2S reacts with 50 g of O2, you need to follow these steps:
1. Write the balanced chemical equation for the reaction between H2S and O2:
2H2S + 3O2 → 2SO2 + 2H2O
2. Determine the molar masses of H2S and O2. The molar mass of H2S is (2 x 1.0079) + 32.07 = 34.0819 g/mol. The molar mass of O2 is (2 x 15.999) = 31.998 g/mol.
3. Calculate the number of moles of H2S and O2 using the given mass and molar mass. The number of moles is equal to mass divided by molar mass.
Moles of H2S = 50 g / 34.0819 g/mol = 1.4671 mol
Moles of O2 = 50 g / 31.998 g/mol = 1.562 moles
4. Determine the stoichiometric ratio between H2S and SO2 from the balanced chemical equation. In this case, it is a 2:2 ratio, meaning 2 moles of H2S react to produce 2 moles of SO2.
5. Use the stoichiometric ratio to calculate the moles of SO2 produced. Since the stoichiometric ratio is 2:2, the moles of SO2 will be the same as the moles of H2S.
Moles of SO2 = 1.4671 mol
6. Calculate the mass of SO2 produced using the molar mass of SO2.
Mass of SO2 = Moles of SO2 x Molar mass of SO2
= 1.4671 mol x (32.07 g/mol)
= 47.01 g
Therefore, when 50 g of H2S reacts with 50 g of O2, it will produce around 47.01 g of SO2.