For the reaction in question 2 above, determine the predicted yield for Mg(OH)2 and H2. What is the actual yield for these products if the percent yield is 80 percent?

You're in the wrong forum and you refer to a question that isn't there.

To determine the predicted yield for Mg(OH)2 and H2, as well as the actual yield given the percent yield, we need the stoichiometry of the reaction and the starting amount of reactant.

Unfortunately, you mentioned "question 2 above", but I don't have access to that information. Therefore, I won't be able to provide the specific answer for your reaction. However, I can guide you on how to calculate the predicted and actual yield using the given percent yield.

1. Determine the balanced chemical equation for the reaction.

2. From the balanced equation, identify the stoichiometry of the reaction, which shows the mole ratio between the reactants and products.

3. Determine the moles of the reactant used by dividing the given mass of the reactant by its molar mass.

4. Use the stoichiometry to calculate the moles of the products that can be produced.

5. To calculate the predicted yield, multiply the moles of the desired product by its molar mass to obtain the mass of the product that should be obtained in theory.

6. To calculate the actual yield, multiply the predicted yield by the given percent yield.

Remember that percent yield is calculated by dividing the actual yield by the theoretical yield and then multiplying by 100%.

I hope this general explanation helps you understand the steps involved in determining the predicted and actual yield. If you provide me with the specific reaction and starting amount of reactant, I will be able to help you with the calculations.