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Stoichiometric calculations always require a balanced equation. Chemists often use balanced chemical reactions to predict amounts of products used or amounts of reactants needed. To solve mass to mass problems you need to be able to: A. Convert mass to mole and mole to mass B. Use coefficients from balanced equations to make mole to mole calculations Mass to mole conversions \& mole to mass conversions (review) Equation: 1 mole =1 molar mass in grams Questions: How many moles of KOH is 21.0g of KOH ? Questions: What is the mass of 0.210 moles K2SO4 in grams? Stoichiometric mole to mole calculations For mole to mole calculations, one predicts mole quantities of reactants or products based on the provided moles of another reactant or product within the same chemical equation. You only need to use the coefficients and their ratios (mole ratios) to make the necessary calculations. The following equation is already balanced. 2KOH(aq)+H2SO4(aq)K2SO4(aq)+2H2O(l) Question-1: How many moles of KsO4 is produced if 7.00 moles of KOH is used for the reaction? Questions-2: How many moles of HSO is needed to react with 6.00 moles of KOH ? Mass To Mass Stoichiometric Calculations In these kinds of problems you utilize your skills in mass to mole and stoichiometric mole to mole calculations. If you can do both, you shouldn't have any problem doing stoichiometric mass to mass problems. These are 3 step problems. 2KOH(aq)+H2SO4(aq)K2SO4(aq)+2H2O(l) Question-1: Using the above equation, predict how many grams of K2SO4 is produced, if 18.0g of KOH is used in the reaction. [Hint: mass of KOH mol of KOHmolK2SO4 mass of K2SO4 ] Question-2: Using the above equation, predict what mass of H2SO4 is needed to react with 1.60g of KOH