# 6.03 Calorimetric Analysis

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1. 15.8 g of KCl is dissolved in 225 mL of water. Calculate the molarity. 2. Calculate the mass of KCl required to prepare 250. mL of 0.250 M solution. 3. Calculate the volume of 0.30 M KCl solution that contains 6.00 g of KCl. 6.00 g x 1 mole x 1 L = 0.27 L 74.6 g 0.30 mol 4. Calculate the volume of 0.250 M H2SO4 that contains 0.250 g H2SO4. 0.250 g H2SO4 x 1 mole x 1 L = 0.0102 L 98.12 g 0.250 mole 5. 1.50 g of NaCl is dissolved in 100.0 mL of water. Calculate the concentration. 6. How many moles of NaCl are in 250. mL of a 0.200 M solution? 1. 15.8 g of KCl is dissolved in 225 mL of water. Calculate the molarity. 2. Calculate…show more content…
Pb (NO3) 2 10. A compound is 42.3 % C, 5.94 % H, 32.9 % N, and 18.8 % O and has a molecular mass of 425.25 g/mol. Calculate the empirical and molecular formula. C15H25N10O5 11. How many moles of Al2O3 are produced by the reaction 200. g Al? 4Al + 302 → 2Al2O3 3.70 mole 12. How many moles Al are required to produce 300. g Al2O3? 4Al + 302 → 2Al2O3 5.88 mole 13. 100. g Al reacts with excess O2 to produce 150. g Al2O3 according to Calculate the theoretical and percentage yield. 4Al + 302 → 2 Al2O3. 79.4 % 14. Calculate the energy produced by the complete reaction of 150. g H2. 2H2 + O2 → 2H2O + 130KJ 4.83 x 103 kJ 15. How many grams of H2 would be needed to produce 260. KJ of energy? 2H2 + O2 → 2H2O + 130KJ 8.08 g 16. 20. mol H2 reacts with 8.0 mol O2 to produce H2O. Determine the number of grams reactant in excess and number of grams H2O produced. Identify the limiting reactant. 8.1 g H2 , 2.9 x 102 g H2O 17. How many litres of O2 gas are required to produce 100. g Al2O3? 4Al + 302 →