Answer Happy

1. Calculate the final temperature for each of the following mixtures. Assume no heat loss to the environment. Show your method for part b. a. 50.0 mL of water at 25.0°C is mixed with 50.0 mL of water at 85.0°C. b. 75.0 g of water at 25.0°C is mixed with 25.0 g of water at 85.0°C. 2. a. In Part B of this experiment, 0.10g of Mg is added to 50. mL of 1.0M HC1. Which is the limiting reactant? Show calculations. b. In Part C, 0.25 g of MgO is added to 50.mL of 1.0M HC1. Which is the limiting reactant? 3. When 50.0mL of 1.00M H₂SO4 at 26.1°C was added to 50.0mL of 1.00M NaOH also at 26.1°C, the temperature rose to 32.6°C. Assume the resulting solution had a total volume of 100.0 mL with the same density and specific heat as water. Calculate AH for the reaction described by this equation. H₂SO4(aq) + 2 NaOH(aq) → Na₂SO4(aq) + 2 H₂O(1) Steps: Which reactant limits? How many moles of it are present? How much energy required to heat 100.0g solution from 26.1°C to 32.6°C? How much energy is released by the reaction. per one mole of the limiting reactant? How many moles of that reactant are in the given equation? What is AH in kJ (not kJ/mol)? Show calculations here: