Question

Question 1. An insulated container is used to hold 54.0 g of water at 17.6°C. A sample of copper weighing 7.10 g is placed in a dry test tube and heated for 30 minutes in a boiling water bath at 100.1°C. The heated test tube is carefully removed from the water bath with laboratory tongs and inclined so that the copper slides into the water in the insulated container. Given that the specific heat of solid copper is 0.385 J/(g·°C), calculate the maximum temperature of the water in the insulated container after the copper metal is added.

Question 2. A 53.00 mL sample of 0.70 M NaOH is mixed with 88.7 mL of 1.0 M H₂SO₄ in a large Styrofoam coffee cup; the cup is fitted with a lid through which passes a calibrated thermometer. The temperature of each solution before mixing is 21.3°C. After adding the NaOH solution to the coffee cup and stirring the mixed solutions with the thermometer, calculate the maximum temperature measured. Assume that the density of the mixed solutions is 1.00 g/mL, that the specific heat of the mixed solutions is 4.18 J/(g · °C), ΔH_rxn = -114kJ/mol H₂SO₄, and that no heat is lost to the surroundings.(Hint: To complete this problem you need to determine how many moles of H₂SO₄ actually reacted. This requires a Limiting reagent calculation. Once you have the moles of H₂SO₄ you can convert ΔH_rxn to q_rxn by using the -114kJ/mol as a conversion factor)

Please explain step by step, thank you

Answer 1