In a constant-pressure calorimetry experiment, a coffee-cup calorimeter containing 100 mL of water at an initial temperature of 23.0 °C is used. If 4.60 g of CaCl2 is added to the calorimeter, what will be the final temperature of the solution, assuming the dissolution of CaCl2 is an exothermic process?

In a constant-pressure calorimetry experiment, butane was burnt causing a temperature change of 25.5 K in 1200 g of water (specific heat capacity = 4.18 J/g⋅K). Calculate the heat change of the water. Give the answer to three significant figures.

In a coffee-cup calorimeter experiment, 10.00 g of a soluble ionic compound was added to the calorimeter containing 75.0 g H2O initially at 23.2°C. The final temperature of the solution was 31.8°C. What was the change in enthalpy (ΔH) for the dissolution of the compound?

In a constant-pressure calorimeter, 70.0 mL of 0.330 M Ba(OH)2 is mixed with 70.0 mL of 0.660 M HCl, causing the temperature to rise from 22.99 °C to 27.49 °C. Assuming the solution has the same density and specific heat as water, what is the enthalpy change (ΔH) of the reaction per mole of Ba(OH)2?

In a constant-pressure calorimetry experiment, a coffee-cup calorimeter containing 100 mL of water is used. The initial temperature of the calorimeter is 23.0 °C. If 8.20 g of CaCl2 is added to the calorimeter, what will be the final temperature of the solution, given that the enthalpy change for the dissolution of CaCl2 is -82.8 kJ/mol?

You are experimentally determining the change in enthalpy when dissolving an ionic compound in water using a coffee-cup calorimeter. When you dissolve 38.28 g of the ionic compound (molar mass = 102 g/mol) in 369 g of water in a coffee-cup calorimeter, the temperature of the solution changes from 25.0°C to 28.5°C. Given that the specific heat capacity of water is 4.18 J/g°C, what is the change in enthalpy (ΔH) for the dissolution process?

What is the enthalpy change (ΔH) for the reaction when 200.0 mL of 0.100 M AgNO3 is mixed with 100.0 mL of 0.100 M NaCl in a coffee cup calorimeter, given that the temperature rises from 24.69°C to 25.16°C and the calorimeter has a heat capacity of 105.5 J/°C?

Using a coffee-cup calorimeter, the ΔH_rxn for the dissolution of KCl(s) into KCl(aq) is determined. The initial temperature of the water in the calorimeter is 26.5°C. After the reaction, the temperature is measured again and found to be 23.0°C. What is the sign of ΔH_rxn for this reaction?

When 1.80 g of magnesium metal reacts with 200 mL of 6.00 M aqueous HCl, the temperature rises from 25.0 °C to 42.1 °C. Calculate ΔH in kilojoules for the reaction, assuming the heat capacity of the calorimeter is 776 J/°C. What is the value of ΔH?