When 53.14 grams of fictional compound X is added to water to make 522.1 grams of solution, the temperature increases from 20.89 °C to 64.83 °C. What is the heat of solution for compound X given that the molar mass of compound X is 91.01 g/mol? Assume the specific heat capacity of the solution is 4.18 J/g°C.     164.2 kJ/mol     -164.2 kJ/mol     -95.90 kJ/mol     -11.74 kJ/mol     95.90 kJ/mol

A hot lump of 42.4g of copper at an initial temperature of 64.7 °C is placed in 50.0 mL H2O initially at 25.0 °C and allowed to reach thermal equilibrium. What is the final temperature of the copper and water, given that the specific heat of copper is 0.385 J/(g·°C)?0.385 J/(g·°C)? Assume no heat is lost to surroundings.

A 33.6-g piece of silver initially at 46.5 °C is submerged into 162.4 g of water at 12.3 °C. What is the final temperature of the metal once the metal and water reaches thermal equilibrium? The specific heats of silver and water are 0.235 J/g·°C and 4.18 J/g·°C, respectively. 29.4 °C 10.4 °C 11.0 °C 12.7 °C 21.0 °C

When 30.87 grams of fictional compound X is added to water to make 438.9 grams of solution, the temperature increases from 26.23 °C to 62.34 °C. What is the heat of solution for compound X given that the molar mass of compound X is 130.58 g/mol? Assume the specific heat capacity of the solution is 4.18 J/g°C.     -280.2 kJ/mol     280.2 kJ/mol     -66.24 kJ/mol     4.649 kJ/mol     66.24 kJ/mol