Question

3. The reaction between hydrochloric acid and barium hydroxide has a heat of neutralization of -118 kJ per mole of barium chloride. In a coffee-cup calorimeter, 100.0 mL of 0.500 M hydrochloric acid is mixed with 300.0 mL of 0.100 M barium hydroxide, both at 25.0°C. After the reaction, the final mixture has a mass of 400.0 g and has a specific heat capacity of 4.184 J/g°C. Calculate the final temperature of the mixture. 4. A 0.1964 g sample of quinone ($C_6H_4O_2$) is burned in a bomb calorimeter that has a heat capacity of 1.56 kJ/°C, and the temperature of the calorimeter rises from 21.0°C to 24.2°C. Calculate the heat of combustion of quinone in kJ per gram of quinone. 5. Using your answer from question 4, calculate the amount of heat released or absorbed when the given amounts of quinone are burned. (a) 3.65 grams of quinone (b) 75.0 mL of quinone (density = 1.256 g/mL)

          3. The reaction between hydrochloric acid and barium hydroxide has a heat of neutralization of -118 kJ per mole of barium chloride. In a coffee-cup calorimeter, 100.0 mL of 0.500 M hydrochloric acid is mixed with 300.0 mL of 0.100 M barium hydroxide, both at 25.0°C. After the reaction, the final mixture has a mass of 400.0 g and has a specific heat capacity of 4.184 J/g°C. Calculate the final temperature of the mixture.
4. A 0.1964 g sample of quinone ($C_6H_4O_2$) is burned in a bomb calorimeter that has a heat capacity of 1.56 kJ/°C, and the temperature of the calorimeter rises from 21.0°C to 24.2°C. Calculate the heat of combustion of quinone in kJ per gram of quinone.
5. Using your answer from question 4, calculate the amount of heat released or absorbed when the given amounts of quinone are burned.
(a) 3.65 grams of quinone
(b) 75.0 mL of quinone (density = 1.256 g/mL)

3. The reaction between hydrochloric acid and barium hydroxide has a heat of neutralization of -118 kJ per mole of barium chloride. In a coffee-cup calorimeter, 100.0 mL of 0.500 M hydrochloric acid is mixed with 300.0 mL of 0.100 M barium hydroxide, both at 25.0°C. After the reaction, the final mixture has a mass of 400.0 g and has a specific heat capacity of 4.184 J/g°C. Calculate the final temperature of the mixture.
4. A 0.1964 g sample of quinone (C6H4O2) is burned in a bomb calorimeter that has a heat capacity of 1.56 kJ/°C, and the temperature of the calorimeter rises from 21.0°C to 24.2°C. Calculate the heat of combustion of quinone in kJ per gram of quinone.
5. Using your answer from question 4, calculate the amount of heat released or absorbed when the given amounts of quinone are burned.
(a) 3.65 grams of quinone
(b) 75.0 mL of quinone (density = 1.256 g/mL)

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