When 15.00 mL of 3.00 M NaOH was mixed in a calorimeter with 13.30 ml. of 3.00 M HCI, both initially at room temperature (22.00 °C), the temperature increased to 29.80 °C. The resultant salt solution had a mass of 28.30 g and a specific heat capacity of 3.74 J Kg. What is the heat capacity of the calorimeter (in J/°C)? Note: The molar enthalpy of neutralization per mole of HCI is -55.84 kJ mol-¹. heat capacity of the calorimeter: JPC

When 15.00 mL of 3.00 M NaOH was mixed in a calorimeter with 13.30 ml. of 3.00 M HCI, both initially at room temperature (22.00 °C), the temperature increased to 29.80 °C. The resultant salt solution had a mass of 28.30 g and a specific heat capacity of 3.74 J Kg. What is the heat capacity of the calorimeter (in J/°C)? Note: The molar enthalpy of neutralization per mole of HCI is -55.84 kJ mol-¹. heat capacity of the calorimeter: JPC

Chemistry

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Chapter6: Thermochemistry

Section: Chapter Questions

Problem 66E: In a coffee-cup calorimeter, 100.0 mL of 1.0 M NaOH and 100.0 mL of 1.0 M HCI are mixed. Both...

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A student performing a calorimetry experiment combined 100.0 ml. of 0.50 M HCI and 100.0 ml. of 0.50 M NaOH in a StyrofoamTM cup calorimeter. Both solutions were initially at 20.0 C, but when the two were mixed, the temperature rose to 23.2 C (a) Suppose the experiment is repeated in the same calorimeter but this time using 200 mL of 0.50 M HCl and 200.0 ml of 0.50 M NaOH. WIII the AT observed be greater than, less than, or equal to that in the first experiment, and why? (b) Suppose that the experiment is repeated once again in the same calorimeter, this time using 100 mL of 1.00 M HCI and 100.0 ml. of 1.00 M NaOH. Will the T observed be greater than, less than, or equal to that in the first experiment, and why?
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