THERMODYNAMICS: The combustion of 1.00 mol of glucose (C6H1206) liberates 2820 kJ of heat. If 1.57 g of glucose is burned in a calorimeter containing 985 g of water, and the temperature of the...


THERMODYNAMICS: The combustion of 1.00 mol of glucose (C6H1206) liberates 2820 kJ of heat. If 1.57 g of glucose is<br>burned in a calorimeter containing 985 g of water, and the temperature of the assembly increases from 20.10°C to 23.57°C,<br>what is the heat capacity of the calorimeter in kJ/°C? MW of glucose is 180 g/mol. (Round off the final answer to TWO decimal<br>places. Do not include the unit.)<br>QUESTION 9<br>THERMODYNAMICS: Given the following hvpothetical thermochemicaleguations:<br>

Extracted text: THERMODYNAMICS: The combustion of 1.00 mol of glucose (C6H1206) liberates 2820 kJ of heat. If 1.57 g of glucose is burned in a calorimeter containing 985 g of water, and the temperature of the assembly increases from 20.10°C to 23.57°C, what is the heat capacity of the calorimeter in kJ/°C? MW of glucose is 180 g/mol. (Round off the final answer to TWO decimal places. Do not include the unit.) QUESTION 9 THERMODYNAMICS: Given the following hvpothetical thermochemicaleguations:

Jun 09, 2022
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