When 0.514 g of biphenyl, C12H10, undergoes combustion in a bomb calorimeter, the temperature rises from 25.8 C to 29.4 C. Find ∆Urxn for the combustion of biphenyl. The bomb calorimeter contains 750.0 mL of water and has a heat capacity of 2.72 kJ/C.

When 0.515 g of biphenyl (C12H10) undergoes combustion in a bomb calorimeter, the temperature rises from 25.8oC to 29.4oC. Find ∆Erxn for the combustion of biphenyl in kJ/mol. The heat capacity of the bomb calorimeter, determined separately, is 5.86 kJ/oC.

Mothballs are composed primarily of the hydrocarbon naphthalene (C10H8). When 1.025 g of naphthalene burns in a bomb calorimeter, the temperature rises from 24.25 °C to 32.33 °C. Find ΔErxn for the combustion of naphthalene. The heat capacity of the bomb calorimeter, determined in a separate experiment, is 5.11 kJ/°C.

A certain chemical reaction releases 269. kJ of heat energy per mole of reactant consumed. Suppose some moles of the reactant are put into a calorimeter (a device for measuring heat flow). It takes 3.21 J of heat energy to raise the temperature of this calorimeter by 1 °C. Now the reaction is run until all the reactant is gone, and the temperature of the calorimeter is found to rise by 5.0 °C. How would you calculate the number of moles of reactant that were consumed? Set the math up. But don't do any of it. Just leave your answer as a math expression. Also, be sure your answer includes all the correct unit symbols. moles consumed = x10 010 X Ś