Question

I need c,d,e, and f please.

2.00 g of Benzoic Acid arc burned in a bomb calorimeter, and the temperature increases from 17.84 degree C to 23.34 degree C. What is the heat capacity of the calorimeter? You burn 4.08 g of Arginine in the bomb calorimeter. The temperature increases from 17.49 degree C to 23.83 degree C. Determine the enthalpy of combusion and the enthalpy of formation of Arginine. Arginine has a standard molar entropy of 250.G J/mol K. Determine the entropy of reaction for the combusion of 4.08 g Arginine. Calculate the entropy change of the surroundings and the universe for the combustion of 4.08 g of Arginine. Calculate the Gibbs energy (if reaction for the combusion of 4.08 k of Arginine. Predict the enthalpy of combusion for 1.08 K of Arginine at 373 K. Arginine has a heat capacity of 232.8 J/mol K which you may mum is constant.

Answer 1

a) The heat of combustion of benzoic acid is -3227 KJ/mol

The equation for the combustion is,

C7H6O2(s) + 7.5 O2(g) -> 7CO2(g) + 3H2O(l), dH° = 3227 kJ

Since 7.5 moles of O₂ gas is needed, and 7 moles of CO₂ is produced, some pressure-volume work is done, to the calorimeter:

P V = dn * R * T, where dn = (7 - 7.5) = - 0.5 mol
dE = dH - dn R T
= - 3227 - (-0.5*    0.008314 kJ/(K mol) * 298)

= - 3226 kJ/mol (a small correction)

The amount of heat produced by 2.0 g benzoic acid is

q = 2.0 /122.13 mol x 3226 (kJ/mol) = 52.83kJ

Thus, the heat capacity is

C = q / dT = 52.83 / (23.34 -17.84)

C= 52.83 / 5.5 = 9.6 kJ / K.(answer)