liquid heptane C7H16 is completely combusted to produce CO2 and H2O: C7H16 + 11O2 --> 7CO2 + 8H2O

the heat combustion for one mole of C7H16 is -4.85*10^-3
CO2 heat of comb. = -393.5
H2O h of c= -285.8
a) calc. the vale of heat of cumbustion for C7H16 in kJ/mol

a .0108 mol sample of C7H16 is combusted in a bomb calorimeter.
1) calc. amnt of heat releasd to the calorimeter
2) total heat capacity is 9.273 kJ/C, calc. temp. change of the calorimeter.

a. heat combustion = [delta H products]-[delta H reactants].

1. You know what 1 mole is, set up ratio/proportion for 00108 mol. This is q.
2. q = 9.273 kJ/c x delta T. Solve for delta T.

a) To calculate the heat of combustion for C7H16 in kJ/mol, we need to use the given values for the heat of combustion of CO2 and H2O.

Since 1 mole of C7H16 produces 7 moles of CO2 and 8 moles of H2O, the heat of combustion for C7H16 can be calculated as follows:

Heat of combustion for C7H16 = (7 mol CO2 × -393.5 kJ/mol CO2) + (8 mol H2O × -285.8 kJ/mol H2O)
= -2754.5 kJ/mol + (-2286.4 kJ/mol)
= -5039.7 kJ/mol

Therefore, the heat of combustion for C7H16 is -5039.7 kJ/mol.

1) To calculate the amount of heat released to the calorimeter, we need to use the heat of combustion of C7H16.

Amount of heat released = moles of C7H16 combusted × heat of combustion for C7H16
= 0.0108 mol × (-5039.7 kJ/mol)
= -54.44 kJ

Therefore, the amount of heat released to the calorimeter is -54.44 kJ.

2) To calculate the temperature change of the calorimeter, we need to use the total heat capacity of the calorimeter.

Temperature change = Amount of heat released / Total heat capacity
= -54.44 kJ / 9.273 kJ/C
= -5.87°C

Therefore, the temperature change of the calorimeter is -5.87°C.

To calculate the heat of combustion for C7H16 in kJ/mol, you need to use the stoichiometric coefficients provided in the balanced equation and the heat of combustion values for CO2 and H2O.

Step 1: Calculate the heat of combustion for one mole of C7H16
From the balanced equation:
1 mole of C7H16 produces 7 moles of CO2 and 8 moles of H2O.
Therefore, the heat of combustion for one mole of C7H16 can be calculated as follows:
H = (7 × heat of combustion of CO2) + (8 × heat of combustion of H2O)
H = (7 × -393.5 kJ/mol) + (8 × -285.8 kJ/mol)
H ≈ -3935 kJ/mol

So, the heat of combustion for one mole of C7H16 is approximately -3935 kJ/mol.

Step 2: Calculate the amount of heat released to the calorimeter
Given that you have a 0.0108 mol sample of C7H16, you can calculate the heat released to the calorimeter using the heat of combustion value obtained in Step 1:
Heat released = moles of C7H16 × heat of combustion for one mole of C7H16
Heat released = 0.0108 mol × -3935 kJ/mol
Heat released ≈ -42.468 kJ

Therefore, approximately -42.468 kJ of heat is released to the calorimeter.

Step 3: Calculate the temperature change of the calorimeter
Given that the total heat capacity of the calorimeter is 9.273 kJ/°C, you can calculate the temperature change using the heat released obtained in Step 2:
Temperature change = Heat released / Heat capacity
Temperature change = -42.468 kJ / 9.273 kJ/°C
Temperature change ≈ -4.58 °C

Therefore, the temperature of the calorimeter decreases by approximately 4.58 °C.