At constant volume, the heat of combustion of a particular compound is –3323.0 kJ/mol. When 1.489 g of this compound (molar mass = 131.02 g/mol) was burned in a bomb calorimeter, the temperature of the calorimeter (including its contents) rose by 8.077 °C. What is the heat capacity (calorimeter constant) of the calorimeter?

mols compound = 1.489/131.02 = about 0.0114 but you need to do that more accurately.

kJ heat added to calorimeter = 3323 kJ/mol x 0.0114 mol = ? Then substitute this into
q = Ccal x delta T
Solve for Ccal.

To find the heat capacity (calorimeter constant) of the calorimeter, you can use the equation:

q = C × ΔT

Where:
q = heat transferred
C = heat capacity of the calorimeter
ΔT = change in temperature

First, convert the mass of the compound burned to moles:

mol = mass / molar mass
mol = 1.489 g / 131.02 g/mol
mol = 0.01137 mol

Since the heat of combustion is given per mole, the heat transferred can be calculated using the equation:

q = moles × heat of combustion
q = 0.01137 mol × (-3323.0 kJ/mol)
q = -37.76 kJ

Now, convert the temperature change to Kelvin:

ΔT = 8.077 °C + 273.15 K
ΔT = 281.23 K

Substituting the values into the equation:

-37.76 kJ = C × 281.23 K

Solving for C:

C = -37.76 kJ / 281.23 K
C ≈ -0.134 kJ/K

Therefore, the heat capacity (calorimeter constant) of the calorimeter is approximately -0.134 kJ/K.

To calculate the heat capacity (calorimeter constant) of the calorimeter, we need to use the equation:

q = C * ΔT

Where:
q = heat transferred (in this case, the heat of combustion)
C = heat capacity (calorimeter constant)
ΔT = change in temperature

First, let's convert the given mass of the compound burned to moles:
moles = mass / molar mass
moles = 1.489 g / 131.02 g/mol
moles ≈ 0.0114 mol

Next, we can calculate the heat transferred using the heat of combustion:
q = moles * heat of combustion
q = 0.0114 mol * (-3323.0 kJ/mol) ≈ -37.92 kJ

Now we have the heat transferred (q) and the change in temperature (ΔT = 8.077 °C). We can substitute these values into the equation and solve for the heat capacity (C):

-37.92 kJ = C * 8.077 °C

To convert the units, we'll convert kJ to calories:
1 kJ ≈ 239.0 calories

-37.92 kJ ≈ -37.92 * 239.0 cal

Now we have the equation in calories:
-37.92 * 239.0 cal = C * 8.077 °C

Simplifying the equation:
-9071.68 cal = C * 8.077 °C

Finally, solve for C by dividing both sides of the equation:
C = -9071.68 cal / 8.077 °C ≈ -1124.7 cal/°C

Therefore, the heat capacity (calorimeter constant) of the calorimeter is approximately -1124.7 cal/°C.