(A). A reaction with a known q is performed in a bomb calorimeter and is found that 10.0 kj of heat is required to raise the temperature of the calorimeter by 2.15 degrees C. calculate the heat capacity of the calorimeter.

(B). When 1.00 g of C2H6(g) is burned in the bomb calorimeter from (A), the temperature rises from 22.00 degrees C to 33.13 degrees C. calculate q for the combustion of C2H6(g) as performed

Ccal x delta T = q

(mass x specific heat x delta T) + Ccal*delta T = q.

To solve both parts of the problem, we need to understand the concept of heat capacity and understand the equation for heat transfer.

Heat capacity (C) is the amount of heat required to raise the temperature of an object by 1 degree Celsius (or 1 Kelvin). It is calculated using the equation:

C = q / ΔT

where:
C = heat capacity
q = heat transfer
ΔT = change in temperature

Now let's solve each part of the problem:

(A) To calculate the heat capacity of the calorimeter, we need to use the given information: 10.0 kJ of heat is required to raise the temperature of the calorimeter by 2.15 degrees Celsius.

We can plug these values into the heat capacity equation to find C:

C = q / ΔT
C = 10.0 kJ / 2.15 °C

Make sure to convert the temperature change to Kelvin if needed. In this case, both Celsius and Kelvin have the same increment, so we can use Celsius directly.

C = 4.65 kJ/°C

Therefore, the heat capacity of the calorimeter is 4.65 kJ/°C.

(B) To calculate q for the combustion of C2H6(g), we need to use the temperature change and the heat capacity of the calorimeter.

We know that the temperature rises from 22.00 °C to 33.13 °C when 1.00 g of C2H6(g) is burned in the calorimeter.

The heat transferred during the combustion (q) can be calculated using the equation:

q = C * ΔT

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

We already calculated the heat capacity of the calorimeter in part (A) as 4.65 kJ/°C. Let's plug in the values to find q:

q = (4.65 kJ/°C) * (33.13 °C - 22.00 °C)

q = 4.65 kJ/°C * 11.13 °C

q ≈ 51.61 kJ

Therefore, q for the combustion of C2H6(g) is approximately 51.61 kJ.