At constant volume, the heat of combustion of a particular compound, compound a, is –3568.0 kj/mol. when 1.411 g of compound a (molar mass = 115.27 g/mol) was burned in a bomb calorimeter, the temperature of the calorimeter (including its contents) rose by 3.379 °
c. using this data, what is the heat capacity (calorimeter constant) of the calorimeter?

Answer : The heat capacity (calorimeter constant) of the calorimeter is,

Explanation:

First we have to calculate the moles of compound A.

Now we have to calculate the heat of combustion of compound A for 0.01224 mol.

As, 1 mole of compound A has heat of combustion = 3568.0 kJ

So, 0.01224 mole of compound A has heat of combustion = 0.01224 × 3568.0 kJ

                                                                                                 = 43.67 kJ

Now we have to calculate the heat capacity (calorimeter constant) of the calorimeter.

where,

q = heat of combustion = 43.67 kJ

c = heat capacity = ?

= change in temperature =

Now put all the given values in the above expression, we get:

Therefore, the heat capacity (calorimeter constant) of the calorimeter is,

r just means there's a number of carbon in teh chain. for example rcooh means that after x number of carbon, the chain ends with cooh.

explanation:

hloride, what is the mass of calcium in

explanation: