Question

We have a bomb calorimeter with a heat capacity of 555 J/K. In this bomb calorimeter, we place 1000.0 mL of water. We burn 2.465 g of a solid in this bomb calorimeter. The temperature of the bomb calorimeter and the water increases by 2.22 oC. The molar mass of the solid is 551.2 g/mol. How much heat (in kJ) will be released if we were to burn 0.162 mol of this same solid in the bomb calorimeter? Keep in mind that we want to find the amout of heat released. The specific heat capacity or water is 4.184 J/K/g. Approximate the density of water as being exactly 1.00 g/mL.

Answer 1

To find the amount of heat released when burning 0.162 mol of the solid in the bomb calorimeter, we can use the concept of heat capacity and the equation:

q = C * ΔT

where:
q is the heat transferred (in joules),
C is the heat capacity of the bomb calorimeter (in joules per Kelvin),
ΔT is the change in temperature (in Kelvin).

First, let's calculate the heat released when burning 2.465 g of the solid:

First, convert the mass of the solid to moles:
moles = mass / molar mass
moles = 2.465 g / 551.2 g/mol
moles = 0.00447 mol

Now, let's calculate the heat released for this amount of solid burned:
q1 = C * ΔT
q1 = 555 J/K * 2.22 K
q1 = 1232.1 J

Now, let's find the heat released per mole of the solid:
q per mole = q1 / 0.00447 mol
q per mole = 1232.1 J / 0.00447 mol
q per mole = 275,695 J/mol

Finally, let's find the heat released when burning 0.162 mol of the solid:
q2 = q per mole * 0.162 mol
q2 = 275,695 J/mol * 0.162 mol
q2 = 44,697 J

Converting the heat released to kilojoules:
q2_kJ = q2 / 1000
q2_kJ = 44,697 J / 1000
q2_kJ = 44.697 kJ

Therefore, if we were to burn 0.162 mol of the solid in the bomb calorimeter, approximately 44.697 kJ of heat would be released.