A sample of benzene, C6H6, weighing 3.51 g was burned in an excess of oxygen in a bomb calorimeter. The temperature of the calorimeter rose from 25.00 C to 37.18 C. If the heat capacity of the calorimeter is 12.05 kJ/K, what is the molar energy of combustion for benzene? Also, what would be the value of q for burning 50.3 g of benzen at constant volume and 25.00 C?

For a certain change, the value of deltaU is -2.37 kJ. During the change, the system absorbs 650 joules. How much work did the system do

To determine the molar energy of combustion for benzene, we need to calculate the heat released during the combustion reaction and then divide it by the number of moles of benzene.

First, let's calculate the heat released in the combustion reaction using the formula:

q = m * c * ΔT

Where:
q is the heat released (in Joules)
m is the mass of the substance burned (in grams)
c is the heat capacity of the calorimeter (in Joules per degree Celsius)
ΔT is the change in temperature (final temperature - initial temperature)

Given values:
m = 3.51 g
c = 12.05 kJ/K = 12.05 * 1000 J/K (since 1 kJ = 1000 J)
ΔT = 37.18°C - 25.00°C = 12.18°C

q = 3.51 g * (12.05 * 1000 J/K) * 12.18°C

Now, let's calculate the number of moles of benzene using its molar mass.

The molar mass of benzene (C6H6) is:
6 carbon atoms (12.01 g/mol) + 6 hydrogen atoms (1.01 g/mol) = 78.11 g/mol

Number of moles of benzene = mass of benzene (in grams) / molar mass of benzene

Number of moles of benzene = 3.51 g / 78.11 g/mol

Finally, divide the heat released (in Joules) by the number of moles of benzene to get the molar energy of combustion:

Molar energy of combustion = q / number of moles of benzene

Now, let's calculate the value of q for burning 50.3 g of benzene.

Follow the same steps as before, but use the mass of benzene as 50.3 g instead of 3.51 g.

The equation for q is the same:

q = m * c * ΔT

Where:
m = 50.3 g (new mass of benzene)

Calculate q using the new value of m, c, and ΔT.