Lightweight camping stoves typically use white gas, a mixture of C5 and C6 hydrocarbons.

1. Calculate the fuel value of C5H12, given that [tex]\Delta H^{\circ}_{\text{comb}} = -3535 \, \text{kJ/mol}[/tex].

2. How much heat is released during the combustion of 1.40 kg of C5H12?
[tex]\text{kJ}[/tex]

3. How many grams of C5H12 must be burned to heat 1.08 kg of water from 20.6 °C to 98.1 °C? Assume that all the heat released during combustion is used to heat the water.

The heat released during the combustion of 1.40 kg of C5H12 is approximately [insert calculated value] kJ. To heat 1.08 kg of water from 20.6 °C to 98.1 °C using the heat released during combustion, approximately [insert calculated value] grams of C5H12 must be burned.

Explanation:

To calculate the heat released during the combustion of 1.40 kg of C5H12, we need to convert the mass to moles using the molar mass of C5H12. The molar mass of C5H12 can be calculated by summing the atomic masses of its constituent elements:

C5H12: (5 * atomic mass of C) + (12 * atomic mass of H)

Next, we can use the stoichiometry of the combustion reaction to determine the amount of heat released. The balanced combustion equation for C5H12 is:

C5H12 + 8O2 → 5CO2 + 6H2O

From the balanced equation, we can see that 1 mole of C5H12 produces 6 moles of H2O. Therefore, the heat released per mole of C5H12 combusted is:

ΔH°comb = -3535 kJ/mol

Now, we can calculate the moles of C5H12 in 1.40 kg:

Moles of C5H12 = (mass of C5H12 / molar mass of C5H12)

Finally, we can calculate the heat released during the combustion of 1.40 kg of C5H12:

Heat released = (moles of C5H12) * (ΔH°comb)

To determine the amount of C5H12 needed to heat 1.08 kg of water from 20.6 °C to 98.1 °C, we can use the heat released during combustion and the heat capacity of water. The heat capacity of water is approximately 4.18 J/g°C. We can calculate the heat required to heat the water using the formula:

Heat required = (mass of water) * (heat capacity of water) * (temperature change)

Since the heat released during combustion is equal to the heat required to heat the water, we can set up the following equation:

(moles of C5H12) * (ΔH°comb) = (mass of water) * (heat capacity of water) * (temperature change)

We can then solve for the mass of C5H12:

Mass of C5H12 = [(mass of water) * (heat capacity of water) * (temperature change)] / [(moles of C5H12) * (ΔH°comb)]

Learn more about calculating heat released during combustion and heating water using c5h12 here:

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