Compound A is burned in a bomb calorimeter that contains 2.50 dm3of water. If thecombustion of 0.175 moles of this compound causes the temperature of the water torise 45.00C, what is the molar heat of combustion of compound A?The heat capacity of water is 4.18 J g-1K
Question
Compound A is burned in a bomb calorimeter that contains 2.50 dm3of water. If thecombustion of 0.175 moles of this compound causes the temperature of the water torise 45.00C, what is the molar heat of combustion of compound A?The heat capacity of water is 4.18 J g-1K
Solution
To solve this problem, we need to use the formula for heat transfer: q = mcΔT, where:
- q is the heat transferred,
- m is the mass of the substance (in this case, water),
- c is the specific heat capacity of the substance,
- ΔT is the change in temperature.
First, we need to convert the volume of water to mass. Since the density of water is approximately 1 g/cm³ (or 1 g/dm³), the mass of the water is 2.50 dm³ * 1 g/dm³ = 2500 g.
Next, we can calculate the heat transferred using the formula:
q = mcΔT q = 2500 g * 4.18 J/gK * 45.00 K q = 470250 J
This is the amount of heat produced by the combustion of 0.175 moles of compound A. To find the molar heat of combustion, we divide this value by the number of moles:
q/n = 470250 J / 0.175 mol = 2687142.86 J/mol
Therefore, the molar heat of combustion of compound A is approximately 2687142.86 J/mol.
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