CHEMISTRY HIGH SCHOOL

A 0.0489 mol sample of a nutrient substance, with a formula weight of 114 g/mol, is burned in a bomb calorimeter containing 6.56 × 10² g h2o. given that the fuel value is 2.04 × 10⁻¹ in nutritional cal when the temperature of the water is increased by 1.73°c, calculate the fuel value in kj.

Answers

Answer 1
Answer: To calculate the fuel value in kJ, we need to convert the nutritional calories to kilojoules.

1 nutritional calorie (cal) = 4.184 kilojoules (kJ)

First, let's calculate the energy released by burning the 0.0489 mol sample of the nutrient substance in calories:

Energy released = moles of nutrient substance * formula weight * fuel value

Energy released = 0.0489 mol * 114 g/mol * 2.04 × 10⁻¹ cal

Next, let's convert the energy released from calories to kilojoules:

Energy released (kJ) = Energy released (cal) * 4.184 kJ/cal

Now, let's substitute the given values into the equations:

Energy released = 0.0489 mol * 114 g/mol * 2.04 × 10⁻¹ cal
Energy released ≈ 0.11185 cal

Energy released (kJ) = 0.11185 cal * 4.184 kJ/cal
Energy released (kJ) ≈ 0.467 kJ

Therefore, the fuel value of the nutrient substance is approximately 0.467 kJ.
Answer 2
Answer:

Final answer:

To calculate the fuel value in kJ, convert nutritional calories to joules and then to kilojoules.

Explanation:

To calculate the fuel value in kJ, we need to convert the nutritional calories to joules and then to kilojoules. We can use the equation: fuel value (in kJ) = fuel value (in cal) x 4.184 / 1000. Given that the fuel value is 2.04 × 10⁻¹ nutritional cal, we can substitute it into the equation to get the fuel value in kJ.


fuel value (in kJ) = 2.04 × 10⁻¹ x 4.184 / 1000 =8.5288 x 10⁻³ kJ

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Final answer:

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Explanation:

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