Calculate the energy required to heat 0.20kg of ethanol from 4.5°C to 10.0°C. Assume the specific heat capacity of ethanol under these conditions is ·2.44J·g−1K−1 . Be sure your answer has the correct number of significant digits.

To calculate the energy required to heat a substance, we can use the formula:

Q = mcΔT

where: Q = heat energy (Joules, J) m = mass (grams, g) c = specific heat capacity (Joules per gram per degree Celsius, J/g°C) ΔT = change in temperature (degrees Celsius, °C)

First, we need to convert the mass from kg to g because the specific heat capacity is given in J/g°C.

1 kg = 1000 g

So, 0.20 kg = 0.20 * 1000 = 200 g

The change in temperature, ΔT, is the final temperature minus the initial temperature.

ΔT = T_final - T_initial = 10.0°C - 4.5°C = 5.5°C

Now we can plug the values into the formula:

Q = mcΔT = 200g * 2.44J/g°C * 5.5°C = 2682 J

So, the energy required to heat 0.20 kg of ethanol from 4.5°C to 10.0°C is 2682 Joules. This answer is rounded to four significant digits because the number with the least number of significant digits in the question is the specific heat capacity, which has three significant digits.

To calculate the energy required to heat a substance, we can use the formula:

Q = mcΔT

where: Q = heat energy (Joules, J) m = mass (grams, g) c = specific heat capacity (Joules per gram per degree Celsius, J/g°C) ΔT = change in temperature (degrees Celsius, °C)

Given: m = 0.20 kg = 200 g (since 1 kg = 1000 g) c = 2.44 J/g°C ΔT = 10.0°C - 4.5°C = 5.5°C

Substituting the given values into the formula:

Q = (200 g) * (2.44 J/g°C) * (5.5°C) = 2682 J

So, the energy required to heat 0.20 kg of ethanol from 4.5°C to 10.0°C is 2682 Joules.