Question

Calculate the amount of heat required to heat a 45-kg sample of ethanol from 11.0 °C to 19.0 °C.

Answer 1

Answer:

Q=874800J

Explanation:

1. Use the specific heat capacity:

The specific heat capacity of ethanol is approximately 2.42 joules per gram per degree Celsius (J/g°C). This means it takes 2.42 J to raise the temperature of 1 gram of ethanol by 1°C.

2. Calculate the temperature change:

The temperature change is 19.0°C - 11.0°C = 8.0°C.

3. Calculate the total mass in grams:

We need to convert the sample size from kilograms to grams: 45 kg * 1000 g/kg = 45000 g.

4.Apply the formula:

Now, we can use the formula to calculate the amount of heat required:

Q = mcΔT

where:

• Q is the amount of heat (in joules)
• m is the mass (in grams)
• c is the specific heat capacity (in J/g°C)
• ΔT is the temperature change (in °C)

Substituting the values:

Q = 45000 g * 2.42 J/g°C * 8.0°C

Q = 874800 joules

Therefore, approximately 874,800 joules of heat are required to heat the 45-kg sample of ethanol from 11.0°C to 19.0°C.