Answer: 286 calories of heat (energy) to heat 13.0g of water from 31.0°C to 53.0°C
Step-by-step explanation:
To calculate the amount of heat (energy) required to heat 13.0g of water from 31.0°C to 53.0°C, we can use the equation:
q = m * c * ΔT
where:
- q is the heat (energy) in calories,
- m is the mass of the substance (water in this case) in grams,
- c is the specific heat capacity of the substance, and
- ΔT is the change in temperature in degrees Celsius.
The specific heat capacity of water is approximately 1 calorie/gram°C.
First, let's calculate the change in temperature (ΔT):
ΔT = final temperature - initial temperature
= 53.0°C - 31.0°C
= 22.0°C
Next, substitute the values into the equation:
q = 13.0g * 1 calorie/gram°C * 22.0°C
= 286 calories
Therefore, it would take 286 calories of heat (energy) to heat 13.0g of water from 31.0°C to 53.0°C.