Answer:
Step-by-step explanation:
I believe there is a mistake in the temperature values provided in your question. Water cannot exist at a temperature of 283.0°C or 303.0°C, as it boils at 100°C and freezes at 0°C under standard conditions.
If you meant to say that the initial temperature of the water was 283.0K and the final temperature was 303.0K, then we can use the formula:
q = m * c * ΔT
where q is the amount of energy absorbed, m is the mass of water, c is the specific heat capacity of water, and ΔT is the change in temperature.
The specific heat capacity of water is approximately 4.18 J/g*K.
Using the values given, we have:
m = 20.0 g
c = 4.18 J/g*K
ΔT = 303.0K - 283.0K = 20.0K
Plugging in these values, we get:
q = 20.0 g * 4.18 J/g*K * 20.0K = 1672 J
Therefore, 20.0 g of water must absorb 1672 J of energy to increase its temperature from 283.0K to 303.0K.