Final answer:
To determine the amount of energy required to increase the temperature of water from 183 °C to 303 °C, we can use the equation: q = m * c * ΔT, where q is the energy absorbed, m is the mass of water, c is the specific heat capacity of water, and ΔT is the change in temperature. Substituting the given values, we can calculate the energy absorbed as 10044.8 J.
Step-by-step explanation:
To determine the amount of energy required to increase the temperature of water from 183 °C to 303 °C, we can use the equation:
q = m * c * ΔT
where:
-
-
- q is the energy absorbed (in joules)
-
-
- m is the mass of water (in grams)
-
-
- c is the specific heat capacity of water (in J/g °C)
-
-
- ΔT is the change in temperature (in °C)
-
Substituting the given values:
-
-
- m = 20.0 g
-
-
- c = 4.184 J/g °C
-
-
- ΔT = 303 °C - 183 °C = 120 °C
-
We can calculate the energy absorbed by multiplying the mass, specific heat capacity, and change in temperature:
q = 20.0 g * 4.184 J/g °C * 120 °C = 10044.8 J
Therefore, 20.0 g of water must absorb 10044.8 J of energy to increase its temperature from 183 °C to 303 °C.