Water has a specific heat of 4.18 J/g- °C. What is the quantity of energy (in kJ) required to increase the temperature of a 50.0 g sample of water from 25 °C to 99 °C?
q = mass H2O x specific heat H2O x (Tfinal-Tinitial)
Substitute and solve for q. The answer will be in joules. Convert to kJ.
Post your work if you get stuck.
To find the quantity of energy required to increase the temperature of water, we can use the equation:
Q = m * c * ΔT
where Q represents the energy, m is the mass of water, c is the specific heat of water, and ΔT is the change in temperature.
Given:
m = 50.0 g (mass of water)
c = 4.18 J/g-°C (specific heat of water)
ΔT = (99 °C - 25 °C) = 74 °C (change in temperature)
Now plug in the values into the equation:
Q = (50.0 g) * (4.18 J/g-°C) * (74 °C)
To get the energy in kJ, we need to convert Joules to kilojoules by dividing the result by 1000:
Q = ((50.0 g) * (4.18 J/g-°C) * (74 °C)) / 1000
Calculating this expression, we find:
Q ≈ 154.924 kJ
Therefore, the quantity of energy required to increase the temperature of a 50.0 g sample of water from 25 °C to 99 °C is approximately 154.924 kJ.