A 100g sample of water absorbs 308kJ of heat. If the water was initially at -10 degrees Celsius, what is its final temperature?

Is that water at -10. Does it go through freezing or not.

yes, its freezing

To find the final temperature of the water, we can use the equation:

q = m * c * ΔT

where:
q is the heat absorbed (308 kJ),
m is the mass of the water sample (100 g),
c is the specific heat capacity of water (4.18 J/g°C),
ΔT is the change in temperature.

First, we need to convert the heat absorbed from kilojoules to joules:
308 kJ = 308,000 J

Rearranging the equation, we can solve for ΔT:
ΔT = q / (m * c)

Substituting the values:
ΔT = 308,000 J / (100 g * 4.18 J/g°C)

Calculating:
ΔT ≈ 737.32°C

Since we started with -10°C, the final temperature can be calculated by adding the change in temperature to the initial temperature:
Final temperature = -10°C + 737.32°C

Final temperature ≈ 727.32°C