what is the amount of heat lost in KJ for 50 ml of water going from 70.0 degrees C to 1.0 degrees?

To calculate the amount of heat lost by water, we can use the formula:

Q = m * c * ΔT

Where:
Q is the amount of heat lost (in kilojoules, KJ)
m is the mass of the water (in grams)
c is the specific heat capacity of water (4.18 J/g°C)
ΔT is the change in temperature (in degrees Celsius)

First, we need to convert the given volume of water (50 mL) to mass. Since the density of water is approximately 1 g/mL, the mass can be calculated as:

Mass = Volume * Density
Mass = 50 mL * 1 g/mL = 50 grams

Next, we can calculate the change in temperature:

ΔT = Final Temperature - Initial Temperature
ΔT = 1.0°C - 70.0°C = -69.0°C

Now we have all the values we need to calculate the amount of heat lost:

Q = m * c * ΔT
Q = 50 g * 4.18 J/g°C * -69.0°C

To convert the final answer to kilojoules (KJ), we divide the result by 1000:

Q = (50 g * 4.18 J/g°C * -69.0°C) / 1000 KJ
Q = -144.27 KJ

Therefore, the amount of heat lost by 50 ml of water going from 70.0°C to 1.0°C is approximately 144.27 KJ.