How much energy would be required to raise the temperature of 1.25g of water from 17 to 31 degree celsius.

To calculate the energy required to raise the temperature of a substance, you can use the specific heat capacity (C) formula:

Q = m * C * ΔT

Where:
Q is the energy required (in joules),
m is the mass of the substance (in grams),
C is the specific heat capacity of the substance (in J/g°C), and
ΔT is the change in temperature (in °C).

For water, the specific heat capacity (C) is approximately 4.18 J/g°C.

Now, let's calculate the energy required to raise the temperature of 1.25g of water from 17 to 31 degrees Celsius.

First, find the change in temperature:
ΔT = Final temperature - Initial temperature
= 31°C - 17°C
= 14°C

Next, substitute the values into the formula:

Q = 1.25g * 4.18 J/g°C * 14°C
= 73.325 J

Therefore, it would require approximately 73.325 joules of energy to raise the temperature of 1.25 grams of water from 17 to 31 degrees Celsius.