to have 500ml of water, how many joules of energy will be required to change the temperature from 25°C to 95°C

Answer 1

The specific heat of water is 4.184 J/g C.

Since water's density is 1 g/ mL, 500 mL of water will have a mass of 500 g.

The equation to calculate the joules of energy required is:
heat = mass x specific heat x change in temperature

energy = 500 (4.184)(95-25)
energy = 146440 J or 146.44 kJ

Hope that helped.

Answer 2

Energy = mass * specific heat * change in temperature

Assuming a density of 1 g/ml, 500 ml = 500 g

Energy = 500 g * (4.184 J / g C) * 70 C = 146,440 J or 146 kJ

Answer 3

If I recall, a calorie is the amount of energy needed to heat one gram of water one degree centigrate. If you assume the water to have a density of 1g/ml, then the math is just 500*70=35,000 calories. Now all you have to do is convert from joules to calories (4.186 joules=1 calorie) which gives you 146.5 kilojoules.

Answer 4

Energy required = mass of water x specific heat capacity x change in temperature

SHC of water = 4200 J/Kg/K
1000ml of water = 0.5 Kg of water

Q= 0.25 x 4200 x (95-25)
Q = 73500 J