to solve this we use the formula Q(heat) = mc(change in temp)
so,
Q=(10g)(4.19J/gC)(18-22)
Q=-167.6kJ of heat.
2,641,760J...
The 10 kg of water. This is because the Specific Heat Capacity for water is 9x larger than Iron. The SHC for water is that it takes 1 calorie of water to raise 1 gram by 1 degrees celsius (1C/1gram X 1 degrees celsius) for Iron it takes 0.11 Calories to raise 1 gram by 1 degrees celsius. Therefore meaning since Water has a higher Specific Heat Capacity, it'll take longer to cool down. Just as it requires a large amount of heat to raise the temperature by 1 degrees Celsius, it requires a large amount of heat to drop the temperature by 1 degrres Celsius. - Ataa Ghomashchi
q=mass * Cs * delta T = 0.25kg * 4.18 * (85-10) =78J
If you leave water alone, it is in liquid form. If you raise the temperature of water to boiling, it creates steam. Is this a gas? If you lower the temperature to freezing, it becomes a solid.
114.14g NaCl
mmmm enthalpy
The number of calories required will depend on the mass of water which is to be heated.
42 J
15.37684 joules
2,641,760J...
2,641,760J...
Q=mcΔT Q=14 x 4200 x 21.6 Q=1270080J
3.50 J
raise the temperature of the body by 1 Celsius
1935 J (apex)
10-12
15480.80