Want this question answered?
4.1858 joules of energy will raise the temperature of 1 g of water by 1oC. Thus, 4.1858 * 955 * 80 = 319795.12 joules of energy is required to raise the temperature of 955 g of water by 1oC.
The needed heat is 47,65 Joules.
Using the formula Q=mcΔT, the amount of heat energy required is (82g)(4.18J g-1 K-1)(42K) = 14400J.
The evaporation of water is endothermic. In order for the hydrogen bonds to be broken in water (which is required for water to evaporate), an input of energy is needed. Conversely, the condensation of water vapor is exothermic.
The heat of vaporization is about 2258 joules/gram46 x 2258 = 103,868 J ~ 103.9 kJ(Using the rounded value 2260 joules per gram, about 104 kJ)it is already at boiling point so in theory zero energy is required.I think the question is asking what energy is required to free the water from its liquid state to the vapour state.At 101325Pa, (1 atmosphere in old money), the latent heat of evaporation of water is 2256.7 J/g.So 2256.7 * 46 = 103808 Joules
4.1858 joules of energy will raise the temperature of 1 g of water by 1oC. Thus, 4.1858 * 955 * 80 = 319795.12 joules of energy is required to raise the temperature of 955 g of water by 1oC.
Evaporation because it requires 2,260 Joules to gain heat energy. Condensation, freezing, and melting require less Joules than evaporation.
15480.80
1 BTU is the energy required to heat 1 pound of water by 1 degree F. 1 Joule is defined mechanically, but in thermal terms it is 1/4.2 of a calorie (4.2 Joules/calorie), and 1 calorie is the energy required to heat 1 gram of water by 1 degree C. In fact 1 BTU = 1055 Joules.
Energy required to raise 1 gramme of water by 1 degree C = 1 calorie also, 1 calorie = 4.186 Joules
4.184 J/g/K = 4.184 x 150 x (318-274) = 27614 Joules
Generally it isn't, diffusion is a process that requires no energy.
The energy required to raise the temperature of water depends on the atmospheric pressure as well as the starting temperature. At a pressure of one atmosphere, the amount of energy required to raise the temperature of water from 0 deg C to 100 deg C (32 to 212 deg F) is 4.19 joules per gram. At 4 deg C, (39.2 deg F) it is approx 4.204 joules per gram per deg C. That is 4.204/1.8 = 2.33555... recurring joules per gram per deg F and so, for a kilogram, the energy required is 2335.55... joules.
334.8 Joules
Energy is released.
To raise the temperature of both an equal amount, water would require more energy. In terms of the energy required to raise the temperature: iron = 0.45 joules / gram . kelvin water = 4.2 joules / gram . kelvin This is known as the specific heat capacity of a material
The needed heat is 47,65 Joules.