calculate required heat energy (q)to change 10g of water from 30⁰ ti 40⁰(specific heat of water =1)
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Answer:
Calculate the heat lost by the water, Q, according to the equation Q = m * c * deltaT, where m represents the mass of water and c represents water's specific heat capacity, or 4.184 joules per gram degree Celsius.
Explanation:
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Answer:
Calculate the heat lost by the water, Q, according to the equation Q = m * c * deltaT, where m represents the mass of water and c represents water's specific heat capacity, or 4.184 joules per gram degree Celsius. The specific heat capacity of water is 4,200 Joules per kilogram per degree Celsius (J/kg°C). This means that it takes 4,200 J to raise the temperature of 1 kg of water by 1°C. Lead will warm up and cool down fastest because it doesn't take much energy to change its temperature.The quantitative relationship between heat transfer and temperature change contains all three factors: Q=mcΔT Q = mc Δ T , where Q is the symbol for heat transfer, m is the mass of the substance, and ΔT is the change in temperature. The symbol c stands for specific heat and depends on the material and phase.Calculate the kilowatt-hours (kWh) required to heat the water using the following formula: Pt = (4.2 × L × T ) ÷ 3600. Pt is the power used to heat the water, in kWh. L is the number of liters of water that is being heated and T is the difference in temperature from what you started with, listed in degrees Celsius.
Enthalpy of Solution (Heat of Solution) Example
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Calculate the enthalpy change, ΔH, in kJ mol-1 of solute:
Water's heat of vaporization is around 540 cal/g at 100 °C, water's boiling point. Note that some molecules of water – ones that happen to have high kinetic energy – will escape from the surface of the water even at lower temperatures.
Explanation: