How much total heat, in kJ, does it take to heat 82.58 grams of ice at 0°C to 91.36°C?   cwater = 4.184 J/g°C ΔHvap = 2260 J/g ΔHfus = 334 J/g

Ethanol, C₂H5OH, boils at 78.29 °C. How much energy, in joules, is required to raise the temperature of 3.00 kg of ethanol from 43.0 °C to the boiling point and then to change the liquid to vapor at that temperature? (The specific heat capacity of liquid ethanol is 2.44 J/g. K, and its enthalpy of vaporization is 855 J/g.) Energy required = J

Based on enthalpy of formation data species∆H◦fH2S(g)−20.63 kJ/molO2(g)0 kJ/molH2O(ℓ)−285.83 kJ/molSO2(g)−296.83 kJ/mol calculate ∆Hrxnfor2 H2O(ℓ) + 2 SO2(g)←→2 H2S(g) + 3 O2(g) 1.562 kJ·mol−1 3 2.−562 kJ·mol−1 3.−1124 kJ·mol−1 4.1124 kJ·mol−1

A 12.5-g sample of granite initially at 82.0 °C is immersed into 25.0 g of water that is initially at 22.0 °C. What is the final temperature of both substances when they reach thermal equilibrium? (For water, Cs = 4.18 J/g ⋅ °C and for granite, Cs = 0.790 J/g ⋅ °C.)

Which substance will have the largest temperature change if the same amount of heat is added to each of them?Gold, Au(s): specific heat = 0.0308 calories per gram degree Celsius.Water, H2O(l): specific heat = 1.00 calorie per gram degree Celsius.Copper, Cu(s): specific heat = 0.0920 calorie per gram degree Celsius.Ethanol, C2H5OH(l): specific heat = 0.588 calorie per gram degree Celsius

12.4 grams of ethanol are heated from 14.5°C to 117.6°C how many joules of energy were required?  Ethanol heat of vaporization is ΔH(vap) 38.6 kJ/mol and heat of fusion is ΔH(fus) 4.60 kj/mol. Specific heats for the three phases of ethanol are: cp (liquid) ethanol 2.46 J/g°C, cp (gas) ethanol 1.43 J/g°C, cp (solid) ethanol 2.42 J/g°C. Ethanol is 46.0 g/mol.  The melting point of ethanol is -114.1 °C and the boiling point is 78.4 °C.

A sample of water with a mass of 726.2 g undergoes a temperature change from 58.3°C to 40.50°C. What is the heat change in Joules?  (Specific Heat of H2O (l) = 4.184 J/g∙°C)

How hot does a thanksgiving dinner roll need to be to warm up and melt a 4.0 g 'pat' of butter? (Roll: 25 g, Csteam= 1.996 J/g°C; Tr = 32°C; Butter: Ti = 2.0°C, Tr = 32°C, Cbutter = 2.72 J/g°C, Hfusion = 32 J/g). [Remember, heat lost by roll equals heat gained by butter. Assume the specific heat of the roll is the same as the %3D specific heat of steam.]

The specific heat capacity of liquid mercury is 0.14 J/g-K. How many kilojoules of heat are needed to raise the temperature of 9.00 g of mercury from 25.1 °C to 65.3 °C?

Calculate the amount of heat (in J) needed to warm up 250. g of silver from 45.0° C to 67.0°C.