calculate the amount of heat in Joules required to heat 3.5kg of gold of bar from 21°C to 67°C (sp heat of gold =0.128j/g°C

calculate the amount of heat in Joules required to heat 3.5kg of gold of bar from...
Calculate the amount of heat required to heat a 3.5-kg gold bar from 21 degree C to 67 degree C.
What change in temperature results when 2500 Joules of heat is applied to a 7.00 gram bar of gold? Specific heat is 0.129 J/g degree Celsius Calculate the heat transferred from a 5.5 g iron nail that is cooled from 37.0 degrees Celsius to 25.0 degrees Celsius? The specific heat of iron is 0.450 J/g degree C
Calculate the quantity of heat energy, in Joules, that is absorbed when a gold (.128J/goC) ring with a mass of 12.68 is warmed from 23.2 oC to 58.1 oC. Report your answer, in J, using the correct number of significant figures. Do not enter units and do not use scientific notation.
Calculate the amount of heat in J required to increase the temperature of 25.0 grams of water from 25. °C to 50.0 °C. ice Specific Heats of Common Substances at 25 °C and 1 bar Substance Symbol Specific Heat (J/g (state) °C) helium He(s) 5.193 water H2O(1) 4.184 ethanol C2H60(1) 2.376 H2O(s) 2.093 (at -10 °C) water vapor H2O(g) 1.864 nitrogen N2(8) 1.040 air 1.007 oxygen O2(8) 0.918 aluminum Al(s) 0.897 carbon CO2(8) 0.853 dioxide argon Ar(s) 0.522 iron Fe(s)...
How much heat in joules is required to heat a 50 g sample of aluminum from 70 ∘F to 141 ∘F? (The specific heat capacity of aluminum is 0.903 J/(g⋅∘C).) Express your answer using two significant figures.
Calculate the heat required in Joules to convert 18.0 grams of water ice at a temperature of -20° C to liquid water at the normal boiling point of water. Given: -specific heat of ice = 2.09 J/g°C -specific heat of liquid water = 4.184 J/g°C -specific heat of water vapor = 2.03 J/g°C -molar heat of fusion of water = 6.02 kJ/mol -molar heat of vaporization of water = 40.7 kJ/mol
At 25°C, 230 joules of heat is added to 10.0-g samples of pure gold and copper. Which metal has a higher final temperature?
8. Calculate the amount of heat (in kJ) required to heat 1.01 kilogram of water from 5°C to 35.81°C. [Specific heat of water-4.184J/g.°C] A metal ball with a mass of 100.0 g was heated to a temperature of 88.4°C and then dropped into 125 g water originally at 25.1°C. The final temperature of both the metal ball and the water is 31.3°C. Calculate the specific heat capacity (s) of the metal. [Specific heat capacity of water = 4.184J/g.°c).
Calculate the amount of heat required to heat a 50 kg sample of ethanol from 11.0 ∘C to 19.0 ∘C. Specific heat capacity of ethanol is 2.42 J/g∘C. Express your answer using two significant figures.
Calculate the amount of heat (in kJ) required to heat 255 g of water from 25.2 0C to 90.5 0C. (Cs = 4.18 J/g 0C for water)