a) A system does work on the surroundings equal to 64 J and the change in energy is -213 J. Calculate the heat J
b) If 6.40 kJ of heat is needed to raise the temperature of a sample of metal from 14°C to 28°C, how many kilojoules of heat will be required to raise the temperature of the same sample of metal from 31°C to 54°C?
c) If 137 J of heat is applied to a 34 g sample of mercury, how many degrees will the temperature of the sample of mercury increase?
d) What quantity of heat is required to raise the temperature of 57.4 g of gold from 27°C to 66°C?
e) For the reaction below ÎH = -296 kJ per mole of SO2 formed.
S(s) + O2(g) â SO2(g)
(1) Calculate the quantity of heat released when 1.45 g of sulfur is burned in oxygen.
(2) Calculate the quantity of heat released when 0.522 mol of sulfur is burned in air.
(3)What quantity of energy is required to break up exactly 4 mol of SO2(g) into its constituent elements?
a) A system does work on the surroundings equal to 64 J and the change in energy is -213 J. Calculate the heat J
b) If 6.40 kJ of heat is needed to raise the temperature of a sample of metal from 14°C to 28°C, how many kilojoules of heat will be required to raise the temperature of the same sample of metal from 31°C to 54°C?
c) If 137 J of heat is applied to a 34 g sample of mercury, how many degrees will the temperature of the sample of mercury increase?
d) What quantity of heat is required to raise the temperature of 57.4 g of gold from 27°C to 66°C?
e) For the reaction below ÎH = -296 kJ per mole of SO2 formed.
S(s) + O2(g) â SO2(g)
(1) Calculate the quantity of heat released when 1.45 g of sulfur is burned in oxygen.
(2) Calculate the quantity of heat released when 0.522 mol of sulfur is burned in air.
(3)What quantity of energy is required to break up exactly 4 mol of SO2(g) into its constituent elements?
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