A 7.3-g copper coin is at a temperature of 18.8°C. This coin is placed in 10.0 g of water at a temperature of 54.0°C. What is the final temperature of the coin and water, assuming no heat is lost to the surroundings? Specific heat of water is 4.184 J/g*°C and specific heat of copper is 0.385 J/g*°C.

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8. A 7.3-g copper coin is at a temperature of 18.8°C. This coin is placed in 10.0 g of water at a
temperature of 54.0°C. What is the final temperature of the coin and water, assuming no heat is
lost to the surroundings? Specific heat of water is 4.184 J/g*°C and specific heat of copper is
0.385 J/g *°C.
9. The K, value of the reaction
N₂O4 =2NO₂ (g)
is 0.113. What is the Gibbs free energy, AG, of the reaction if the initial pressure of N₂O4 is 1.23
atm while NO₂ is 0.750 atm? Is the process spontaneous?
10. The molar heat of vaporization of ammonia is 23.4 kJ/mol while its boiling point is -33.34 °C.
Calculate the AS for the vaporization of 0.75 moles of ammonia. Express your answer with unit
J/K.
Transcribed Image Text:8. A 7.3-g copper coin is at a temperature of 18.8°C. This coin is placed in 10.0 g of water at a temperature of 54.0°C. What is the final temperature of the coin and water, assuming no heat is lost to the surroundings? Specific heat of water is 4.184 J/g*°C and specific heat of copper is 0.385 J/g *°C. 9. The K, value of the reaction N₂O4 =2NO₂ (g) is 0.113. What is the Gibbs free energy, AG, of the reaction if the initial pressure of N₂O4 is 1.23 atm while NO₂ is 0.750 atm? Is the process spontaneous? 10. The molar heat of vaporization of ammonia is 23.4 kJ/mol while its boiling point is -33.34 °C. Calculate the AS for the vaporization of 0.75 moles of ammonia. Express your answer with unit J/K.
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