Question 3: (a) (6 points) We place 120.0 g of a metal at 80.00oC in 436.3...

Question:

Question 3:

(a) (6 points) We place 120.0 g of a metal at 80.00oC in 436.3 g of water at 25.00oC. The water is in a beaker that is also at 25.00oC. The specific heat of water is 4.184 J K-1 g-1 and the heat capacity of the beaker is 0.6666 kJ K-1. The specific heat capacity of the metal is 0.4444 J K-1 mol-1. What is the final temperature of the metal, the water, and the beaker?

(b) (3 points) For the decomposition of exactly one mole of a solid, X(s),

X(s) → Y(s) + 2 Z(g)

under a constant pressure of 1.00 atm and a temperature of 25.0oC, the value of ΔH is 58.6 kJ. What are the values of ΔU, Q, and W for this decomposition under these conditions?

Question 3: (a) (6 points) We place 120.0 g of a metal at 80.00°C in 436.3 g of water at 25.00°C. The water is in a beaker that is also at 25.00°C. The specific heat of water is 4.184 J K-1g-1 and the heat capacity of the beaker is 0.6666 kJ K-1. The specific heat capacity of the metal is 0.4444 J K-1 mol-!. What is the final temperature of the metal, the water, and the beaker? (b) (3 points) For the decomposition of exactly one mole of a solid, X(s), X(s) → Y(s) + 2 Z(9) under a constant pressure of 1.00 atm and a temperature of 25.0°C, the value of AH is 58.6 kJ. What are the values of AU, Q, and W for this decomposition under these conditions?

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