a) We place 125.0 g of a metal at 5.00°C in 350.0 g of water at 100.00°C. The water is in a beaker also at 100.00°C. The specific heat of the water is 4.184 J K-1 g-1. The specific heat of the metal is 0.609 J K-1 g-1. The heat capacity of the beaker is 0.888 kJ K-1. What will be the final temperature of the water, beaker and metal? b) For the reaction: A(g) → 3 B(g), Q = 52.0 kJ for the decomposition of 1.00 mol of A(g) under constant volume conditions and at a temperature of 25.0 °C. If the same reaction takes place under conditions of constant pressure, what will be the values of Q, W, H and U for the decomposition of 1.00 mol of A(g) at a temperature of 25.0 °C.

a) We place 125.0 g of a metal at 5.00°C in 350.0 g of water at 100.00°C. The water is in a beaker also at 100.00°C. The specific heat of the water is 4.184 J K-1 g-1. The specific heat of the metal is 0.609 J K-1 g-1. The heat capacity of the beaker is 0.888 kJ K-1. What will be the final temperature of the water, beaker and metal?

b) For the reaction: A(g) → 3 B(g), Q = 52.0 kJ for the decomposition of 1.00 mol of A(g) under constant volume conditions and at a temperature of 25.0 °C. If the same reaction takes place under conditions of constant pressure, what will be the values of Q, W, H and U for the decomposition of 1.00 mol of A(g) at a temperature of 25.0 °C.