Please answer these questions on your Page 7 (a) ) We place 88.8 g of a metal at 10.00°C in 333.3 g of water at 90.00°C. The water is in a beaker that is also at 90.00°C. The specific heat of water is 4.184 J K-¹g-¹. The heat capacity of the beaker is 0.888 kJ K-¹. The final temperature is 88.15°C. What is the specific heat of the metal?

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Chapter1: Chemical Foundations
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Please answer these questions on your Page 7
(a)
) We place 88.8 g of a metal at 10.00°C in 333.3 g of water at 90.00°C. The water is in a
beaker that is also at 90.00°C. The specific heat of water is 4.184 J K-¹g-¹. The heat capacity of
the beaker is 0.888 kJ K−¹. The final temperature is 88.15°C. What is the specific heat of the metal?
(b)
) For the reaction 2 A(g) → A₂(g), Q = −45.00 kJ for the formation of one mole of A₂(g)
at constant volume and a temperature of 25.00°C. If we did this same reaction at constant
pressure, what would be the values of Q, W, AU, and AH for the formation of one mole of A2 (g)
at a temperature of 25.00°C?
Transcribed Image Text:Please answer these questions on your Page 7 (a) ) We place 88.8 g of a metal at 10.00°C in 333.3 g of water at 90.00°C. The water is in a beaker that is also at 90.00°C. The specific heat of water is 4.184 J K-¹g-¹. The heat capacity of the beaker is 0.888 kJ K−¹. The final temperature is 88.15°C. What is the specific heat of the metal? (b) ) For the reaction 2 A(g) → A₂(g), Q = −45.00 kJ for the formation of one mole of A₂(g) at constant volume and a temperature of 25.00°C. If we did this same reaction at constant pressure, what would be the values of Q, W, AU, and AH for the formation of one mole of A2 (g) at a temperature of 25.00°C?
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