c10q12-2 Chapter West Virginia University Dr. Robert Belford

Question 1
 How much heat (in Joules) is required to raise 32.6 g of Al(s) from 0.0oC to 100.0oC. (A)  3KJ (B)  2.9KJ (C)  2.94KJ (D)  2,939J Hint

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Question 2
 How much heat is required to raise 28.4 g of Copper from 25.0oC to 350.0oC. (A)  3.55KJ (B)  4.41 KJ (C)  849J (D)  2.36 KJ Hint

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Question 3
 A 2.36 g sample of unknown material changes temperature from 27.4oC to 39.4oC after 1.79 J of heat are added. What is the heat capacity of this material? (A)  9.10 J/g.oc (B)  9.1 J/g.oc (C)  0.063 J/g.oc (D)  0.0632 J/g.oc Hint

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Question 4
 A 2.27 g sample of unknown material changes temperature from 12.5oC to 98.7oC after 98.0 J of heat are added. What is the heat capacity of this material? (A)  2.36 J/g.oc (B)  2.87 J/g.oc (C)  0.500 J/g.oc (D)  5.34 J/g.oc Hint

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Question 5
 A 74.9 g sample of silver at 25.0oC gains 319 J of heat. What is the final temperature of the silver? The specific heat capacity of silver is 0.236J/g0C. (A)  34.0 oC (B)  198oC (C)  43.0 oC (D)  388oC Hint

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Question 6
 A 2.40 g sample of Iron at 10.00oC gains 250 J of heat. What is the final temperature of the iron? (A)  240.8oC (B)  128oC (C)  567oC (D)  241oC Hint

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Question 7
 An unknown mass of copper at 98.2 oC is placed in 50.0 g of water at 24.0oC. What is the mass of the copper if the final temperature is 29.8oC? (A)  46.1g (B)  36.4g (C)  88.3g (D)  46g Hint

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Question 8
 An unknown mass of iron at 354 oC is placed in100.0 g of water at 0.0oC. What is the mass of the iron if the final temperature is 78.0oC? (A)  138g (B)  2.62g (C)  26.2g (D)  262g Hint

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Question 9
 What is the density of gaseous Fl2 at 0.50 atm and 189oC? (A)  2.8g/L (B)  7.8g/L (C)  0.50g/L (D)  1.2g/L Hint

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Question 10
 How much heat in Joules is required to melt 32.2 g of ice at 0.0oC? (A)  10.7KJ (B)  2.57KJ (C)  17.4KJ (D)  72.7KJ Hint

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Question 11
 How much heat in Joules is required to boil 32.2 g of water at 100.0oC? (A)  10.7 KJ (B)  2.57 KJ (C)  17.4KJ (D)  72.7 KJ Hint

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