Suppose that a 17.70 gram ball of metal initially at 84.1°C is added to 18.28 grams of an unknown liquid initially at 20.1°C. Assume that the specific heat of the metal is 1.33 J/(g·°C) and the specific heat of the liquid is 3.15 J/(g·°C).
What is the final temperature of the metal in °C? Report your answer to three decimal places.
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Connect the whole numbers on the periodic table to indicate what they represent?
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Given the following at 25c calculate delta hf for hcn (g) at 25c. 2nh3 (g) +3o2 (g) + 2ch4 (g) > 2hcn (g) + 6h2o (g) delta h rxn= -870.8 kj. delta hf=-80.3 kj/mol for nh3 (g), -74.6 kj/mol for ch4, and -241.8 kj/mol for h2o (g)
Answers: 1
Suppose that a 17.70 gram ball of metal initially at 84.1°C is added to 18.28 grams of an unknown li...
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