5. 14 points My Notes Ask Your Teacher A 30.5 g sample of an alloy at 93.6°C is

Question

5. 14 points My Notes Ask Your Teacher A 30.5 g sample of an alloy at 93.6°C is placed into 44.7 g water at 23.4°C in an insulated coffee cup. The heat capacity of the coffee cup (without the water) is 9.2 J/K. If the final temperature of the system is 31.1°C, what is the specific heat capacity of the alloy? (c of water is 4.184 /gxK) Submit Answer 6. -/4 points My NotesAsk Your Teacher when 32.0 mL of 0.655 M H2SO4 is added to 32.0 mL of 1.31 M KOH in a coffee-cup calorimeter at 23.50°C, the temperature rises to 30.170C. Calculate of this reaction per mole of H2S04 and KOH reacted. (Assume that the total volume is the sum of the individual volumes and that the density and specific heat capacity of the solution are the same as for pure water: d = 1.00 g/mL and c = 4.184 J/gK.) per mole of H2SO4 reacted: kJ/mol AH per mole of KOH reacted kJ/mol 49D

Explanation / Answer

heat lost by the alloy = heat gained by the water & cup

m C dT alloy = m C dT water & C dT cup

(30.5 g )(C)(93.6 - 31.1) = (44.7 g)(4.184 J/g-C)(31.1 - 23.4) + (9.2J/C)(31.1 - 23.4)

(30.5 g )(C)(62.5) = (44.7 g)(4.184 J/g-C)(7.7) + (9.2J/C)(7.7)

1906.25 C = 1440.091 + 70.84

C = 1510.931 / 1906.25

C = 0.792 J/g-K

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