Hello, The problems below I\'ve completed, but the online homework system says m
ID: 791428 • Letter: H
Question
Hello,
The problems below I've completed, but the online homework system says my answers are incorrect. A few of these are basic, but perhaps I'm missing a step? I would like to see what answers you come up with and compare them to mine and see if I can figure it out before I ask a tutor.
1) One piece of copper jewelry at 101
The problems below I've completed, but the online homework system says my answers are incorrect. A few of these are basic, but perhaps I'm missing a step? I would like to see what answers you come up with and compare them to mine and see if I can figure it out before I ask a tutor. One piece of copper jewelry at 101 degree C has exactly twice the mass of another piece, which is at 36.0 degree C. Both pieces are placed inside a calorimeter whose heat capacity is negligible. What is the final temperature inside the calorimeter (c of copper = 0.387 J/g middot K)? When 34.0 mL of 0.530 M H2SO4 is added to 34.0 mL of 1.06 M KOH in a coffee-cup calorimeter at 23.50 degree C, the temperature rises to 30.17 degree C. Calculate Delta H of this reaction per mole of H2SO4 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/g times K.) Delta H per mole of H2SO4 reacted in kJ/mol?: Delta H per mole of KOH reacted in kJ/mol?: Use the following information to find Delta H degree f of ethanol [CH3CH2OH(l)]. CH3CH2OH(l) + 3 O2(g) rightarrow 2 CO2(g) + 3 H2O(g) A 26.8 g sample of ethylene glycol, a car radiator coolant, loses 667 J of heat. What was the initial temperature of ethylene glycol if the final temperature is 32.5 degree C (c of ethylene glycol = 2.42 J/g middot K)?Explanation / Answer
can you tell me the course code so I can help you..
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