Question

I put down all the info that I found but I cant figure out the questions 1 & 2 at the bottom!!

Empty Calorimeter- 11.6 g
Room temp - 21 degrees celcius
Three different experiments of 50mL 1(M) HCl reacts with 0.15 g Mg, 0.25g Mg, and 0.35g Mg respectively.
The maximum temperatures after reaction were, 29.27 degrees Celcius, 34.78 degrees Celcius and 40.29 degrees celcius. Which makes deltaT 8.27, 13.78, and 19.29.
The weight after reaction minus the empty calorimeter is: 49.957g, 50.049g, and 50.141g.

1.Calculate the number of moles reacted in the three experiments (MW= 24.305 g/mol)
2.Calculate the heat released into the solution for the 3 reactions, according to:
3. Find the molar heat of reaction for each experiment in units of Joules / (mole of Mg) by dividing the heat of reaction by the moles of Mg used.

4. Calculate and record the average molar heat of reaction from the three results.


q(reaction) = Ccal * Delta T + mass(contents) * Cp (contents) * deltaT
assume that calorimeter constant is 0

Answer 1

Note the correct spelling of celsius.
1. moles Mg = grams Mg/molar mass Mg.
2. q = heat released = mass water x specific heat water x delta T. Note that the answer to 2 is note at bottom (after question 4) "q(reaction) = ...._"