A 1.34 g sample of caffeine (C8H10N4O2) burns in a constant-volume calorimeter that has a heat...
A 1.34 g sample of caffeine (C8H10N4O2) burns in a constant-volume calorimeter that has a heat capacity of 7.71 kJ/K. The temperature increases from 297.65 K to 302.07 K. Determine the heat (qv) associated with this reaction. 1476 kJ/mol
Now use the data above to find ΔE for the combustion of one mole of caffeine.
Homework Answers
qv = mSdT
= 7.71 KJ/K * (302.07-297.65)
= 34.078 KJ
Now mole of caffeine present = 1.34/ 194 = 6.9*10^-3 moles
so heat per mole = 34.078/ 6.9*10^-3 = 4933.68 KJ/mole
Add Answer to:
A 1.34 g sample of caffeine (C8H10N4O2) burns in a
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A 2.47 g sample of caffeine
(C8H10N4O2) burns in a
constant-volume calorimeter that has a heat capacity of 7.86 kJ/K.
The temperature increases from 297.65 K to 305.65 K. Determine the
heat (qv) associated with this reaction.
Now use the data above to find ΔE for the combustion of one mole
of caffeine.
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A 2.47 g sample of caffeine
(C8H10N4O2) burns in a
constant-volume calorimeter that has a heat capacity of 7.86 kJ/K.
The temperature increases from 297.65 K to 305.65 K. Determine the
heat (qv) associated with this reaction.
Now use the data above to find ΔE for the combustion of one mole
of caffeine.
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please solve both if possible
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