the following equations is the balanced combustion reactions for c6h6
2C6H6(l)+15O2---->12CO2(G)+6H20(l)+6542 k j
if 7.700 g of C6H6is burned and the heat produced from the burning is added to 5691 g of water at 21 c what is the final temperature of the water?
Molar mass of C6H6,
MM = 6*MM(C) + 6*MM(H)
= 6*12.01 + 6*1.008
= 78.108 g/mol
mass(C6H6)= 7.700 g
use:
number of mol of C6H6,
n = mass of C6H6/molar mass of C6H6
=(7.7 g)/(78.11 g/mol)
= 9.858*10^-2 mol
Since Δ H is negative, heat is released
when 2 mol of C6H6 reacts, heat released = 6542.0 KJ
So,
for 9.858*10^-2 mol of C6H6, heat released = 9.858*10^-2*6542.0/2 KJ
= 322.5 KJ
= 322500 J
This heat is absorbed by water
Given:
Q = 322500 J
m = 5691 g
C = 4.184 J/g.oC
Ti = 21 oC
use:
Q = m*C*(Tf-Ti)
322500 = 5691*4.184*(Tf-21)
Tf -21.0 = 13.5 oC
Tf = 34.5 oC
Answer: 34.5 oC
the following equations is the balanced combustion reactions for c6h6 2C6H6(l)+15O2---->12CO2(G)+6H20(l)+6542 k j if 7.700 g...
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