The thermochemical equation for the combustion (i.e., burning) of one mole of benzene under standard conditions is
C6H6(l)+15/2O2(g)→6CO2(g)+3H2O(l)
with ΔHocomb=–3267.7kJ/mol
1)
Since ΔH is negative, the reaction is exothermic
Answer: exothermic
2)
mass(C6H6)= 5.00 g
use:
number of mol of C6H6,
n = mass of C6H6/molar mass of C6H6
=(5 g)/(78.11 g/mol)
= 6.401*10^-2 mol
Now use:
Q = number of mol * ΔH
= (6.401*10^-2 mol) * (-3267.7 KJ/mol)
= -209.2 KJ
So,
209.2 KJ is heat released
Answer: 209.2 KJ
The thermochemical equation for the combustion (i.e., burning) of one mole of benzene under standard conditions...
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Write a balanced equation for the combustion of benzene, C6H6(l) . If the standard heat of combustion of benzene is –3271 kJ/mol. Calculate its standard heat of formation, H°f , given the following data: ( 4 pts) H°f [CO2(g)] = –394 kJ; H°f [H2O(l)] = –286 kJ
Butane (C_4H_10) releases 2877 kJ per mole during a standard combustion reaction in air. a. What is the balanced thermochemical equation for this reaction? b. How much heat will be released when 200.0 g of butane is burned?
Heat Capacity and Calorimetry
A sample of ethanol, C2H5OH, weighing 2.84 g was burned in an
excess of oxygen in a bomb calorimeter. The temperature of the
calorimeter rose from 25C to 33.73C. If the heat capacity of the
calorimeter and contents is 9.63kJ/C, what is the value of q for
burning 1.00 lol of ethanol at constant volume and 25.00C.
Is q equal to U or H?
214e Questions and Problems the enthalpy change when 0.710 mol of calcium...
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