The heat liberated on complete combustio...

The heat liberated on complete combustion of 7.8 g benzene is 327 kJ. Calculate heat of combustion measured at constant volume and at `27^@C`.

Text Solution

Verified by Experts

-3270 kJ

Topper's Solved these Questions

STATES OF MATTER (GASES & LIQUIDS)
PATHFINDER|Exercise QUESTION BANK|280 Videos

Similar Questions

Explore conceptually related problems

The amount of heat evolved during complete combustion of 7.8 g benzene at constant volume and 27^(@)C is 3270 kJ. Calculate heat of combustion of benzene at constant pressure and 27^(@)C .

The heat of combustion of benzoic acid at constant volume is -321.3 kJ at 27^@C . The heat of combustion at constant pressure is

At 25^(@)C , heat evolved due to complete combustion of 7.8 g of C_(6)H_(6)(l) is 326.4 kJ. Calculate the heat evolved due to complete combustion of the same amount of C_(6)H_(6)(l) at the same temperature and constant pressure of 1 atm.

Calculate heat of combustion of benzene at constant pressure at 27^@C . (R=8.3 J mol^-1 K^-1)

Given that : (i) heat of formation of water = -68.3 kcal (ii) heat of combustion of acetylene = - 310.6 kcal (iii) heat of combustion of ethylene = - 337.2 kcal. Calculate the heat of reaction for the hydrogenation of acetylene at constant volume (25^(@)C) .

At 25^(@)C , the heat of combustion of naphthalene at constant volume is -1230 " kcal mol"^(-1) . Calculate the heat of reaction at constant pressure and 25^(@)C .

The combustion of benzene (l) gives CO_(2) (g) and H_(2)O (l) . Given that heat of combustion of benzene at constant volume is -3263.9 kJ * mol^(-1) at 25^(@) C , heat of combustion ( in kJ * mol^(-1)) of benzene at constant pressure will be - (R = 8.314 J * K^(-1) * mol^(-1) )

From the following data at constant volume for combustion of benzene, calculate the heat of this reaction at constant pressure condition. C_(6)H_(6(1))+71//2O_(2(g))rarr 6CO_(2(g))+13H_(2)O_((l))

When a gas (molar mass =28g*mol^(-1) ) of mass 3.5 is burnt completely in presence of excess oxygen in a bomb calorimeter, the temperature of the calorimeter increases from 298 K to 298.45 K. the heat of combustion at constant volume for the gas (Given: heat capacity of the calorimeter =2.5kJ*K^(-1) ) is-

PATHFINDER-THERMODYNAMICS-QUESTION BANK

One mole of an ideal gas is heated at constant pressure from 0 o C t...
Text Solution
|
Calculate DeltaH^@ for 2Al+Fe2O3rarr2Fe+Al2O3 given that standard heat...
Text Solution
|
The heat liberated on complete combustion of 7.8 g benzene is 327 kJ. ...
Text Solution
|
Calculate heat of combustion of benzene at constant pressure at 27^@C....
Text Solution
|
The enthalpy change involved in the oxidation of glucose is -2880 kJ m...
Text Solution
|
The heat of formation of ethane is -20.3 kcal. Calculate the bond ener...
Text Solution
|
Calculate the resonance energy of N2O from the following data Delta1 H...
Text Solution
|
The following reaction is performed at 298 K. 2NO(g) + O2(g) rarr 2NO...
Text Solution
|
The standard Gibbs energy change at 300 K for the reaction 2A iff B+C ...
Text Solution
|
For the reaction X2Y4(l) to 2 XY2(g) at 300 K the values of DeltaU and...
Text Solution
|
The values of DeltaH and DeltaS of a certain reaction are -400 kJ mol^...
Text Solution
|
The enthalpy of vaporization of a certain liquid at its boiling point ...
Text Solution
|
Given that The heat of formation of carbon monoxide will be
Text Solution
|
The value of DeltaH for cooling 2 mole of an ideal monoatomic gas from...
Text Solution
|
For a spontaneous process, the correct statement(s) is (are)
Text Solution
|
Which of the following statements is correct for the spontaneous absor...
Text Solution
|
For the reaction X2O4(l) to 2XO2(g), DeltaU = 2.1 kcal, DeltaS = 20 ...
Text Solution
|
The ratio of heats liberated at 298K from the combustion of one kg of ...
Text Solution
|
Conversion of oxygen into ozone is non-spontaneous at
Text Solution
|
For an ideal binary liquid mixture
Text Solution
|