Home
Class 11
CHEMISTRY
19.5 g of benzene on burning in the free...

19.5 g of benzene on burning in the free supply of oxygen liberated 12.6 kJ of energy at constant pressure. Calculate the enthalpy of combustion of benzene. Write the thermochemical equation. 

Text Solution

Verified by Experts

19.5 grams of benzene on burning liberated 126 kl. 78 grams of benzene on burning liberated 502 kJ.
The enthalpy of combustion of benzene is` -502 kJ mol ^(-1).` The thermochemical equation is given as,
`C _(6) H _(6(l)) + (15)/(2) O _(2(g)) to 6CO _(2(g)) + 3H_(2(g)) + 3H _(2) O _((l)), Delta H =-502 kJ mol ^(-1)`
Promotional Banner

Similar Questions

Explore conceptually related problems

The heat of combustion of benzene at 27^@C and at constant volume is -3245 KJ. Then the heat of combustion of benzene at the same temperature and at constant pressure

The combustion of one mole of benzene takes place at 298 and 1 atm. After combustion, CO_(2)(g) and H_(2)O(l) are produced and 3267.0 kJ of heat is liberated. Calculate the standard enthalpy of formation. triangle_f H^@ benzene. Standard enthalpies of formation of CO_2(g) and H_20(l) are -393,5 kJ mol ""^(-1) and "-285.83 kJ mol"^(-1) respectively.

At constant pressure, the heat of combustion of carbon monoxide at 17^0 C is –284.5 kJ. Calculate its heat of combustion at constant volume

2 g of benzoic acid (C_(6)H_(5)COOH) dissolved in 25g of benzene shows a depression in freezing point equal to 1.62 K. Molal depression constant for benzene is 4.9 K kg "mol"^(-1) . What is the precentage association of acid if it forms dimer in solution ?

Change in enthalpy and change in internal energy are state functions. The value of DeltaH, DeltaU can be determined by using Kirchoff's equation. Calculate the heat of formation of methane, given that heat of formation of water = -286kJ mol^(-1) , heat of combustion of methane = -890kJ mol^(-1) heat of combustion of carbon = -393.5 kJ mol^(-1)

2.0 g of a non-electrolyte solute dissovled in 100 g of benezene lowered the freezing point of benzene by 0.4^@C . If the freezing point depression constant of benezene is 5.12 K kg mol^(-1) . Calculate the molar mass of solute.

How many litres of oxygen (at STP) are required for complete combustion of 39 g of liquid benzene? (Atomic weights:C=12,0=16,H=1)

2.0g of a non-electrolyte dissolved in 100g of benzene lowers the freezing point of benzene by 1.2K. The freezing pont depression constant of benzene is 5.12 K kg mol^(-1) . The molar mass of the solute is