The enthalpy of combustion of $C_{6} H_{6}$ $(l)$ is $3250 k J$ . When $0.39 g$ of benzene is burnt in excess of oxygen in an open vessel, the amount of heat liberated is:

16.25 J

No worries! We‘ve got your back. Try BYJU‘S free classes today!

16.25 kJ

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

32.5 J

No worries! We‘ve got your back. Try BYJU‘S free classes today!

32.5 kJ

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is B 16.25 kJ
Molecular weight of $C_{6} H_{6} = 78 g m o l^{- 1}$

Heat liberated when,

$78 g C_{6} H_{6}$ burned $= 3250 k J$

$0.39 g C_{6} H_{6}$ burned $= x k J$

$x = \frac{0.39 \times 3250}{78}$

$x = 16.25 k J$

Hence, te correct option is $B$

Suggest Corrections

Similar questions

The enthalpy of combustion of C $_{6}$ H $_{6}$ $(l)$ is -3250 kJ. When 0.39 g of benzene is burnt in excess of oxygen in an open vessel, the amount of heat liberated is:

Q. The heat evolved in the combustion of benzene is given by

C_{6} H_{6} (l) + 7 \frac{1}{2} O_{2} (g) \to 3 H_{2} O (l) + 6 C O_{2} (g), Δ H = - 781.0 K c a l m o l^{- 1}

When

156

g of

C_{6} H_{6}

is burnt in an open container, the amount of heat energy released will be

Q. The enthalpy of combustion of methane at

25^{\circ} C

890

kJ. The heat liberated when

3.2

g of methane is burnt in air is:

When 6 g carbon is burnt in a sufficient amount of oxygen, the heat evolved is $x$ kJ. The heat of combustion of carbon is :

Join BYJU'S Learning Program

The enthalpy of combustion of C6H6 (l) is 3250 kJ. When 0.39 g of benzene is burnt in excess of oxygen in an open vessel, the amount of heat liberated is:

The correct option is B 16.25 kJMolecular weight of C6H6=78g mol−1Heat liberated when,78 g C6H6 burned =3250kJ0.39 g C6H6 burned =xkJx=0.39×325078x=16.25 kJHence, te correct option is B

The enthalpy of combustion of $C_{6} H_{6}$ $(l)$ is $3250 k J$ . When $0.39 g$ of benzene is burnt in excess of oxygen in an open vessel, the amount of heat liberated is:

The correct option is B 16.25 kJ
Molecular weight of $C_{6} H_{6} = 78 g m o l^{- 1}$

Heat liberated when,

$78 g C_{6} H_{6}$ burned $= 3250 k J$

$0.39 g C_{6} H_{6}$ burned $= x k J$

$x = \frac{0.39 \times 3250}{78}$

$x = 16.25 k J$

Hence, te correct option is $B$