When hydrogen gas is burnt in chlorine, 2000 cals of heat is liberated during the formation of 3.65 g of HCl. $Δ$ H of formation of HCl is:

2

Kcal

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

- 20

Kcal

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

+ 20

Kcal

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

- 2

Kcal

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

Open in App

Solution

The correct option is B $- 20$ Kcal
for 3.65 g of HCl 2000 cals of heat
3.65 g $= \frac{3.65}{1 + 35.5} = \frac{3.65}{36.5} = \frac{1}{10}$ moles
for $\frac{1}{10}$ moles ----- 2000 cals
for 1 mole ----- 20 K cals
$∴ Δ H$ of formation of HCl $=$ -20 Kcals
As heat is liberated $Δ H =$ - ve

Suggest Corrections

Similar questions

H_{2} + C l_{2} \to 2 H C l; Δ H = - 44 k c a l

.
Heat of formation of

H C l

is:

Q. Bond dissociation enthalpies of

H_{2 (g)}, C l_{2} a n d H C l_{(g)}

are 104, 58 and 103 kcal respectively. The enthalpy of formation of HCl is

The Bond dissociation Energies of $H_{2}$ , $C l_{2}$ , and $H C l$ are $104$ , $58$ and $103$ $K c a l$ respectively. The Enthalpy of formation of $H C l$ of $H C l$ gas will be

Q. The bond dissociation energy of gaseous

H_{2}, C l_{2}

and HCl are 104, 58 and 103

k c a l m o l^{- 1}

respectively. The enthalpy of formation for

H C l

gas will be

Q. Given,

C (s) + O_{2} (g) \to C O_{2} (g) Δ H = - 94.2 k c a l

H_{2} (g) + \frac{1}{2} O_{2} (g) \to H_{2} O (l) Δ H = - 68.3 k c a l

C H_{4} (g) + 2 O_{2} (g) \to C O_{2} (g) + 2 H_{2} O (l) Δ H = - 210.8 k c a l

The heat of formation of methane in kcal will be :

Join BYJU'S Learning Program

When hydrogen gas is burnt in chlorine, 2000 cals of heat is liberated during the formation of 3.65 g of HCl. ΔH of formation of HCl is:

The correct option is B −20 Kcalfor 3.65 g of HCl 2000 cals of heat3.65 g =3.651+35.5=3.6536.5=110 molesfor 110 moles ----- 2000 calsfor 1 mole ----- 20 K cals∴ΔH of formation of HCl = -20 KcalsAs heat is liberated ΔH= - ve

When hydrogen gas is burnt in chlorine, 2000 cals of heat is liberated during the formation of 3.65 g of HCl. $Δ$ H of formation of HCl is:

The correct option is B $- 20$ Kcal
for 3.65 g of HCl 2000 cals of heat
3.65 g $= \frac{3.65}{1 + 35.5} = \frac{3.65}{36.5} = \frac{1}{10}$ moles
for $\frac{1}{10}$ moles ----- 2000 cals
for 1 mole ----- 20 K cals
$∴ Δ H$ of formation of HCl $=$ -20 Kcals
As heat is liberated $Δ H =$ - ve