How much heat will be required at constant pressure to form 1-28 kg of CaC 2 from CaO s and C s - Given- r H 0 CaO - s -152 kcal - mol- r H 0 CaC 2- s -14 kcal - mol- r H 0 CO - g -26 kcal - mol-A- 3840 kcalB- 2240 kcalC- 22-4 kcalD- 224 kcal

The correct option is B 2240 kcal CaO(s) + 3C(s) → CaC_2(s) + CO(g) Δ_fH^0 = ( 14 26) ( 152) = +112 kcal/mol Total heat required = (1280/64) × 112 ⇒ 2240 k ...

You visited us 1 times! Enjoying our articles? Unlock Full Access!

Byju's Answer

Standard XII

Chemistry

Heat of Formation

How much heat...

Question

How much heat will be required at constant pressure to form $1.28 k g$ of $C a C_{2}$ from $C a O (s)$ and $C (s)$ ?

Given:

$Δ_{r} H^{0} (C a O, s) = - 152 k c a l / m o l$ .

$Δ_{r} H^{0} (C a C_{2}, s) = - 14 k c a l / m o l$ .

$Δ_{r} H^{0} (C O, g) = - 26 k c a l / m o l$ .

22.4 kcal

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

224 kcal

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

3840 kcal

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

2240 kcal

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

Open in App

Solution

The correct option is D
2240 kcal

$C a O (s) + 3 C (s) \to C a C_{2} (s) + C O (g)$

$Δ_{f} H^{0} = (- 14 - 26) - (- 152) = + 112 k c a l / m o l$

Total heat required = $(\frac{1280}{64}) \times 112$

$\Rightarrow 2240 k c a l$

Suggest Corrections

Similar questions

How much heat will be required at constant pressure to form $1.28 k g$ of $C a C_{2}$ from $C a O (s)$ and $C (s)$ ?

Given:

$Δ_{r} H^{0} (C a O, s) = - 152 k c a l / m o l$ .

$Δ_{r} H^{0} (C a C_{2}, s) = - 14 k c a l / m o l$ .

$Δ_{r} H^{0} (C O, g) = - 26 k c a l / m o l$ .

Q. How much heat will be required to make

2 k g

of calcium carbide

(C a C_{2})

according to the following reaction?

C a O (s) + 3 C (s) \to C a C_{2} + C O (g)

The heats of formation of

C a O (s), C a C_{2} (s)

and

C O (g)

are

- 151.6, - 14.2, - 26.4 k c a l

respectively.

Q. What is the amount of heat to be supplied to prepare

128 g

C a C_{2}

by using

C a C O_{3}

and followed by reaction with carbon. Reactions are:

C a C O_{3} (s) \to C a O (s) + C O_{2} (g); △ H^{o} = 42 .8 kcal

C a O (s) + 3 C (s) \to C a C_{2} (s) + C O (g); △ H^{o} = 111 kcal

140 cal

of heat is required to raise the temperature of

2

mole of a diatomic gas at constant pressure from

0^{\circ} C

10^{\circ} C

. How much heat will be required to rise its temperature from

0^{\circ} C

10^{\circ} C

at constant volume?

140 cal

of heat is required to raise the temperature of

2

mole of a diatomic gas at constant pressure from

0^{\circ} C

10^{\circ} C

. How much heat will be required to rise its temperature from

0^{\circ} C

10^{\circ} C

at constant volume?

Join BYJU'S Learning Program

How much heat will be required at constant pressure to form 1.28 kg of CaC2 from CaO(s) and C(s)? Given: ΔrH0(CaO,s) = −152 kcal/mol. ΔrH0(CaC2,s) = −14 kcal/mol. ΔrH0(CO,g) = −26 kcal/mol.

The correct option is D 2240 kcal CaO(s) + 3C(s) → CaC2(s) + CO(g) ΔfH0 = (−14 − 26) − (−152) = +112 kcal/mol Total heat required = (128064) × 112 ⇒ 2240 kcal

How much heat will be required at constant pressure to form $1.28 k g$ of $C a C_{2}$ from $C a O (s)$ and $C (s)$ ?

Given:

$Δ_{r} H^{0} (C a O, s) = - 152 k c a l / m o l$ .

$Δ_{r} H^{0} (C a C_{2}, s) = - 14 k c a l / m o l$ .

$Δ_{r} H^{0} (C O, g) = - 26 k c a l / m o l$ .

The correct option is D
2240 kcal

$C a O (s) + 3 C (s) \to C a C_{2} (s) + C O (g)$

$Δ_{f} H^{0} = (- 14 - 26) - (- 152) = + 112 k c a l / m o l$

Total heat required = $(\frac{1280}{64}) \times 112$

$\Rightarrow 2240 k c a l$