What is the value of - H for the reaction X - 2Y - 2Z- W-X- 2Y - - H- 400 kcal-mol 2W - 3X - 2Z - 2Y - - H- 150 kcal-mol

The correct option is E + 650 kcal/molMultiply equation #160; W+X→ #160; 2Y with 2 . #160; 2W+2X→ #160; 4Y ; #160; #160; Δ H ...

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Byju's Answer

Standard XII

Chemistry

Hess' Law

What is the v...

Question

What is the value of $Δ H$ for the reaction $X + 2 Y \to 2 Z$ ?
$W + X \to 2 Y$ ; $Δ H = - 400$ kcal/mol
$2 W + 3 X \to 2 Z + 2 Y$ ; $Δ H = - 150$ kcal/mol

- 550

kcal/mol

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+ 50

kcal/mol

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- 50

kcal/mol

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+ 650

kcal/mol

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+ 250

kcal/mol

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Solution

The correct option is E $+ 650$ kcal/mol
Multiply equation $W + X \to 2 Y$ with $2$ .
$2 W + 2 X \to 4 Y$ ; $Δ H = 400 \times 2 = - 800$ kcal .....(1)
$2 W + 3 X \to 2 Z + 2 Y$ $Δ H = - 150$ kcal .....(2)
Subtracting equation (1) from equation (2) we get,
$X + 2 Y \to 2 Z$

$Δ H = - 150 - (- 800) = + 650$ kcal

Suggest Corrections

Similar questions

C (s) + O_{2} (g) \to C O_{2}, (g);

Δ H = - 94.3

kcal/mol

C O (g) + \frac{1}{2} O_{2} (g) \to C O_{2} (g);

Δ H = - 67.4

kcal/mol

O_{2} (g) \to 2 O (g);

Δ H = 117.4

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C O (g) \to C (g) + O (g);

Δ H = 230.6

kcal/mol.
Calculate

Δ H

for

C (s) \to C (g)

in kcal/mol.

C (s) + O_{2} (g) \to C O_{2} (g); Δ H = - 94.3

kcal/mol

C O (g) + 1 / 2 O_{2} (g) \to C O_{2} (g); Δ H = - 67.4

kcal/mol

O_{2} (g) \to 2 O (g); Δ H = 117.4

kcal/mol

C O (g) \to C (g) + O (g); Δ H = 230.6

kcal/mol

Calculate

Δ H

for

C (s)

\to

C (g)

in Kcal/mol.

Following are the thermochemical reactions:

H_{2} + \frac{1}{2} O_{2} \to H_{2} O; Δ H = - 68.39

kcal/mol

K + H_{2} O \to K O H (a q) + \frac{1}{2} H_{2}; Δ H = - 48.0

kcal/mol

K O H + H_{2} O \to K O H (a q); Δ H = - 14.0

kcal/mol

The heat of formation (in kcal/mol) of

K O H

is:

C s O H + H C l ⟶ C s C l + H_{2} O; Δ H = - 13.4 K c a l m o l^{- 1} . . . . (i)

C s O H + H F ⟶ C s F + H_{2} O; Δ H = - 16.4 K c a l m o l^{- 1} . . . . (i i)

Calculate

Δ H

for the ionisation of

H F

H_{2} O

Q. How many degree for 2-methyl butene and 2-pentene are -30 kcal/mol and -28 kcal/mol respectively. The heats of combustion of 2-methyl butane and pentane are -784 kcal/mol and -782 kcal/mol respectively. All the value are given under standard conditions. Taking into account that combustion of both alkanes gives the same products, what is

Δ H

(in kcal/mol) for the following reaction under the same condition?

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What is the value of ΔH for the reaction X+2Y→2Z?W+X→2Y ; ΔH=−400 kcal/mol2W+3X→2Z+2Y ; ΔH=−150 kcal/mol

The correct option is E +650 kcal/molMultiply equation W+X→2Y with 2.2W+2X→4Y ; ΔH=400×2=−800 kcal .....(1)2W+3X→2Z+2Y ΔH=−150 kcal .....(2)Subtracting equation (1) from equation (2) we get,X+2Y→2Z ΔH=−150−(−800)=+650 kcal

What is the value of $Δ H$ for the reaction $X + 2 Y \to 2 Z$ ?
$W + X \to 2 Y$ ; $Δ H = - 400$ kcal/mol
$2 W + 3 X \to 2 Z + 2 Y$ ; $Δ H = - 150$ kcal/mol