Study the given graph and choose the correct option.

Δ H

is the net heat absorbed from the surroundings

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Δ H

is the net heat given to the surroundings

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Δ H

is positive for the reaction

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Δ H

is the total energy possessed by the reactants

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Solution

The correct option is A $Δ H$ is the net heat given to the surroundings
Since the value of $Δ H$ is negative, it shows that the reaction is exothermic and $Δ H$ is the heat given to the surroundings.

Hence, the correct answer is option $B$ .

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Similar questions

The heat energy q absorbed by a gas is equal to

Δ H

if heat is absorbed at a constant pressure.

Q. Heat of reaction for the reaction is:

P C l_{5} (g) + H_{2} O (g) ⟶ P O C l_{3} (g) + 2 H C l (g)

Given that,

P_{w h i t e} + (3 / 2) C l_{2} (g) + \frac{1}{2} O_{2} (g) ⟶ P O C l_{3}; Δ H = - 135.5 k c a l

H_{2} (g) + C l_{2} (g) ⟶ + 2 H C l (g); Δ H = - 44.1 k c a l

P (w) + (5 / 2) C l_{2} (g) ⟶ P C l_{5} (g); Δ H = - 89.6 k c a l

H_{2} (g) + \frac{1}{2} O_{2} (g) ⟶ H_{2} O (g); Δ H = - 57.8 k c a l

A vessel contains 100 litres of a liquid $x$ . Heat is supplied to the liquid in such a fashion that, Heat given = change in enthalpy. The volume of the liquid increases by 2 litres. If the external pressure is one atm, and 202.6 Joules of heat were supplied then, [ U - total internal energy ]

Q. Use the given standard enthalpies of formation to determine the heat of reaction of the following reaction:

T i C L_{4} (g) + 2 H_{2} O (g) \to T i O_{2} (g) + 4 H C l (g)

Δ H_{f}^{\circ} T i C L_{4} (g) = - 763.2 k J / m o l

Δ H_{f}^{\circ} T i O_{2} (g) = - 944.7 k J / m o l

Δ H_{f}^{\circ} H_{2} O (g) = - 241.8 k J / m o l

Δ H_{f}^{\circ} H C l (g) = - 92.3 k J / m o l

Q. Given that,

H_{2} (g) + I_{2} (s) \to 2 H I (g); Δ H = 51.9 K J / m o l e

H_{2} (g) + I_{2} (g) \to 2 H I (g); Δ H = - 9.2 K J / m o l e

The heat of reaction of $I_{2} (s) \to I_{2} (g)$ is:

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Study the given graph and choose the correct option.

The correct option is A ΔH is the net heat given to the surroundingsSince the value of ΔH is negative, it shows that the reaction is exothermic and ΔH is the heat given to the surroundings.Hence, the correct answer is option B.

The correct option is A $Δ H$ is the net heat given to the surroundings
Since the value of $Δ H$ is negative, it shows that the reaction is exothermic and $Δ H$ is the heat given to the surroundings.

Hence, the correct answer is option $B$ .