Statement 1 - An exothermic reaction has a positive - H-Statement 2 - Heat must be added to the system for the reaction to occur-

The correct option is E #10; #10; #10; #9; #10; #9; #10; #9; #10; #9; #10; #10; #10;Both the Statement 1 #10;and Statement 2 are n ...

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Standard XII

Chemistry

Liquid-Vapour Equillibrium

Statement 1 :...

Question

Statement 1 : An exothermic reaction has a positive $Δ H$ .
Statement 2 : Heat must be added to the system for the reaction to occur.

Both Statement 1 and Statement 2 are correct and Statement 2 is the correct explanation of Statement 1.

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Both Statement 1 and Statement 2 are correct and Statement 2 is not the correct explanation of Statement 1.

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Statement 1 is correct but Statement 2 is not correct.

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Statement 1 is not correct but Statement 2 is correct.

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Both the Statement 1 and Statement 2 are not correct.

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Solution

The correct option is E
Both the Statement 1 and Statement 2 are not correct.

Exothermic and endothermic reactions cause energy level differences and therefore differences in enthalpy $Δ H$ , the sum of all potential and kinetic energies. $Δ H$ is determined by the system, not the surrounding environment in a reaction. A system that releases heat to the surroundings, an exothermic reaction, has a negative $Δ H$ by convention because the enthalpy of the products is lower than the enthalpy of the reactants of the system
$C (s) + O_{2} (g) \to C O_{2} (g) (Δ H = - 393.5 k J)$
$H_{2} (g) + \frac{1}{2} O_{2} (g) \to H_{2} O (l) (Δ H = - 285.8 k J)$
The enthalpies of these reactions are less than zero and are therefore exothermic reactions.
For an exothermic reaction, heat should be released by the system to occur the reactions.

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Statement 1 : An exothermic reaction has a positive ΔH.Statement 2 : Heat must be added to the system for the reaction to occur.

Statement 1 : An exothermic reaction has a positive $Δ H$ .
Statement 2 : Heat must be added to the system for the reaction to occur.