From the following data at 25anddeg;CWhich of the following statement(s) is/are correct :Statement(a) : andDelta;rHanddeg; for the reaction H2O(g) andrarr; 2H(g) + O(g) is 925 kJ/molStatement(b) : andDelta;rHanddeg; for the reaction OH(g) andrarr; H(g) + O(g) is 502 kJ/molStatement(c) : Enthalpy of formation of H(g) is-andndash;218 kJ/molStatement(d) : Enthalpy of formation of OH(g) is 42 kJ/mola)Statement cb)Statement a, b, dc)Statement b,cd)Statement a, dCorrect answer is option 'D'. Can you explain this answer?

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From the following data at 25°C

Which of the following statement(s) is/are correct :
Statement(a) : Δ_rH° for the reaction H₂O(g) → 2H(g) + O(g) is 925 kJ/mol
Statement(b) : Δ_rH° for the reaction OH(g) → H(g) + O(g) is 502 kJ/mol
Statement(c) : Enthalpy of formation of H(g) is-–218 kJ/mol
Statement(d) : Enthalpy of formation of OH(g) is 42 kJ/mol

a)
Statement c
b)
Statement a, b, d
c)
Statement b,c
d)
Statement a, d

Correct answer is option 'D'. Can you explain this answer?

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From the following data at 25°CWhich of the following statement(s)...

Let's check statement (a)
Statement(a) : ΔrH° for the reaction H₂O(g) → 2H(g) + O(g) is 925 kJ/mol
For this, we need - (II) + (III) + ½ (IV)
We get, H₂O(g) → 2H(g) + O(g) - (-242)+436+½ 495 = 925.5 kJ mol^-1
So it is true.
Let's check statement (b)
Statement(b) : ΔrH° for the reaction OH(g) → H(g) + O(g) is 502 kJ/mol
For this we need -(I)+½ (III)+½ (IV)
We get OH(g) → H(g) + O(g) -(42) + ½ (436) + ½ (495) = 423.5 kJ mol-1
So statement (b) is wrong.
Let's check statement (c)
Statement(c) : Enthalpy of formation of H(g) is -218 kJ/mol
We can see that for enthalpy of formation, we need to divide eqn (III) by 2
So, it would become :-
½ H₂(g) → H(g)
436/2 = 218 kJ
So, statement (c) is wrong.
Let's check statement (d)
Statement(d) : Enthalpy of formation of OH(g) is 42 kJ/mol
For that, we have eqn (I) as it is. So, statement (d) is correct.

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From the following data at 25°CWhich of the following statement(s) is/are correct :Statement(a) : ΔrH° for the reaction H2O(g) → 2H(g) + O(g) is 925 kJ/molStatement(b) : ΔrH° for the reaction OH(g) → H(g) + O(g) is 502 kJ/molStatement(c) : Enthalpy of formation of H(g) is-–218 kJ/molStatement(d) : Enthalpy of formation of OH(g) is 42 kJ/mola)Statement cb)Statement a, b, dc)Statement b,cd)Statement a, dCorrect answer is option 'D'. Can you explain this answer?

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From the following data at 25°CWhich of the following statement(s) is/are correct :Statement(a) : ΔrH° for the reaction H2O(g) → 2H(g) + O(g) is 925 kJ/molStatement(b) : ΔrH° for the reaction OH(g) → H(g) + O(g) is 502 kJ/molStatement(c) : Enthalpy of formation of H(g) is-–218 kJ/molStatement(d) : Enthalpy of formation of OH(g) is 42 kJ/mola)Statement cb)Statement a, b, dc)Statement b,cd)Statement a, dCorrect answer is option 'D'. Can you explain this answer? for Class 11 2024 is part of Class 11 preparation. The Question and answers have been prepared according to the Class 11 exam syllabus. Information about From the following data at 25°CWhich of the following statement(s) is/are correct :Statement(a) : ΔrH° for the reaction H2O(g) → 2H(g) + O(g) is 925 kJ/molStatement(b) : ΔrH° for the reaction OH(g) → H(g) + O(g) is 502 kJ/molStatement(c) : Enthalpy of formation of H(g) is-–218 kJ/molStatement(d) : Enthalpy of formation of OH(g) is 42 kJ/mola)Statement cb)Statement a, b, dc)Statement b,cd)Statement a, dCorrect answer is option 'D'. Can you explain this answer? covers all topics & solutions for Class 11 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for From the following data at 25°CWhich of the following statement(s) is/are correct :Statement(a) : ΔrH° for the reaction H2O(g) → 2H(g) + O(g) is 925 kJ/molStatement(b) : ΔrH° for the reaction OH(g) → H(g) + O(g) is 502 kJ/molStatement(c) : Enthalpy of formation of H(g) is-–218 kJ/molStatement(d) : Enthalpy of formation of OH(g) is 42 kJ/mola)Statement cb)Statement a, b, dc)Statement b,cd)Statement a, dCorrect answer is option 'D'. Can you explain this answer?.

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