Calculate the entropy change in surroundings when 1.00 mol of H 2 O( l ) is formed under standard conditions. ∆ f H 0 = –286 kJ mol –1 . - Wired Faculty

Thermodynamics

Question

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Calculate the entropy change in surroundings when 1.00 mol of H₂O(l) is formed under standard conditions. ∆_fH⁰ = –286 kJ mol^–1.

Solution

The thermochemical equation is,
$space straight H subscript 2 left parenthesis straight g right parenthesis space plus space 1 half straight O subscript 2 space space space rightwards arrow space space straight H subscript 2 straight O left parenthesis l right parenthesis semicolon space triangle subscript straight f straight H to the power of 0 space equals space minus 286 space kJ space mol to the power of negative 1 end exponent$
From the above equation, it is clear that when 1 mol of H₂O(l) is formed, 286 kJ of heat is released. The same amount of heat is absorbed by the surroundings.
$straight i. straight e. space space space space straight q subscript surr space equals space plus 286 space kJ space mol to the power of negative 1 end exponent We space know comma space increment straight S space equals space straight q subscript surr over straight T space equals space fraction numerator 286 space kJ space mol to the power of negative 1 end exponent over denominator 298 space straight K end fraction space space space space equals space 0.9597 space kJ space straight K to the power of negative 1 end exponent mol to the power of negative 1 end exponent space space space space equals space 959.7 space JK to the power of negative 1 end exponent space mol to the power of negative 1 end exponent space space$

Some More Questions From Thermodynamics Chapter

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Thermodynamics

Calculate the entropy change in surroundings when 1.00 mol of H₂O(l) is formed under standard conditions. ∆_fH⁰ = –286 kJ mol^–1.

Some More Questions From Thermodynamics Chapter

Define intensive properties.

Define extensive properties.

Why all living systems need to be 'open systems'?

Define state variables of a system.

From thermodynamic point of view, to which system the animals and plants belong?

What is a state function?

A thermodynamic state function is a quantity

What is reversible process in thermodynamics?

Define irreversible change.

Name the variable that is kept constant in isochoric process and isobaric process.

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For Daily Free Study Material Join wiredfaculty

Thermodynamics

Calculate the entropy change in surroundings when 1.00 mol of H2O(l) is formed under standard conditions. ∆fH0 = –286 kJ mol–1.

Some More Questions From Thermodynamics Chapter

Define intensive properties.

Define extensive properties.

Why all living systems need to be 'open systems'?

Define state variables of a system.

From thermodynamic point of view, to which system the animals and plants belong?

What is a state function?

A thermodynamic state function is a quantity

What is reversible process in thermodynamics?

Define irreversible change.

Name the variable that is kept constant in isochoric process and isobaric process.

Mock Test Series

NCERT Sample Papers

Entrance Exams Preparation

Calculate the entropy change in surroundings when 1.00 mol of H₂O(l) is formed under standard conditions. ∆_fH⁰ = –286 kJ mol^–1.