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The standard enthalpy of formation ( Δf U0300 ) at 1 bar and 300 K for the formation of CF2ClCF2Cl(g) from its constituent elements in the standard state is -900 kJ mol-1. Given R = 8.3 J K-1 mol-1, the standard internal energy of formation ( Δf U0300 ) at the same pressure and temperature is
- a)-905 kJ mol-1
- b)-895 kJ mol-1
- c)895 kJ mol-1
- d)905 kJ mol-1
Correct answer is option 'B'. Can you explain this answer?
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Verified Answer
The standard enthalpy of formation ( Δf U0300) at 1 bar and 300 K...
ΔH = ΔU + ΔngRT
Formation of CF2ClCF2Cl(g)
2C(s) + 2F2(g) + Cl2 (g) = CF2ClCF2Cl(g)
Δng = gaseous mole of product - gaseous mole of reactant.
Δng = 1 - 3 = - 2; ΔH = ΔU + ΔngRT
ΔU = ΔH - ΔngRT = ΔH + 2RT
= -900 kJ / mole + 2 × 8.314 × 300 JK-1 mole-1 K
= -900 kJ / mole + 5kJ / mole = -895 kJ/mole
Correct option is (b)
Formation of CF2ClCF2Cl(g)
2C(s) + 2F2(g) + Cl2 (g) = CF2ClCF2Cl(g)
Δng = gaseous mole of product - gaseous mole of reactant.
Δng = 1 - 3 = - 2; ΔH = ΔU + ΔngRT
ΔU = ΔH - ΔngRT = ΔH + 2RT
= -900 kJ / mole + 2 × 8.314 × 300 JK-1 mole-1 K
= -900 kJ / mole + 5kJ / mole = -895 kJ/mole
Correct option is (b)
Most Upvoted Answer
The standard enthalpy of formation ( Δf U0300) at 1 bar and 300 K...
The standard internal energy of formation (ΔU°f) can be calculated using the equation:
ΔU°f = ΔH°f - RT
where ΔH°f is the standard enthalpy of formation, R is the gas constant, and T is the temperature in Kelvin.
Given:
ΔH°f = -900 kJ mol-1
R = 8.3 J K-1 mol-1
T = 300 K
Substituting these values into the equation, we can calculate the standard internal energy of formation:
ΔU°f = -900 kJ mol-1 - (8.3 J K-1 mol-1)(300 K)
Simplifying the equation:
ΔU°f = -900 kJ mol-1 - 2490 J mol-1
Since we have different units (kJ and J), we need to convert kJ to J:
1 kJ = 1000 J
ΔU°f = -900,000 J mol-1 - 2490 J mol-1
ΔU°f = -902,490 J mol-1
Converting back to kJ:
1 kJ = 1000 J
ΔU°f = -902,490 J mol-1 / 1000
ΔU°f = -902.49 kJ mol-1
The standard internal energy of formation at 1 bar and 300 K is approximately -902.49 kJ mol-1. Since the answer choices are given in kJ mol-1, we can round this value to the nearest whole number, which is -895 kJ mol-1.
Therefore, the correct answer is option 'B', -895 kJ mol-1.
ΔU°f = ΔH°f - RT
where ΔH°f is the standard enthalpy of formation, R is the gas constant, and T is the temperature in Kelvin.
Given:
ΔH°f = -900 kJ mol-1
R = 8.3 J K-1 mol-1
T = 300 K
Substituting these values into the equation, we can calculate the standard internal energy of formation:
ΔU°f = -900 kJ mol-1 - (8.3 J K-1 mol-1)(300 K)
Simplifying the equation:
ΔU°f = -900 kJ mol-1 - 2490 J mol-1
Since we have different units (kJ and J), we need to convert kJ to J:
1 kJ = 1000 J
ΔU°f = -900,000 J mol-1 - 2490 J mol-1
ΔU°f = -902,490 J mol-1
Converting back to kJ:
1 kJ = 1000 J
ΔU°f = -902,490 J mol-1 / 1000
ΔU°f = -902.49 kJ mol-1
The standard internal energy of formation at 1 bar and 300 K is approximately -902.49 kJ mol-1. Since the answer choices are given in kJ mol-1, we can round this value to the nearest whole number, which is -895 kJ mol-1.
Therefore, the correct answer is option 'B', -895 kJ mol-1.
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The standard enthalpy of formation ( Δf U0300) at 1 bar and 300 K for the formation of CF2ClCF2Cl(g) from its constituent elements in the standard state is -900 kJ mol-1. Given R = 8.3 J K-1 mol-1, the standard internal energy of formation ( Δf U0300) at the same pressure and temperature isa)-905 kJ mol-1b)-895 kJ mol-1c)895 kJ mol-1d)905 kJ mol-1Correct answer is option 'B'. Can you explain this answer?
Question Description
The standard enthalpy of formation ( Δf U0300) at 1 bar and 300 K for the formation of CF2ClCF2Cl(g) from its constituent elements in the standard state is -900 kJ mol-1. Given R = 8.3 J K-1 mol-1, the standard internal energy of formation ( Δf U0300) at the same pressure and temperature isa)-905 kJ mol-1b)-895 kJ mol-1c)895 kJ mol-1d)905 kJ mol-1Correct answer is option 'B'. Can you explain this answer? for Chemistry 2024 is part of Chemistry preparation. The Question and answers have been prepared according to the Chemistry exam syllabus. Information about The standard enthalpy of formation ( Δf U0300) at 1 bar and 300 K for the formation of CF2ClCF2Cl(g) from its constituent elements in the standard state is -900 kJ mol-1. Given R = 8.3 J K-1 mol-1, the standard internal energy of formation ( Δf U0300) at the same pressure and temperature isa)-905 kJ mol-1b)-895 kJ mol-1c)895 kJ mol-1d)905 kJ mol-1Correct answer is option 'B'. Can you explain this answer? covers all topics & solutions for Chemistry 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The standard enthalpy of formation ( Δf U0300) at 1 bar and 300 K for the formation of CF2ClCF2Cl(g) from its constituent elements in the standard state is -900 kJ mol-1. Given R = 8.3 J K-1 mol-1, the standard internal energy of formation ( Δf U0300) at the same pressure and temperature isa)-905 kJ mol-1b)-895 kJ mol-1c)895 kJ mol-1d)905 kJ mol-1Correct answer is option 'B'. Can you explain this answer?.
The standard enthalpy of formation ( Δf U0300) at 1 bar and 300 K for the formation of CF2ClCF2Cl(g) from its constituent elements in the standard state is -900 kJ mol-1. Given R = 8.3 J K-1 mol-1, the standard internal energy of formation ( Δf U0300) at the same pressure and temperature isa)-905 kJ mol-1b)-895 kJ mol-1c)895 kJ mol-1d)905 kJ mol-1Correct answer is option 'B'. Can you explain this answer? for Chemistry 2024 is part of Chemistry preparation. The Question and answers have been prepared according to the Chemistry exam syllabus. Information about The standard enthalpy of formation ( Δf U0300) at 1 bar and 300 K for the formation of CF2ClCF2Cl(g) from its constituent elements in the standard state is -900 kJ mol-1. Given R = 8.3 J K-1 mol-1, the standard internal energy of formation ( Δf U0300) at the same pressure and temperature isa)-905 kJ mol-1b)-895 kJ mol-1c)895 kJ mol-1d)905 kJ mol-1Correct answer is option 'B'. Can you explain this answer? covers all topics & solutions for Chemistry 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The standard enthalpy of formation ( Δf U0300) at 1 bar and 300 K for the formation of CF2ClCF2Cl(g) from its constituent elements in the standard state is -900 kJ mol-1. Given R = 8.3 J K-1 mol-1, the standard internal energy of formation ( Δf U0300) at the same pressure and temperature isa)-905 kJ mol-1b)-895 kJ mol-1c)895 kJ mol-1d)905 kJ mol-1Correct answer is option 'B'. Can you explain this answer?.
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