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The emf of a standard cadmium cell is 1.02V at 300K .The temperature coefficient of the cell is -5.0times10^(-5)VS^(-1) .The value of Delta H^(@) for the cell is (rounded up to two decimal places). 1F=96500 C Mol^(-1)?
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The emf of a standard cadmium cell is 1.02V at 300K .The temperature c...
**Calculating Delta H° for the Cell**
To calculate Delta H° for the cell, we can use the equation:
Delta H° = -nFE°
Where:
- Delta H° is the standard enthalpy change of the cell reaction,
- n is the number of electrons transferred in the cell reaction,
- F is Faraday's constant (96500 C mol^(-1)),
- E° is the standard cell potential.
In this case, the standard cell potential (E°) is given as 1.02 V. We need to determine the value of n, the number of electrons transferred in the cell reaction.
**Determining the Number of Electrons Transferred**
The number of electrons transferred in a redox reaction can be determined by analyzing the balanced half-reactions. In the case of a cadmium cell, the anode half-reaction is:
Cd(s) → Cd^(2+)(aq) + 2e^-
And the cathode half-reaction is:
2H^+(aq) + 2e^- → H2(g)
By comparing the two half-reactions, we can see that 2 electrons are transferred in the cell reaction. Therefore, n = 2.
**Calculating Delta H°**
Now we can calculate Delta H° using the equation:
Delta H° = -nFE°
Substituting the values:
Delta H° = -(2)(96500 C mol^(-1))(1.02 V)
Delta H° = -197130 J mol^(-1)
To convert the result to kilojoules per mole, we divide by 1000:
Delta H° = -197.13 kJ mol^(-1)
**Rounding to Two Decimal Places**
Rounding the result to two decimal places gives:
Delta H° = -197.13 kJ mol^(-1) (rounded to -197.13 kJ mol^(-1))
Therefore, the value of Delta H° for the cell is -197.13 kJ mol^(-1) (rounded to -197.13 kJ mol^(-1)).
To calculate Delta H° for the cell, we can use the equation:
Delta H° = -nFE°
Where:
- Delta H° is the standard enthalpy change of the cell reaction,
- n is the number of electrons transferred in the cell reaction,
- F is Faraday's constant (96500 C mol^(-1)),
- E° is the standard cell potential.
In this case, the standard cell potential (E°) is given as 1.02 V. We need to determine the value of n, the number of electrons transferred in the cell reaction.
**Determining the Number of Electrons Transferred**
The number of electrons transferred in a redox reaction can be determined by analyzing the balanced half-reactions. In the case of a cadmium cell, the anode half-reaction is:
Cd(s) → Cd^(2+)(aq) + 2e^-
And the cathode half-reaction is:
2H^+(aq) + 2e^- → H2(g)
By comparing the two half-reactions, we can see that 2 electrons are transferred in the cell reaction. Therefore, n = 2.
**Calculating Delta H°**
Now we can calculate Delta H° using the equation:
Delta H° = -nFE°
Substituting the values:
Delta H° = -(2)(96500 C mol^(-1))(1.02 V)
Delta H° = -197130 J mol^(-1)
To convert the result to kilojoules per mole, we divide by 1000:
Delta H° = -197.13 kJ mol^(-1)
**Rounding to Two Decimal Places**
Rounding the result to two decimal places gives:
Delta H° = -197.13 kJ mol^(-1) (rounded to -197.13 kJ mol^(-1))
Therefore, the value of Delta H° for the cell is -197.13 kJ mol^(-1) (rounded to -197.13 kJ mol^(-1)).
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The emf of a standard cadmium cell is 1.02V at 300K .The temperature coefficient of the cell is -5.0times10^(-5)VS^(-1) .The value of Delta H^(@) for the cell is (rounded up to two decimal places). 1F=96500 C Mol^(-1)?
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The emf of a standard cadmium cell is 1.02V at 300K .The temperature coefficient of the cell is -5.0times10^(-5)VS^(-1) .The value of Delta H^(@) for the cell is (rounded up to two decimal places). 1F=96500 C Mol^(-1)? for Chemistry 2024 is part of Chemistry preparation. The Question and answers have been prepared according to the Chemistry exam syllabus. Information about The emf of a standard cadmium cell is 1.02V at 300K .The temperature coefficient of the cell is -5.0times10^(-5)VS^(-1) .The value of Delta H^(@) for the cell is (rounded up to two decimal places). 1F=96500 C Mol^(-1)? covers all topics & solutions for Chemistry 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The emf of a standard cadmium cell is 1.02V at 300K .The temperature coefficient of the cell is -5.0times10^(-5)VS^(-1) .The value of Delta H^(@) for the cell is (rounded up to two decimal places). 1F=96500 C Mol^(-1)?.
The emf of a standard cadmium cell is 1.02V at 300K .The temperature coefficient of the cell is -5.0times10^(-5)VS^(-1) .The value of Delta H^(@) for the cell is (rounded up to two decimal places). 1F=96500 C Mol^(-1)? for Chemistry 2024 is part of Chemistry preparation. The Question and answers have been prepared according to the Chemistry exam syllabus. Information about The emf of a standard cadmium cell is 1.02V at 300K .The temperature coefficient of the cell is -5.0times10^(-5)VS^(-1) .The value of Delta H^(@) for the cell is (rounded up to two decimal places). 1F=96500 C Mol^(-1)? covers all topics & solutions for Chemistry 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The emf of a standard cadmium cell is 1.02V at 300K .The temperature coefficient of the cell is -5.0times10^(-5)VS^(-1) .The value of Delta H^(@) for the cell is (rounded up to two decimal places). 1F=96500 C Mol^(-1)?.
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