NEET Test Series from KOTA - 10 Papers In MS WORD
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ELECTROCHEMISTRY
20089
Oxidation and reduction take place in a cell, then its electromotive force will be
1 Positive
2 Negative
3 Zero
4 Stable
Explanation:
(a)Electromotive force is \(+ve\) if oxidation and reduction both takes place in a cell.
ELECTROCHEMISTRY
20090
For a spontaneous reaction the \(\Delta G,\) equilibrium constant \( (K)\) and \(E_{Cell}^o\) will be respectively
1 \( - ve,\, > 1,\, + ve\)
2 \( + ve,\, > 1,\, - ve\)
3 \( - ve,\, < 1,\, - ve\)
4 \( - ve,\, > 1,\, - ve\)
Explanation:
we know \(\Delta G =- RT \ln K =- nF E ^{\circ}\) We know for a spontaneous reaction \(\Delta G \,<\,0 \text {. }\) \(\therefore- RT \ln K \,<\,0\) \(\therefore \ln K\,>\,0\) \(\therefore K\,>\,1\) and \(- nF E ^{\circ}<0\) \(\therefore E _{\text {cell }}^{\circ}\,>\,0\)
ELECTROCHEMISTRY
20091
The reference electrode is made from which of the following
1 \(ZnC{l_2}\)
2 \(CuS{O_4}\)
3 \(H{g_2}C{l_2}\)
4 \(HgC{l_2}\)
Explanation:
It’s obvious.
ELECTROCHEMISTRY
20092
The charge over anode in a galvanic cell is
1 Negative
2 Positive
3 No charge
4 Sometimes negative and sometimes positive
Explanation:
(a)In galvanic cell anode always made up of negative electrode.
20089
Oxidation and reduction take place in a cell, then its electromotive force will be
1 Positive
2 Negative
3 Zero
4 Stable
Explanation:
(a)Electromotive force is \(+ve\) if oxidation and reduction both takes place in a cell.
ELECTROCHEMISTRY
20090
For a spontaneous reaction the \(\Delta G,\) equilibrium constant \( (K)\) and \(E_{Cell}^o\) will be respectively
1 \( - ve,\, > 1,\, + ve\)
2 \( + ve,\, > 1,\, - ve\)
3 \( - ve,\, < 1,\, - ve\)
4 \( - ve,\, > 1,\, - ve\)
Explanation:
we know \(\Delta G =- RT \ln K =- nF E ^{\circ}\) We know for a spontaneous reaction \(\Delta G \,<\,0 \text {. }\) \(\therefore- RT \ln K \,<\,0\) \(\therefore \ln K\,>\,0\) \(\therefore K\,>\,1\) and \(- nF E ^{\circ}<0\) \(\therefore E _{\text {cell }}^{\circ}\,>\,0\)
ELECTROCHEMISTRY
20091
The reference electrode is made from which of the following
1 \(ZnC{l_2}\)
2 \(CuS{O_4}\)
3 \(H{g_2}C{l_2}\)
4 \(HgC{l_2}\)
Explanation:
It’s obvious.
ELECTROCHEMISTRY
20092
The charge over anode in a galvanic cell is
1 Negative
2 Positive
3 No charge
4 Sometimes negative and sometimes positive
Explanation:
(a)In galvanic cell anode always made up of negative electrode.
20089
Oxidation and reduction take place in a cell, then its electromotive force will be
1 Positive
2 Negative
3 Zero
4 Stable
Explanation:
(a)Electromotive force is \(+ve\) if oxidation and reduction both takes place in a cell.
ELECTROCHEMISTRY
20090
For a spontaneous reaction the \(\Delta G,\) equilibrium constant \( (K)\) and \(E_{Cell}^o\) will be respectively
1 \( - ve,\, > 1,\, + ve\)
2 \( + ve,\, > 1,\, - ve\)
3 \( - ve,\, < 1,\, - ve\)
4 \( - ve,\, > 1,\, - ve\)
Explanation:
we know \(\Delta G =- RT \ln K =- nF E ^{\circ}\) We know for a spontaneous reaction \(\Delta G \,<\,0 \text {. }\) \(\therefore- RT \ln K \,<\,0\) \(\therefore \ln K\,>\,0\) \(\therefore K\,>\,1\) and \(- nF E ^{\circ}<0\) \(\therefore E _{\text {cell }}^{\circ}\,>\,0\)
ELECTROCHEMISTRY
20091
The reference electrode is made from which of the following
1 \(ZnC{l_2}\)
2 \(CuS{O_4}\)
3 \(H{g_2}C{l_2}\)
4 \(HgC{l_2}\)
Explanation:
It’s obvious.
ELECTROCHEMISTRY
20092
The charge over anode in a galvanic cell is
1 Negative
2 Positive
3 No charge
4 Sometimes negative and sometimes positive
Explanation:
(a)In galvanic cell anode always made up of negative electrode.
NEET Test Series from KOTA - 10 Papers In MS WORD
WhatsApp Here
ELECTROCHEMISTRY
20089
Oxidation and reduction take place in a cell, then its electromotive force will be
1 Positive
2 Negative
3 Zero
4 Stable
Explanation:
(a)Electromotive force is \(+ve\) if oxidation and reduction both takes place in a cell.
ELECTROCHEMISTRY
20090
For a spontaneous reaction the \(\Delta G,\) equilibrium constant \( (K)\) and \(E_{Cell}^o\) will be respectively
1 \( - ve,\, > 1,\, + ve\)
2 \( + ve,\, > 1,\, - ve\)
3 \( - ve,\, < 1,\, - ve\)
4 \( - ve,\, > 1,\, - ve\)
Explanation:
we know \(\Delta G =- RT \ln K =- nF E ^{\circ}\) We know for a spontaneous reaction \(\Delta G \,<\,0 \text {. }\) \(\therefore- RT \ln K \,<\,0\) \(\therefore \ln K\,>\,0\) \(\therefore K\,>\,1\) and \(- nF E ^{\circ}<0\) \(\therefore E _{\text {cell }}^{\circ}\,>\,0\)
ELECTROCHEMISTRY
20091
The reference electrode is made from which of the following
1 \(ZnC{l_2}\)
2 \(CuS{O_4}\)
3 \(H{g_2}C{l_2}\)
4 \(HgC{l_2}\)
Explanation:
It’s obvious.
ELECTROCHEMISTRY
20092
The charge over anode in a galvanic cell is
1 Negative
2 Positive
3 No charge
4 Sometimes negative and sometimes positive
Explanation:
(a)In galvanic cell anode always made up of negative electrode.