LAB 4 TEST QUESTIONS AND ANSWERS
1. 1 FARADAY = ? - ANSWER-= CHARGE ON 1 MOLE ELECTRON
2. 1 FARADAY = HOW MANY COULOMBS - ANSWER-1 F = 96,500 C/MOL
ELECTRONS
3. 2 X MOL H2 = ? - ANSWER-2 X MOL H2 = MOL ELECTRON
4. A CURRENT OF 3.00A PASSED THROUGH A SOLUTION OF SULFURIC ACID FOR
20min. THE HYDROGEN PRODUCED WAS COLLECTED OVER WATER AT 20
(DEGREES C) AND 657.Five mm Hg AND WAS FOUND TO OCCUPY A VOLUME OF
534 mL. HOW MANY MOLES OF H2 WERE PRODUCED, AND WHAT IS THE VALUE
OF AVOGADRO'S NUMBER, N? - ANSWER-MOL H2 = zero.0187
N = 6.02X10^23
5. A CURRENT OF 3.00A PASSED THROUGH A SOLUTION OF SULFURIC ACID FOR
EXACTLY 20min. HOW MANY ELECTRONS AND HOW MANY COULOMBS WERE
PASSED THROUGH THE SOLUTION? - ANSWER-C = three.60X10^three
ELECTRONS = 2.25X10^22
6. CALCULATE THE PERCENT C2O4^2- IN EACH OF THE FOLLOWING:
- H2C2O4
- Na2C2O4
- K2C2O4
- K3[Al(C2O4)3] x 3H20 - ANSWER-- H2C2O4 = ninety seven.Eight%
- Na2C2O4 = sixty five.7%
- K2C2O4 = fifty three.0%
- K3[Al(C2O4)3] x 3H20 = 53.Eight%
7. COULOMB - ANSWER-THE AMOUNT OF ELECTRICAL CHARGE THAT PASSES A
POINT IN A CIRCUIT WHEN A CURRENT OF 1 AMPERE, A, FLOWS FOR 1
SECOND, S.
8. ELECTROLYSIS OF AN NaCl SOLUTION WITH A CURRENT OF 2.00A FOR A
PERIOD OF 200s PRODUCED 59.6mL OF Cl2 AT 650mm Hg PRESSURE AND 27
DEGREES C. CALCULATE THE VALUE OF THE FARADAY'S CONSTANT FROM THIS
DATA. - ANSWER-F = 96591.02
9. ELECTROLYSIS OF MOLTEN NaCl IS DONE IN A DOWNS CELL OPERATING AT 7.0
VOLTS AND 4.0X10^4A. HOW MUCH Na(s) AND Cl2(g) CAN BE PRODUCED IN eight
HOURS IN SUCH A CELL? - ANSWER-Na(s) = 2.74x10^five
Cl2(g) = 4.2x10^five
10.EQUATION FOR # OF ELECTRONS? - ANSWER-# OF ELECTRONS = C/1.6x10^-19
(c/e-)
11.EQUATION FOR AVOGADRO'S NUMBER, N? - ANSWER-N = (# ELECTRONS/MOL
ELECTRON)
1. 1 FARADAY = ? - ANSWER-= CHARGE ON 1 MOLE ELECTRON
2. 1 FARADAY = HOW MANY COULOMBS - ANSWER-1 F = 96,500 C/MOL
ELECTRONS
3. 2 X MOL H2 = ? - ANSWER-2 X MOL H2 = MOL ELECTRON
4. A CURRENT OF 3.00A PASSED THROUGH A SOLUTION OF SULFURIC ACID FOR
20min. THE HYDROGEN PRODUCED WAS COLLECTED OVER WATER AT 20
(DEGREES C) AND 657.Five mm Hg AND WAS FOUND TO OCCUPY A VOLUME OF
534 mL. HOW MANY MOLES OF H2 WERE PRODUCED, AND WHAT IS THE VALUE
OF AVOGADRO'S NUMBER, N? - ANSWER-MOL H2 = zero.0187
N = 6.02X10^23
5. A CURRENT OF 3.00A PASSED THROUGH A SOLUTION OF SULFURIC ACID FOR
EXACTLY 20min. HOW MANY ELECTRONS AND HOW MANY COULOMBS WERE
PASSED THROUGH THE SOLUTION? - ANSWER-C = three.60X10^three
ELECTRONS = 2.25X10^22
6. CALCULATE THE PERCENT C2O4^2- IN EACH OF THE FOLLOWING:
- H2C2O4
- Na2C2O4
- K2C2O4
- K3[Al(C2O4)3] x 3H20 - ANSWER-- H2C2O4 = ninety seven.Eight%
- Na2C2O4 = sixty five.7%
- K2C2O4 = fifty three.0%
- K3[Al(C2O4)3] x 3H20 = 53.Eight%
7. COULOMB - ANSWER-THE AMOUNT OF ELECTRICAL CHARGE THAT PASSES A
POINT IN A CIRCUIT WHEN A CURRENT OF 1 AMPERE, A, FLOWS FOR 1
SECOND, S.
8. ELECTROLYSIS OF AN NaCl SOLUTION WITH A CURRENT OF 2.00A FOR A
PERIOD OF 200s PRODUCED 59.6mL OF Cl2 AT 650mm Hg PRESSURE AND 27
DEGREES C. CALCULATE THE VALUE OF THE FARADAY'S CONSTANT FROM THIS
DATA. - ANSWER-F = 96591.02
9. ELECTROLYSIS OF MOLTEN NaCl IS DONE IN A DOWNS CELL OPERATING AT 7.0
VOLTS AND 4.0X10^4A. HOW MUCH Na(s) AND Cl2(g) CAN BE PRODUCED IN eight
HOURS IN SUCH A CELL? - ANSWER-Na(s) = 2.74x10^five
Cl2(g) = 4.2x10^five
10.EQUATION FOR # OF ELECTRONS? - ANSWER-# OF ELECTRONS = C/1.6x10^-19
(c/e-)
11.EQUATION FOR AVOGADRO'S NUMBER, N? - ANSWER-N = (# ELECTRONS/MOL
ELECTRON)
