Aqueous CuSO4 solution was electrolysed by passing 2 amp of current for 10 min. What is the weight (in g) of copper deposited at cathode? (Cu = 63 u; F = 96500 C mol-1)
To find the weight of copper deposited at the cathode, we can use Faraday's laws of electrolysis.
According to Faraday's First Law, the mass of a substance deposited or liberated at an electrode is directly proportional to the quantity of electricity passed through the electrolyte. The relationship is given by:
m = (Q × M) / (n × F)
Where:
Step 1: Calculate the total charge (Q)
Q = I × t
Q = 2 A × 600 s = 1200 C
Step 2: Calculate the mass (m) of copper deposited
m = (1200 × 63) / (2 × 96500)
m = 75600 / 193000
m ≈ 0.3912 g
Conclusion:
The weight of copper deposited at the cathode is approximately 0.39 g.
The weight of copper deposited can be calculated using the formula:
W = (I × t × M) / (F × n)
Where:
Substituting the values:
W = (2 × 600 × 63) / (96500 × 2) = 0.39 g
Match the pollination types in List-I with their correct mechanisms in List-II:
List-I (Pollination Type) | List-II (Mechanism) |
---|---|
A) Xenogamy | I) Genetically different type of pollen grains |
B) Ophiophily | II) Pollination by snakes |
C) Chasmogamous | III) Exposed anthers and stigmas |
D) Cleistogamous | IV) Flowers do not open |