On passing 3 ampere of electricity for 50 minutes, 1.8 gram metal deposits. The equivalent mass of metal is20.525.819.330.7

To determine the equivalent mass of the metal deposited, we can use Faraday's laws of electrolysis. According to Faraday's first law, the mass of a substance deposited is directly proportional to the quantity of electricity passed through the electrolyte.

1. ### Break Down the Problem

1. Given:

   • Current ($I$) = 3 A
   • Time ($t$) = 50 minutes
   • Mass deposited ($m$) = 1.8 g

2. The equivalent mass of the metal is required from the options.

2. ### Relevant Concepts

The quantity of electricity ($Q$) can be calculated using the formula: $Q = I \times t$ where $t$ should be in seconds. Thus, we convert 50 minutes to seconds: $t = 50 \times 60 = 3000 \, \text{seconds}$

3. ### Analysis and Detail

Calculating $Q$: $Q = 3 \, \text{A} \times 3000 \, \text{s} = 9000 \, \text{C}$

Next, we use the relationship: $\text{Equivalent mass} = \frac{\text{mass deposited}}{\text{Quantity of charge}} \times \text{equivalent weight}$

The equivalent weight can be found using: $\text{Equivalent weight} = \frac{m}{Q}$ Substituting the values in: $\text{Equivalent weight} = \frac{1.8 \, \text{g}}{9000 \, \text{C}}$

4. ### Verify and Summarize

Calculating the equivalent mass: $\text{Equivalent weight} = \frac{1.8}{9000} \approx 0.0002 \, \text{g/C}$

To find the equivalent mass (in grams), given the relationships and possible answers: We can conclude that the closest equivalent mass to our calculations from the given options of 20.525, 819.3, 30.7 is not explicitly calculable; thus, looking at the possible equivalent masses, we should cross-reference.

Final Answer

The equivalent mass of the metal deposited is approximately $0.2 \, \text{g/C}$, and there seems to be a mismatch with the options presented. Based on usual practices for equivalent masses, further clarity on the context is needed.