During the electrolysis of `CrCl_(3)`, chlorine gas is evolved at the anode and chromium is deposited at the cathode. How many grams of Cr and how many litres of chlorine (at NTP) are produced, when a current of 6 amperes is passed for one hour ?

Explanation

To solve the problem of how many grams of chromium (Cr) and how many liters of chlorine (Cl2) are produced during the electrolysis of CrCl3 when a current of 6 amperes is passed for one hour, we can follow these steps:

### Step 1: Calculate the total charge (Q) passed through the electrolyte
The total charge (Q) can be calculated using the formula:
\[ Q = I \times T \]
Where:
- \( I \) = current in amperes (6 A)
- \( T \) = time in seconds (1 hour = 3600 seconds)
...