750 ml of `N_2` gas when taken in a vessel has pressure equal to 900 mm of Hg 1200 ml of `O_2` gas when taken in another vessel has pressure equal to 1450 mm of Hg. If both the gases are taken in 1000 ml vessel, what will be the total pressure exerted by the mixture of above gases? Assume that the gases are non-reacting.

Explanation

To solve the problem, we will use Boyle's Law and Dalton's Law of Partial Pressures. Here’s a step-by-step solution:

### Step 1: Calculate the Partial Pressure of Nitrogen (N₂)
We know from Boyle's Law that:
\[ P_1 \times V_1 = P_2 \times V_2 \]

Where:
- \( P_1 = 900 \, \text{mm Hg} \) (initial pressure of N₂)
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