A diver uses noen- oxygen mixture containing 70.4 g dioxygen and 167.5 g neon for respiration under water. If the total pressure is 25 bar then find partial pressures of oxygen and neon in the mixture? Atomic mass of oxygen is 16 u and that of neon is 20.2 u.

Explanation

To solve the problem of finding the partial pressures of oxygen and neon in a mixture used by a diver, we will follow these steps:

### Step 1: Calculate the number of moles of dioxygen (O2)
We know the weight of dioxygen and its molar mass. The molar mass of O2 (since the atomic mass of oxygen is 16 u) is:
\[ \text{Molar mass of O2} = 2 \times 16 = 32 \, \text{g/mol} \]

Using the formula for the number of moles:
\[ \text{Number of moles of O2} = \frac{\text{Weight of O2}}{\text{Molar mass of O2}} \]
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