A bubble of 5.00 mol of helium is submerged at a certain depth in liquid water when the water ( and thus the helium ) undergoes a temperature increase `Delta T ` of ` 20.0 ^@ ` C at constant pressure .As a result the bubble expands the helium is monoatomic and ideal
How much work W is done by the helium as it expands against the pressure of the surrounding water during the temperature increase ?

Explanation

To solve the problem of calculating the work done \( W \) by the helium bubble as it expands against the pressure of the surrounding water during a temperature increase, we can follow these steps:

### Step 1: Understand the Work Done Formula
The work done by an ideal gas during expansion at constant pressure can be expressed as:
\[ W = P \Delta V \]
where \( P \) is the pressure and \( \Delta V \) is the change in volume.
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