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
(a) How much energy is added to the helium as heat during the increase and expansion ?

Explanation

To solve the problem, we need to calculate the energy added to the helium bubble during the temperature increase and expansion at constant pressure. Here’s a step-by-step breakdown of the solution:

### Step 1: Identify the Given Data
- Number of moles of helium, \( n = 5.00 \, \text{mol} \)
- Temperature increase, \( \Delta T = 20.0 \, ^\circ C \)
- For helium (a monoatomic ideal gas), we can use the specific heat capacities.

### Step 2: Determine the Specific Heat Capacity at Constant Pressure (\( C_p \))
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