A bubble of $8$ moles of helium is submerged at certain depth in water. The temperature of water increases by $30^{o} C$ . How much heat is added approximately to helium (in $k J$ ) during expansion?

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Solution

The correct option is
A
5

$Q = n C_{p} Δ T = 8 \times \frac{5}{2} \times 8.31 \times 30 = 4986 J = 5 J$
$Option A is correct.$

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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 $Δ T$ of ${20.0}^{\circ} C$ ; 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? Use the first law of thermodynamics.