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Chapter 14: Q24P (page 390)

(I)If\({\bf{3}}{\bf{.40 \times 1}}{{\bf{0}}{\bf{5}}}\;{\bf{J}}\)of energy is supplied to a container of liquid oxygen at\({\bf{ - 183\circ C}}\), how much oxygen can evaporate?

Short Answer

Expert verified

The amount of oxygen evaporated is \(1.61\;{\rm{kg}}\).

Step by step solution

01

Given data

The energy supplied is\(Q = 3.40 \times {105}\;{\rm{J}}\).

The temperature is \(T = - 183\circ {\rm{C}}\).

02

Understanding the evaporation of oxygen

In this problem, the oxygen is at its boiling point, so the heat supplied will create the oxygen to evaporate. To find the mass of oxygen, use the relation of latent heat.

03

Calculation of the amount of oxygen evaporated

The relation to find the mass is given by:

\(Q = mL\)

Here,\(L\)is the latent heat.

On plugging the values in the above relation, you get:

\(\begin{array}{c}3.40 \times {105}\;{\rm{J}} = m\left( {2.1 \times {{10}5}\;{\rm{J/kg}}} \right)\\m = 1.61\;{\rm{kg}}\end{array}\)

Thus, \(m = 1.61\;{\rm{kg}}\) is the mass of the oxygen.

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