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Chapter 19: Q. 27 (page 544)

A container holds 1.0 g of oxygen at a pressure of 8.0 atm.
a. How much heat is required to increase the temperature by 100掳C at constant pressure?
b. How much will the temperature increase if this amount of heat energy is transferred to the gas at constant volume?

Short Answer

Expert verified

The answer for (a) is $91.35 J$ and (b) is $140 K$ .

Step by step solution

01

Description

As per provided information:

A container holds 1.0 g of oxygen at a pressure of 8.0 atm.

Heat required for isobaric heating through the difference of temperature $鈭� T$ of n moles is provided by:

$Q = n C_{p} 鈭� T$

02

Result of finding required heat and temperature

The number of moles is provided as:

$n = \frac{m}{M}$

Thus, it can be written as:

$Q = \frac{1}{32} 路 29.2 路 100 = 91.25 J$

It can be stated that the relation of giving heat needed for the heating of isochoric/.

Thus, there can provide an increase in temperature $鈭� T_{v}$ for the case of isochoric as:

$Q = n C_{v} 鈭� T_{v} 鈬� 鈫� 鈭� T_{v} = \frac{Q}{n C_{v}}$

Thus, it can be written as after analysing the expression for heat:

$鈭� T_{v} = \frac{n C_{p} 鈭� T_{p}}{n C_{v}} = 纬鈭� T_{p}$

Thus, on the basis of numerics:

$鈭� T_{v} = 1.40 路 100 = 140 K$

Therefore,

The answer for (a) is $91.25 J$ and (b) is $140 K$ .

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