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earnstyle [38]
2 years ago
8

Container A and container B hold samples of the same ideal gas. The volume and the pressure of container A is equal to the volum

e and pressure of container B, respectively. If Container A has half as many molecules of the ideal gas in it as Container B does, then which of the following mathematical statements is correct regarding the absolute temperatures TA and TB in Container A and Container B. respectively?
A. TA = TB/2.
B. TA = 4TB.
C. TA = TB/4.
D. TA = 2TB.
E. TA = TB
Physics
1 answer:
SVETLANKA909090 [29]2 years ago
6 0

Answer:

A. TA = TB/2.

Explanation:

Since container A has half as many molecules of the ideal gas in it as container B. Therefore, container A will have half the volume of gas as in container B:

V_A = \frac{1}{2}V_B

Now, from Charle's Law:

\frac{V_A}{T_A}=\frac{V_B}{T_B}\\\\\frac{1}{2}\frac{V_B}{T_A}=\frac{V_B}{T_B}\\\\T_A = \frac{T_B}{2}

Hence, the correct option is:

<u>A. TA = TB/2.</u>

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Explanation:

The heat (thermal energy) needed in to raise the temperature in a process can be found using the following equation:

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Where:

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m=8 g is the mass of the element (<u>water</u> in this case)

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Knowing this, let's rewrite (1) with these values:

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60o |
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