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olasank [31]
3 years ago
9

A sample of a monatomic ideal gas is originally at 20 °c. what is the final temperature of the gas if the pressure is doubled a

nd volume is reduced to one-fourth its initial value?
Physics
1 answer:
Anna11 [10]3 years ago
3 0

Answer:

the final temperature is T2=  -126.5°C

Explanation:

Since the gas behaves as an ideal gas

Initial state) P1*V1=n*R*T1

Final state) P2*V2=n*R*T2

where P= gas pressure , V=volume occupied by the gas , n= number of moles , R= ideal gas constant , T= absolute temperature

dividing both equations

(P2/P1)*(V2/V1)=T2/T1

since P2=2*P1 and V2=1/4*V1 , T1=20°C=293K

2*1/4=T2/T1

T2=T1/2 = 293K/2 = 146.5K

T2= 146.5K= -126.5°C

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In this problem we are describing two different processes:

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In both cases, the total mass of the final products is smaller than the total mass of the initial nuclei.

According to Einsten's formula, this mass difference has been converted into energy, as follows:

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