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No. During Step 1, the temperature got higher, and it stayed at this value during step 2.Ben_Walker1978 said:The volume at constant temperature was 0.12. So is both the volumes 0.12?
No. During Step 1, the temperature got higher, and it stayed at this value during step 2.Ben_Walker1978 said:The volume at constant temperature was 0.12. So is both the volumes 0.12?
You already guessed the correct equation to use. in post #13. But, you used the wrong initial pressure, and you applied the equation incorrectly.Ben_Walker1978 said:Yes the temperature got to 542.99 Kelvin.
But i don't know what equation to use.
P2=14.9/8=1.86 barsBen_Walker1978 said:$$pV^{1.3}=c$$
So change it to
$$P2 = \frac{p1v1^{1.3}}{V2^{1.3}}$$
The "someone" who told you this is wrong (although you should know that without me having to tell you). The final pressure is correct. In the first step, you compressed the gas, and in the second step, the gas expanded. In the second step, you multiplied the volume from the first step to get you back to the original volume. Who is this "someone?"Ben_Walker1978 said:I have one more question.
Someone has told me for final pressure you don't divide by compression ratio.
Because i already divided my compression ration.
I have been told final pressure is wrong.
Are they right? Or is it correct?
Thanks.
No. In the first part, you divided the volume by the compression ratio. In the 2nd part, you multiplied the volume by the compression ratio (and divided the pressure by the compression ratio). You are aware that there is a difference between dividing the volume by the compression ratio and dividing the pressure by the compression ratio, right?Ben_Walker1978 said:Thank you for your reply.
Someone who i work with.
So because the gas has expanded then you need to divided it by the compression ratio again?
I was just making sure. As when he said it confused me.