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anonymous
 one year ago
Can someone please help me with this? I need equation help.
anonymous
 one year ago
Can someone please help me with this? I need equation help.

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anonymous
 one year ago
Best ResponseYou've already chosen the best response.0If a 10. m^3 volume of air (acting as an ideal gas) is at a pressure of 760 mm and a temperature of 27 degrees Celsius is taken to a high altitude where the pressure is 400. mm Hg and a temperature of 23 degrees Celsius, what volume will it occupy? (Hint: remember the temperature must be in Kelvin).

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0This is the question. The formulas I was given are:

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0\[P_{1}V _{1} = P_{2} V_{2}\]

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0\[V_{1}/T_{1} = V_{2}/T_{2}\]

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0\[P_{1} V_{1}/T_{1} = P_{2} V_{2}/ T_{2}\]

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0I have no idea which formula to use, or if I need to make conversions from the 400 mm Hg

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0@Robert136 could you maybe look? I would appreciate it so much

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0@Robert136 could you maybe look? I would appreciate it so much

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0The question is poorly worded. Try again.

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0I know.. I'll give you a medal anyway since you were kind enough to reply

anonymous
 one year ago
Best ResponseYou've already chosen the best response.01.Assume that there is 10m^3 volume of air 2.The air above has a pressure of 760mm & temperature of 300 Kelvin degrees 3.The air mentioned above is taken to where pressure is 400mm and 250 Kelvin 4. Calculate the volume that results from change in temperature and pressure.

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0Ah I see now. So I need to plug those values into the last equation I posted and solve?

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0Thank you so so much! That cleared up a ton of confusion! I appreciate it! :D

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0No problem. I am assuming this is a last year high school chemistry or first year university?

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0I had to do it a while ago

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0It's actually for Physics. They taught me how to use the formulas but threw this curveball at me, and I had no idea what formula would work or if I needed to do conversions for it beforehand.

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0Oh I see your problem now. Make sure to use the Kelvin. Usually units of the pressure doesn't matter because they are all proportional .

IrishBoy123
 one year ago
Best ResponseYou've already chosen the best response.0for an ideal gas, you will have been given something like \(\huge pV= nRT\) as R = const, we can say: \(\huge \frac{pV}{nT} = const\) as it is the same amount of gas, we can say \(\huge \frac{pV}{T} = const\) but as @Robert136 so expertly points out, you need to be sure that you use Kelvin and you are solving \(\huge \frac{p_1V_1}{T_1} = \frac{p_2V_2}{T_2}\) thus \(\huge V_2 = \frac{T_2}{T_1} . \frac{ p_1 }{ p_2}\ . V_1\) again, using Kelvin https://gyazo.com/dad5d1f102f61add6b05a906ef9a617f

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0@IrishBoy123 thank you for your response! :D
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