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anonymous
 one year ago
what would be the pressure of a given mass of a gas, if its volume and temperature are doubled ............. ?
anonymous
 one year ago
what would be the pressure of a given mass of a gas, if its volume and temperature are doubled ............. ?

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anonymous
 one year ago
Best ResponseYou've already chosen the best response.0Considering an ideal gas, you can use the relation: \[PV=nRT\] taking \(n\) (the nomber of molecules) as a constant, since the mass is not changing, and since \(R\) is the ideal gas constant we get: \[\frac{PV}{T}=constant\] so if you double the volume and temperature you must get the same constant value for that expression, and then: \[\frac{P_1V_1}{T_1}=\frac{P_2(2V_1)}{2T_1}\] what is the relation between the new pressure \(P_2\) and \(P_1\) ??

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0he wants complement one word

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0that word is contained in the response to my question: what is the relation between the new pressure \(P_2\) and \(P_1\) ?? What happens if we cancel out the 2's in the right hand side?
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