If you keep pressure constant, the gas is expanding from 0.120 L to 0.610 Liters. Take the change in Volumes and multiply it by pressure to get the work done....
1 Answers 1 viewsOld $"Dalton's Law of Partial Pressures"$ states that in a gaseous mixture, the exerted by a component gas is the same as it would have exerted if it alone occupied...
1 Answers 1 viewsThis is a clear application of $"Boyle's Law"$ $Pprop1/V$ And thus, $P_1V_1=P_2V_2$ We note that $1*atm-=760*mm*Hg$ $P_2=(P_1V_1)/V_2$ $=$ $((850*mm*Hg)/(760*mm*Hg*atm^-1))xx(3.30*L)/(5.63*L)$ $=$ $??atm$ This is not a good question. It has...
1 Answers 1 viewsApply $"Pressure "xx" Volume "=" Constant"$ The temperature being constant $P_1V_1=P_2V_2$ The initial volume is $V_1=2L$ The initial pressure $P_1=1atm$ The final pressure is $P_2=6*10^4atm$ The final volume is...
1 Answers 1 viewsFrom the $PV=nRT$ we can conclude that $n=(PV)/(RT)$. If the pressure $P$, the volume $V$ and the temperature $T$ of the gas change between two points, this change can be...
1 Answers 1 viewsRaising the temperature will increase the volume: $V_T=(300K)/(200K)xx24.0L=36.0L$ Increasing the pressure will decrease the volume: $V_(T,p)=(10.0atm)/(14.0atm)xx36.0L~~25.7L$ It doesn't matter if you first do the one and then the other, or...
1 Answers 1 viewsAnd so.................. $V_2=(P_1xxV_1xxT_2)/(T_1xxP_2)$ $=(2.31*atmxx17.5*Lxx350*K)/(299*Kxx1.75*atm)<=30*L.$
1 Answers 1 viewsUsing $PV=nRT$ and knowing that $nRT$ stays constant you should get: $P_1V_1=P_2V_2$ or $6.414*850=V_2*4423$ and $V_2=1.232 liters$
1 Answers 1 viewsBoyles Law is the only inverse relationship between gas phase variable of the Empirical Gas Law set. That is ... For the Empirical the primary variables considered are Pressure...
1 Answers 1 viewsThis is an example of a problem. $color(blue)(|bar(ul((P_1V_1)/T_1 = (P_2V_2)/T_2|)$ We can rearrange this formula to get $V_2 = V_1 × P_1/P_2 × T_2/T_1$...
1 Answers 1 views