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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.
In this case, the piston is doing work on the environment so it would lose E, and thus your answer should be a negative number.
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Five gases combined in a gas cylinder have the following partial pressures 3.00 atm ($N_2$), 1.80 atm ($O_2), 0.29 atm (Ar), 0.18 atm (He), and 0.10 atm (H). What is the total pressure that is exerted by the gases?
Old $"Dalton's Law of Partial Pressures"$ states that in a gaseous mixture, the exerted by a component gas is the same as it would have exerted if it alone occupied...
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A rigid cylinder with a movable piston contains 500 liters of a gas at 30.0 C with a pressure of 1.00 atmosphere. What is the volume of the gas in the cylinder at STP?
This is an example of a problem. $color(blue)(bar(ul(|color(white)(a/a)(p_1V_1)/T_1 = (p_2V_2)/T_2color(white)(a/a)|)))" "$ We can rearrange this formula to get $V_2 = V_1 × p_1/p_2 ×...
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If I have 5.6 liters of gas in a piston at a pressure of 1.5 atm and compress the gas until its volume is 4.8 L, what will the new pressure inside the piston be?
At constant $T$, $P_1V_1=P_2V_2$....... We solve for $P_2=(P_1V_1)/V_2$, and clearly the $"RHS"$ will have the required units of pressure: $P_2=(1.5*atmxx5.6*L)/(4.8*L)=1.75*atm$ That $P_2>P_1$ is quite reasonable, because we are compressing the...
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A gas takes up a volume of 19.5 liters, has a pressure of 2.9 atm, and a temperature of 5.5°C. If I raise the temperature to 65°C and lower the pressure to 1.5 atm, what is the new volume of the gas?
From 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...
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A cylinder with a moving piston expands from an initial volume of 0.250 L against an external pressure of 2.00 atm. The expansion does 288 J of work on the surroundings. What is the final volume of the cylinder?
This is asking you to apply the definition of reversible work: $w_"rev" = -P int_(V_1)^(V_2) dV$ $= -P (V_2 - V_1) = -"288 J"$ Since the gas did...
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If I initially have a gas at a pressure of 10.0 atm, a volume of 24.0 liters, and a temperature of 200. K, and then I raise the pressure to 14.0 atm and increase the temperature to 300. K, what is the new volume of the gas?
Raising 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...
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A gas takes up a volume of 17.5 liters, has a pressure of 2.31 atm, and a temperature of 299 K. lf the temperature is increased to 350 K and the pressure is decreased to 1.75 atm, what is the new volume of the gas?
And so.................. $V_2=(P_1xxV_1xxT_2)/(T_1xxP_2)$ $=(2.31*atmxx17.5*Lxx350*K)/(299*Kxx1.75*atm)<=30*L.$
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A sample of gas in a cylindrical chamber with a removable piston occupied a volume of 6.414 liters when the pressure was 850 torr and the temperature was 27.2 degree C. The Pressure was just readjusted to 4423 torr by moving the piston. ?
Using $PV=nRT$ and knowing that $nRT$ stays constant you should get: $P_1V_1=P_2V_2$ or $6.414*850=V_2*4423$ and $V_2=1.232 liters$
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At a pressure 47 kPa, the gas in a cylinder has a volume of 12 liters. Assuming temperature remains the same, if the volume of the gas is decreased to 8 liters, what is the new pressure?
Boyles 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...
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Find the amount of heat energy needed to convert 400 grams of ice at -38°C to steam at 160°C?
1284440 Joules
246840 Joules
331056 Joules
159984 Joules
And $"(ii) the LATENT heat of fusion of ice...."$ And $"(iii) the heat capacity of liquid water...."$ And $"(iv) the heat of vaporization of water...."$ And $"(v) the heat capacity...
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