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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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Initially a gas is at a pressure of 12 atm, a volume of 23 L, and a temperature of 200 K, and then the pressure is raised to 14 atm and the temperature to 300 K. What is the new volume of the gas?
$V_2$ $=$ $(P_1V_1T_2)/(P_2T_1)$ $(12*atmxx23*Lxx300K)/(14*atmxx200*K)$ $=$ $??L$ The volume has increased reasonably in that the temperature has increased substantially, yet the pressure has only increased marginally.
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The pressure on a sample of an ideal gas is increased from 715 mmHg to 3.55 atm at constant temperature. If the initial volume of the gas is 485 mL, what is the final volume of the gas?
At constant $T$, $P_1V_1=P_2V_2$; this is Boyle's law. Now $P_1=(715*mm*Hg)/(760*mm*Hg*atm^-1)=0.941*atm$ $V_2=(P_1V_1)/P_2=(0.941*cancel(atm)xx485*mL)/(3.55*cancel(atm))=129*mL$
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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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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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Nitrogen gas (N2) reacts with hydrogen gas (H2) to form ammonia (NH3). At 200°C in a closed container, 1.05 atm of nitrogen gas is mixed with 2.02 atm of hydrogen gas. At equilibrium the total pressure is 2.02 atm. What is the partial pressure of hydrogen gas at equilibrium?
First, write the balanced chemical equation for the equilibrium and set up an ICE table. $color(white)(XXXXXX)"N"_2 color(white)(X)+color(white)(X)"3H"_2 color(white)(l)⇌ color(white)(l)"2NH"_3$ $"I/atm": color(white)(Xll)1.05 color(white)(XXXl)2.02 color(white)(XXXll)0$ $"C/atm": color(white)(X)-x color(white)(XXX)-3x color(white)(XX)+2x$ $"E/atm": color(white)(l)1.05- x...
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What is the initial pressure of a gas having an initial temperature of 90.5K, an initial volume of 40.3 L, final pressure of .83 atm, a final temperature of .54 K and a final volume of 2.7L?
Use the . $(P_1V_1)/T_1=(P_2V_2)/T_2$ Given $V_1="40.3 L"$ $T_1="90.5 K"$ $P_2="0.83 atm"$ $V_2="2.7 L"$ $T_2="0.54 K"$ Unknown $P_1$ Equation $(P_1V_1)/T_1=(P_2V_2)/T_2$ Solution Rearrange the equation to isolate $P_1$ and solve. $P_1=(P_2V_2T_1)/(T_2V_1)$ $P_1=((0.83"atm"...
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Fifty liters of gas is kept at a temperature of 200 K and under pressure of 15 atm. The temperature of the gas is increased to 400 K. The pressure is decreased to 7.5 atm. What is the resulting volume of the gas?
Even without doing any calculations, you should be able to look at the information given and predict that the volume of the gas will increase after temperature is increased and...
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If I initially have a gas at a pressure of 12 atm, a volume of 23 liters, and a temperature of 200 K, and then l raise the pressure to 14 atm and increase the temperature to 300 K, what is the new volume of the gas?
This 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 $V_2 = V_1 × P_1/P_2 × T_2/T_1$...
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