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A cylinder with a movable piston contains a 2.0-liter sample of neon at gas at STP. What is the volume of this of this sample when its temperature is increased to 30. deg C while its pressure is decreased to 90. kilopascals?
Recall, $1"mol" = 22.4"L"$ for most gases, and $PV = nRT$ We're looking to calculate the new volume of the sample (via the ideal gas law) when heat is added...
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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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$60*g$ of ammonia gas, and $2.5*mol$ dihydrogen gas, are confined in a piston at $"STP"$. What is the volume of the piston?
$V = (nRT)/P$. Use an appropriate gas constant, $R$, i.e. $8.314$ $J$ $ K^-1$ $mol^-1$. All you need to do is calculate the moles of each gas, dihydrogen, and of...
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A given mass of oxygen occupies 200 ml when the pressure is 400 mm of Hg. What volume will the gas occupy when the pressure is raised to 200 mmHg, provided the temperature remains constant?
Now we know that $1*atm$ pressure will support of column of mercury $760*mm$ high. A pressure of LESS than one atmosphere will support a column of mercury LESS than this...
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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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An ideal gas at constant temperature is confined In an airtight cylinder, and a piston pushes down on the gas in the cylinder. Assuming the gas behaves as an ideal gas during the compression, what effect will this have on the pressure of the ideal gas?
You are compressing a gas. Is the volume going to increase? Is it going to decrease? If you compress the volume of a gas what is going to happen to...
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Under a pressure of $1.2*atm$ a gas occupies an $8*mL$ volume in a piston. What pressure develops if the volume is increased to $12*mL$?
holds that $P_1V_1=P_2V_2$ at constant temperature. And thus $P_2=(P_1V_1)/V_2=(1.2*atmxx8*mL)/(12*mL)=0.8*atm$. This decrease in pressure is reasonable, given that we have INCREASED the volume.
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A sample of carbon dioxide gas at a pressure of 1.07 atm and a temperature of 166 °C, occupies a volume of 686 mL. If the gas is heated at constant pressure until its volume is 913 mL, the temperature of the gas sample will be ? °C.
The idea here is that the volume and the temperature of a gas have a direct relationship when the pressure and the number of moles of gas are being kept...
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A sample of gas occupies a volume of 50.0 milliliters in a cylinder with a movable piston. The pressure of the sample is 0.90 atmosphere and the temperature is 298 K. What is the volume of the sample at STP?
Use the $(P_1V_1)/T_1=(P_2V_2)/T_2$. $"STP=273.15 K and 1 atm"$ Given/Known $P_1="0.90 atm"$ $V_1="50.0 mL"$ $T_1="298 K"$ $P_2="1 atm"$ $T_2="273.15 K"$ Unknown $V_2$ Solution Rearrange the equation to isolate $V_2$ and solve....
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