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We have $O_2$, $H_2$, $He$, and $HCl$ gases; which gas will behave LEAST ideally?
Ideality assumes negligible intermolecular interaction. However, $"hydrogen chloride gas"$, with $""^(delta+)H-Cl^(delta-)$ dipoles, has the possibility of intermolecular hydrogen , which is a potent intermolecular force. This is reflected in the...
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The volume of a fixed amount of gas is doubled, and the absolute temperature is doubled. According to the ideal gas law, how has the pressure of the gas changed?
$P_1=(nRT)/V$ $P_2=(nRxx2T)/(2V)$ $=$ $(nRxxcancel2T)/(cancel2V)$ $=$ $P_1$. Capisce?
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Container A holds 757 mL of ideal gas at 2.60 atm. Container B holds 164 mL of ideal gas at 4.80 atm. If the gases are allowed to mix together, what is the resulting pressure?
The ideal gas equation of state is $PV = nRT$ In this problem we may consider the temperature to be constant, so we can set up an equation that...
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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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When using the ideal gas constant value, R = 0.0821, in an ideal gas law calculation, what are the units of volume?
$"R=0.0821 L atm K"^(-1) "mol"^(-1)"$
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When do real gases behave most like ideal gases?
An ideal gas has the following qualities: $1$ The particles are extremely tiny compared to the volume filled by the gas - like mathematical points. $2$ The particles are...
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Under what conditions of temperature and pressure does oxygen gas behave least like an ideal gas?
"Ideal" behavior is best seen at moderate temperatures and pressures. Dense gases - either near their liquefaction point or their supercritical point - will deviate the most from ideal gas...
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Container A holds 737 mL of ideal gas at 2.30 atm. Container B holds 114 mL of ideal gas at 4.40 atm. lf the gases are allowed to mix together, what is the resulting pressure?
According to Dalton's Law of Partial Pressures, each gas will exert its pressure independently of the other. Hence we can use to calculate the pressure of each gas separately...
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The attached plot shows the
ratio of PV to RT for 1.0 mole of nitrogen
gas as a function of pressure at T=1000K.
Explain why the ratio should be 1.0 for
an ideal gas, and why nitrogen does not
behave ideally at high pressures?
The ideal gas law is an idealization. What does this mean? It means that we idealize the behaviour of real gases. We assume that gases are mostly empty space, that...
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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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