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A gas evolved during the fermentation of sugar was collected at 22.5°C and 702 mmHg. After purification its volume found to be 25.0 L. How many moles of gas were was collected? R = 0.0821 L*atm/K*mol
$n=(PV)/(RT)=((702*mm*Hg)/(760*mm*Hg*atm^-1)xx25.0*L)/(0.0821*L*atm*K^-1*mol^-1xx295.5*K)$ $~=$ $1*mol$ This value makes sense, in that we are close to $1*atm$, and $298*K$ in the given conditions. By the way? I forgot to ask something...
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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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What is the pressure exerted by 32.00 g of Oxygen gas in a 20. L container at 30.00 C? Use R = 0.0821 L atm/mol k?
First, let's determine the number of mole of oxygen gas. Using $n = frac(m)(M)$: $Rightarrow n("O") = (frac(32.00)(2 times 15.99))$ $"mol"$ $Rightarrow n("O") = (frac(32.00)(31.98))$ $"mol"$ $therefore n("O") = 1.00$...
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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 should I use the ideal gas law and not the combined gas law?
Good question! Let's look at the and the . Ideal Gas Law: PV=nRT Combined Gas Law: $P_1*V_1/T_1 = P_2*V_2/T_2$ The difference is the presence of "n" the number of...
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How does the ideal gas law differ from the combined gas law?
The describes states that $(PV)/T=k$ is a constant for any fixed quantity of gas, but the extends this to say that the value of the constant is proportional to the...
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What is the relationship between the combined gas law and the ideal gas law?
The and the are the same relationships written in different ways. The Combined Gas Law is a combination of Boyle's, Charles' and Gay-Lussac's laws. $PV$ = constant $V/T$ = constant...
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How would you derive the ideal gas law PV= nRT using Avogadros law, Boyles law, and Charles law?
According to , $color(red)(v prop1/p" "$when $" "color(green)(T" & "n$ constant. According to Charle's Law, $color(red)(v prop T" "$when $" "color(green)(p" "&" "n$ constant....
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An ideal gas is compressed at a constant pressure of 120 kPa to one-half of its initial volume. The work done on the gas is 790 J. What was the initial volume of the gas?
$V_1 = "13.2 L"$ $V_2 = "6.6 L"$ This is asking you about the definition of work. $\mathbf(w = -PDeltaV$ ($DeltaV = V_2 - V_1$.)...
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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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