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A 2.01-L sample of O2(g) was collected over water at a total pressure of 785 torr and 25°C. When the O2(g) was dried (water vapor removed), the gas has a volume of 1.92 L at 25°C and 785 torr. How would you calculate the vapor pressure of water at 25°C?
At constant number of mole $n$ and Temperature $T$, using the $PV=nRT$ we can write: $P_1V_1=P_2V_2$ We should calculate the pressure of pure $O_2$ in a $2.01L$ volume: $P_1=(P_2V_2)/V_1=(785" torr"xx1.92cancel(L))/(2.01cancel(L))=750"...
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At 20°C the vapor pressure of benzene (C6H6) is 75 torr, and that of toluene (C7H8) is 22 torr. Assume that benzene and toluene form an ideal solution.
What is the composition in mole fractions of a solution that has a vapor pressure of 40. torr at 20°C?
The idea here is that the vapor pressures of benzene and toluene will contribute to the total vapor pressure of the solution proportionally to their respective mole fraction - this...
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A sample of gas has a volume of 12 liters at 0°C and 380 torr. What will be its volume when the pressure is changed to 760 torr at a constant temperature?
$PV = nRT$ $P$ is pressure in atm (760 torr = 1 atm); $V$ is volume in liters; $n$ is the number of moles; $R$ is the constant 0.0821; $T$...
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If an ideal gas occupies 27.5 ml at 760 torr and 23 °C then, what volume would the same gas occupy at standard conditions?
The volume of the gas at STP is 25.4 mL When you examine the question, you see that the pressure does not change. Standard pressure is 760 Torr. The only...
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The volume of a sample of gas is 4.50 L at STP What volume will the sample occupy at 20.0$"^o$C and 650.0 torr?
First, recall that “Standard” temperature and pressure are 0’C and 1 atm (760Torr), as opposed to “Normal” temperature and pressure of 20’C and 1 atm. In the calculations all...
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A gas sample containing only SO2, PF3, and CO has the following mass percentage: 29.1 % SO2, 61.8 % PF3. How would you calculate the partial pressure in torr, of CO if the total pressure of sample is 684 torr?
The idea here is that the exerted by a gas that's part of a gaseous mixture is proportional to its mole fraction. This means that in order to find...
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Find the partial pressure in a solution containing ethanol and 1-propanol with a total vapor pressure of $"56.3 torr"$? The pure vapor pressures are $"100.0 torr"$ and $"37.6 torr"$, respectively, and the solution has a mol fraction of $0.300$ of ethanol.
Consider Raoult's law compared with Dalton's law of partial pressures: $P_i = overbrace(chi_(i(l))P_i^"*")^"Raoult's Law" = underbrace(chi_(i(v))P_"tot")_"Dalton's Law"$, where: $P_i$ is the partial vapor pressure of component $i$, i.e....
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A mixture of $"N"_2$, $"O"_2$. and $"CO"_2$ has a total pressure of $"740 torr"$ In this mixture, the partial pressure of $"N"_2$ is $"120 torr"$ and the partial pressure of $"O"_2$ is $"400 torr"$. What is the partial pressure of $"CO"_2$ ?
From Dalton's Law of , the total pressure of a mixture of gases is the sum of the partial pressures of each gas. Therefore, the partial pressure of $"CO"_2$ is...
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A sample of propane, a component of LP gas, has a volume of 35.3 L at 315 K and 922 torr. What is its volume at STP?
STP conditions are defined as a pressure of $"100 kPa" = 100 color(red)(cancel(color(black)("kPa"))) * (1color(red)(cancel(color(black)("atm"))))/(101.325color(red)(cancel(color(black)("kPa")))) * "760 torr"/(1color(red)(cancel(color(black)("atm")))) ="750.1 torr"$ and a temperature of $0^@"C" =...
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What is the mol fraction of ethylene glycol in the solution phase for an aqueous solution with a vapor pressure of $"760 torr"$ if the pure vapor pressure was $"1077 torr"$?
I got $0.294$. Raoult's law states: $P_j = chi_j^lP_j^"*"$, where: $P_j$ is the partial vapor pressure above the solution coming from the component $j$ in solution....
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