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How do i calculate the number of moles of magnesium, chlorine, and oxygen atoms in 7.70 moles of magnesium perchlorate, $"Mg"("ClO"_4)_2$. Express the number of moles of Mg, Cl, and O atoms numerically, separated by commas. moles of Mg, Cl, O =?
$1 "mol" " Mg"("ClO"_4)_2$ contains :- $color(red)(1 "mol Mg atoms")$ $color(blue)(2 "mol Cl atoms"$ $color(green)(8 "mol O atoms"$ To find no. of moles of each element,...
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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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A sample of gas occupies 21 L under a pressure of 1.3 atm. What would the resulting volume be if the pressure were increased to 3.9 atm if the temperature did not change?
We apply $P_1V_1=P_2V_2$ The initial volume is $V-1=21L$ The initial pressure is $P_1=1.3 atm$ The final pressure is $P_2=3.9atm$ The final volume is $V_2=P_1/P_2*V_1=1.3/3.9*21$ $=7 L$
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A mixture of neon and oxygen gases, in a 9.77 L flask at 65 °C, contains 2.84 grams of neon and 7.67 grams of oxygen. The partial pressure of oxygen in the flask is ? atm and the total pressure in the flask is atm?
We can use the to calculate the partial pressures. $color(blue)(bar(ul(|color(white)(a/a)pV = nRTcolor(white)(a/a)|)))" "$ or $p = (nRT)/V$ The number of moles $n$...
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A 1.2-liter tank at a temperature of 27°C contains a mixture of 1.5 moles of oxygen, 1.2 moles of nitrogen, and 1.6 moles of hydrogen. What is the total pressure of the mixture inside the tank?
Dalton's law of partial pressures states that in a gaseous mixture, the pressure exerted by a component is the same as it would exert if it alone occupied the container....
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A flask contains oxygen, carbon dioxide, and nitrogen gases. The partial pressures of each are 11.4 atm, 5.6 atm, and 8.7 atm respectively. What is the total pressure in the flask in atm?
The total pressure is the sum of the pressures of the three gases in the flask. $"pressure"_"total" ="11.4 atm + 5.6 atm + 8.7 atm" = "25.7 atm"$
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A vessel collects Gas B over water at 35 C. Within the container, the total pressure is 110 kPa. How do you calculate the partial pressure of Gas B if the water vapor pressure at 35°C is 5.6 kPa?
$P_"container"=P_"gas B"+P_"SVP"$. Here $P_"SVP"$ is the so-called $"saturated vapour pressure (of water)"$. $P_"SVP"$ is usually tabulated, and (typically) quoted in units of $mm*Hg$; it varies according to temperature. Are you...
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A mixture of .250 moles O2, .297 moles N2, and .134 moles Ar has a total pressure of 1.95 atm. What is the mole fraction of O2 and what is the partial pressure of O2?
$"Mole fraction of a gas"=("Number of moles of gas")/("Total moles of gas")$ For $O_2$: $"Mole fraction of"$ $O_2$ $= 0.250/(0.250+0.134+0.297)=0.250/0.681~~0.367$ $"Partial pressure of a gas" = "Mole fraction"...
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A mixture of $2.00$ moles of $"H"_2$, $3.00$ moles of $"NH"_3$, $4.00$ moles of $"CO"_2$, and $5.00$ moles of $"N"_2$ exerts a total pressure of $"800. mmHg"$. What is the partial pressure of each gas?
The idea here is that the of each gas will be proportional to the mole fraction each gas has in the mixture $->$ think Dalton's Law of Partial Pressures....
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A student collects $450$ $mL$ of $HCl (g)$ at a pressure of $100$ $kPa$ and a temperature of $17°C$. What is the new volume of the $HCl$ at standard temperature and pressure?
First convert the temperature to kelvin: $17+273=290$ $K$. Standard temperature is $273$ $K$. Now $100$ $kPa$ is already standard pressure, so the pressure is constant. We should work in...
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