What is the partial pressure of neon in a 4.00 L vessel that contains 0.838 mol...

What is the partial pressure of neon in a 4.00 L vessel that contains 0.838 mol of chloroform, 0.184 mol of ethane, and 0.755 mol of neon at a total pressure of 928 torr?

Solutions

Expert Solution

no of moles of CHCl3 ( nCHCl3) = 0.838 moles

no of moles of C2H6 ( n C2H6) = 0.184 moles

no of moles of Ne ( n Ne) = 0.755 moles

total no of moles = nCHCl3 + n C2H6 +n Ne

= 0.838+0.184+0.755 = 1.777 moles

mole fraction of neon ( X Ne) = n Ne/ nCHCl3 + n C2H6 +n Ne

= 0.755/1.777 = 0.425

partial pressure of neon = mole fraction of neon * total pressure

= 0.425*928 = 394.4torr >>>>>answer

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

At 4.00 L, an expandable vessel contains 0.864 mol of oxygen gas. How many liters of...

At 4.00 L, an expandable vessel contains 0.864 mol of oxygen gas. How many liters of oxygen gas must be added at constant temperature and pressure if you need a total of 1.36 mol of oxygen gas in the vessel? Express the volume to three significant figures, and include the appropriate units.

A mixture of neon and nitrogen gases contains neon at a partial pressure of 594 mm...

A mixture of neon and nitrogen gases contains neon at a partial pressure of 594 mm Hg and nitrogen at a partial pressure of 295 mm Hg. What is the mole fraction of each gas in the mixture? XNe = XN2 = A mixture of oxygen and neon gases at a total pressure of 674 mm Hg contains oxygen at a partial pressure of 299 mm Hg. If the gas mixture contains 2.48 grams of oxygen, how many grams of...

Determine the partial pressure and number of moles of each gas in a 14.25-L vessel at...

Determine the partial pressure and number of moles of each gas in a 14.25-L vessel at 30 degrees C containing a mixture of Xenon and neon gases only. The total pressure in the vessel is 6.70 atm and the mole fraction of xenon is 0.721 What is the partial pressure of Xenon? What is the partial pressure of neon? What is the number of moles of Xenon? What is the number of moles of neon?

If a 1.4-L reaction vessel initially contains 760 torr of N2O5 at 25 ∘C, what partial...

If a 1.4-L reaction vessel initially contains 760 torr of N2O5 at 25 ∘C, what partial pressure of O2 is present in the vessel after 220 minutes?

Determine the partial pressures and the total pressure in a 2.50-L vessel containing the following mixture...

Determine the partial pressures and the total pressure in a 2.50-L vessel containing the following mixture of gases at 17.8°C: 0.0254 mol He, 0.0571 mol H2, and 0.189 mol Ne. Also what is the partial total.

calculate the equilibrium pressure of CO2 in a closed 1 L vessel that contains each of...

calculate the equilibrium pressure of CO2 in a closed 1 L vessel that contains each of the following samples. Assume that ΔH∘ and ΔS∘ are independent of temperature: 15 g of MgCO3 and 1.0 g of MgO at 25 ∘C 15 g of MgCO3 and 1.0 g of MgO at -40 ∘C 30 g of MgCO3 and 1.0 g of MgO at -40 ∘C

1.00 mol of A and 1.00 mol of B are placed in a 4.00-L container. After...

1.00 mol of A and 1.00 mol of B are placed in a 4.00-L container. After equilibrium is established, 0.400 mol of D is present in the container. Calculate the equilibrium constant for the reaction: A(g) + 3 B(g) <---> C(g) + 2 D(g)

A cylinder of volume 0.240 m3 contains 10.1 mol of neon gas at 21.6°C. Assume neon...

A cylinder of volume 0.240 m3 contains 10.1 mol of neon gas at 21.6°C. Assume neon behaves as an ideal gas (g) Compute ΔU − W. (i) Compute Q, the thermal energy transfer.

When 4.00 moles of PCl5 (g) is put in a 1.00 L vessel the equilibrium: PCl3...

When 4.00 moles of PCl5 (g) is put in a 1.00 L vessel the equilibrium: PCl3 (g) + Cl2 (g) <--> PCl5 (g) is established. At equilibrium [Cl2]e = 5.20 x 10^-3 M. What is Kc for this equilibrium as written? a.) 9.61 x 10^2 b.) 6.77 x 10^-6 c.) 1.48 x 10^5 d.) 9.0 x 10^-6 e.) impossible to determine

A. 4.00×10−3 mol of HBr are dissolved in water to make 17.0 L of solution. What...

A. 4.00×10−3 mol of HBr are dissolved in water to make 17.0 L of solution. What is the concentration of hydroxide ions, [OH−], in this solution? B. 8.00 g of NaOH are dissolved in water to make 2.00 L of solution. What is the concentration of hydronium ions, [H3O+], in this solution? Express your answer with the appropriate units.

Subjects