10.0 grams of argon and 20.0 grams of neon are placed in a 1015.0 ml container...

Question

Question

10.0 grams of argon and 20.0 grams of neon are placed in a 1015.0 ml container at 35.0 °C. The partial pressure of neon is ________ atm.

1. 29.7

2. 60.7

3. 6.23

4. 24.7

5. 2.81

Answer 1

Answer #1

Moles of neon: moler mass 20.01 to 20 - 1 mol pressure molux gas const. x Temperature volume I notx (0.08211 - alom ) x ( 35+

Answer 2

Similar Homework Help Questions

30.0 grams of argon and 15.0 grams of xenon are placed in a 170.9 ml container...

30.0 grams of argon and 15.0 grams of xenon are placed in a 170.9 ml container at 21.8 °C. The partial pressure of xenon is ________ atm
Page 2 of 3 5. What is the pressure in atm of a sample of 25.0 g of argon gas in a 4.00 L container and a temperatu...

Page 2 of 3 5. What is the pressure in atm of a sample of 25.0 g of argon gas in a 4.00 L container and a temperature of 27°C? (10 pts) 6. What is the volume of a sample of 64.0 g of oxygen gas at a pressure of 745 torr and a temperature of 25.0°C? (10 pts) 7. How many grams of neon are in a 20.0 L steel tank at a pressure of 987 torr and a...
If 1.00 mol of argon is placed in a 0.500-L container at 30.0 ∘C , what...

If 1.00 mol of argon is placed in a 0.500-L container at 30.0 ∘C , what is the difference between the ideal pressure (as predicted by the ideal gas law) and the real pressure (as predicted by the van der Waals equation)? For argon, a=1.345(L2⋅atm)/mol2 and b=0.03219L/mol.

A 500.0-mL sealed flask contains 0.060 mol of neon and 0.050 mol of argon at 25°C....

A 500.0-mL sealed flask contains 0.060 mol of neon and 0.050 mol of argon at 25°C. Select the correct partial pressures for each of the gases. R=0.0821 L.atm/K-mol Check all that apply. Pe= 5.4 atm P = 2.9 atm P.-2.9 atm = 5.4 atm Ar PA = 2.4 atm Do you know the answer?
If 1.00 mol of argon is placed in a 0.500-L container at 30.0 ∘C , what...

If 1.00 mol of argon is placed in a 0.500-L container at 30.0 ∘C , what is the difference between the ideal pressure (as predicted by the ideal gas law) and the real pressure (as predicted by the van der Waals equation)? For argon, a=1.345(L2⋅atm)/mol2 and b=0.03219L/mol. Express your answer to two significant figures and include the appropriate units.
If 1.00 mol of argon is placed in a 0.500-L container at 22.0 ∘C , what...

If 1.00 mol of argon is placed in a 0.500-L container at 22.0 ∘C , what is the difference between the ideal pressure (as predicted by the ideal gas law) and the real pressure (as predicted by the van der Waals equation)? For argon, a=1.345(L2⋅atm)/mol2 and b=0.03219L/mol. Express your answer to two significant figures and include the appropriate units.

50.0 g of calcium carbonate are placed in a container with 20.0 g of CaO and...

50.0 g of calcium carbonate are placed in a container with 20.0 g of CaO and 1.04 atm carbon dioxide. What will the equilibrium pressure be in the container? How much calcium carbonate will be left at equilibrium? CaCO3 (s) ⇌ CaO(s) + CO2 (g) KP = 1.04 atm at 900 °C
CO (5.00 g) and CO2 (5.00 g) were placed in a 750.0 mL container at 50.0°C....

CO (5.00 g) and CO2 (5.00 g) were placed in a 750.0 mL container at 50.0°C. The partial pressure of CO2 in the container was __________ atm. 4.02 10.3 1.60 0.292 6.31
A mixture of neon and oxygen gases, at a total pressure of 635 mm Hg, contains 2.31 grams of neon and 2.80 grams of oxy...

A mixture of neon and oxygen gases, at a total pressure of 635 mm Hg, contains 2.31 grams of neon and 2.80 grams of oxygen. What is the partial pressure of each gas in the mixture? PNe = mm Hg mm Hg What volume of oxygen gas is produced when 42.5 g of mercury(II) oxide reacts completely according to the following reaction at 25 °C and 1 atm? mercury(II) oxide (s) — mercury (1) + oxygen(g) liters oxygen gas

4. In a steel container of 20.0 L, at a temperature of 25.0°C, we have a...

4. In a steel container of 20.0 L, at a temperature of 25.0°C, we have a mixture of F2(g) and Cl2(g). The partial pressure of F2(9) is 6.77 atm and that of C2(g) is 2.44 atm. The following reaction takes place: 5 F2(g) +C2(9)2 CIF(g). What mass of CIFs(g) can be produced? If all of the limiting reagent were to react, what would be the partial pressure of the excess reagent? The volume is fixed at 20.0 L and the...