A 2.00 L reaction container at 25.0 °C contains CO2 (g) and O2 (g). The total...

A 2.00 L reaction container at 25.0 °C contains CO₂ (g) and O₂ (g). The total pressure of the gases in the container was 656 torr and the mole fraction of CO₂ is 0.245.

Calculate the partial pressure of oxygen gas in the mixture

Calculate the mass of oxygen gas in the mixture (in g).

Which gas will rise to the top of the container? Explain your answer.

Calculate the total volume of the container if 15.0 g of helium gas was added to the initial mixture of CO₂ and O₂ gases at STP.

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queen_honey_blossom answered 2 years ago

A gas mixture contains 1.25 g N2 and 0.84 g O2 in a 1.53-L container at...

A gas mixture contains 1.25 g N2 and 0.84 g O2 in a 1.53-L container at 14 ∘C. A.) Calculate the mole fraction of N2. B.) Calculate the mole fraction of O2. C.) Calculate the partial pressure of N2. D.) Calculate the partial pressure of O2.

Consider the reaction N2O4 (g) ? 2 NO2 (g). At equilibrium, a 2.00-L reaction vessel contains...

Consider the reaction N2O4 (g) ? 2 NO2 (g). At equilibrium, a 2.00-L reaction vessel contains NO2 at a pressure of 0.269 atm and N2O4 at a pressure of 0.500 atm. The reaction vessel is then compressed to 1.00 L. What will be the pressures of NO2 and N2O4 once equilibrium is re-established?

- 25.0-L tank contains 295 g N2, 135 g O2, and 24.0 He gases. Calculate the...

- 25.0-L tank contains 295 g N2, 135 g O2, and 24.0 He gases. Calculate the partial pressure of each gas and the total gas pressure at 20.0oC. (Answer: PN2 = 10.1 atm; PO2 = 4.06 atm; PHe = 5.77 atm; Ptotal = 19.9 atm) - A 5.0-gallon gas tank contains N2 and H2 gas, such that the partial pressure of H2 is three times that of N2 gas. If the total gas pressure is 2.4 atm at 25oC,...

When propane is burned, the balanced reaction is: C3H8(l) + 5 O2(g) -> 3 CO2(g) +...

When propane is burned, the balanced reaction is: C3H8(l) + 5 O2(g) -> 3 CO2(g) + 4 H2O(g). If 31.66 L of water vapor are produced at 865.7 torr and 75°C, how many grams of propane were burned?

Consider the combustion of butane: C4H10(g) +O2(g)->CO2(g)+H2O(l) (unbalanced) Let 2.00 g of butane gas and 3.05...

Consider the combustion of butane: C4H10(g) +O2(g)->CO2(g)+H2O(l) (unbalanced) Let 2.00 g of butane gas and 3.05 atm of oxygen gas completely react (limiting) in a 2.00-L container at 125C. 2.1 Will there be a net increase or decrease in total pressure after the reaction is complete? 2.2 After complete reaction, what will be the mole fraction of H2O gas in the system?

a 2.00 l container holds 4.00 moles of o2 and 2.70 moles of he at 293...

a 2.00 l container holds 4.00 moles of o2 and 2.70 moles of he at 293 k. What is the partial pressure of o2? He? what is the total pressure?

2.00 moles of CO2 and 1.50 moles of H2 are placed into a rigid 5.00-L container...

2.00 moles of CO2 and 1.50 moles of H2 are placed into a rigid 5.00-L container and they react according to the equation ? ? CO2(g) + H2(g) ? CO(g) + H2O(g) ? ? K = 2.50 What will be the concentration of carbon monoxide when equilibrium is reached?

Balance the combustion reaction of chrysene (C18H12) at 298K. C18H12(s)+ O2(g) CO2(g) + H2O(l) What is...

Balance the combustion reaction of chrysene (C18H12) at 298K. C18H12(s)+ O2(g) CO2(g) + H2O(l) What is the value of ng for the combustion reaction? ng = mol What is Hcomb of chrysene if Ecomb = -8942.6 kJ/mol? Hcomb = kJ/mol What is the heat of formation of chrysene? See Thermodynamic Properties Hf = kJ/mol

Consider the following reaction at 25.0 °C and 760.0 torr: SO3 (l) → SO2 (g) +...

Consider the following reaction at 25.0 °C and 760.0 torr: SO3 (l) → SO2 (g) + ½ O2 (g) The following data were obtained. Compound H°f(kJ/mole) SO3 (l) -395.7 SO2(g) -296.8 O2(g) 0.00 Calculate ∆H° for the reaction. The reaction is ________. Calculate the volume of the products if 2.25 g of SO3 (l) is decomposed at 25.0 °C and 760.0 torr. Calculate the partial pressure of oxygen gas in this reaction. Calculate ∆H° for the reaction: 3SO2 (g) +...

For 2SO2(g)+O2(g)⇌2SO3(g), Kp=3.0×104 at 700 K. In a 2.00-L vessel the equilibrium mixture contains 1.13 g...

For 2SO2(g)+O2(g)⇌2SO3(g), Kp=3.0×104 at 700 K. In a 2.00-L vessel the equilibrium mixture contains 1.13 g of SO3 and 0.104 g of O2 How many grams of SO2 are in the vessel?

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