A 3 L container is filled with 12 moles of N2 at -140.6 °C. Calculate the...

A 3 L container is filled with 12 moles of N₂ at -140.6 °C. Calculate the pressure using ideal gas equation, van der Waals equation, SRK equation, virial equation, and the compressibility factor chart correlation.

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Amanda K answered 7 months ago

A container is filled to the brim with 1.4 L of mercury at 20°C. As the...

A container is filled to the brim with 1.4 L of mercury at 20°C. As the temperature of the container and mercury is increased to 51°C, a total of 7.6 mL of mercury spill over the brim of the container. Determine the linear expansion coefficient of the material that makes up the container. The coefficient of volume expansion of mercury is 1.8☓10-4 (°C)-1.

5.00 moles of N2 and 8.00 moles of H2 are placed in an empty container, the...

5.00 moles of N2 and 8.00 moles of H2 are placed in an empty container, the container is heated to 887 degrees Celsius, and a catalyst is added that catalyzes the rxn. of these gases to form NH3 as the only product. At equilibrium 1.00 mole of NH3 is found to be present. Find number of moles N2 and moles H2 present at equilibrium. * I think that the concentrations of the reactants changes by 1 mole but I'm not...

A container is filled to the brim with 1.5 L of mercury at 20

an elastic container filled with an ideal gas occupies 148 L volume at 85 degree c...

an elastic container filled with an ideal gas occupies 148 L volume at 85 degree c . what would the volumevbe at 15 degree c?

One mole of N2 and 3 moles of H2 are placed in a flask at 397°C....

One mole of N2 and 3 moles of H2 are placed in a flask at 397°C. Calculate the total pressure of the system at equilibrium if the mole fraction of NH3 is found to be 0.258. The KP for the reaction is 4.31 × 10^-4

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?

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?

A 2.50 L container is filled with gaseous H2S at 13.0ºC and a pressure of 169.1...

A 2.50 L container is filled with gaseous H2S at 13.0ºC and a pressure of 169.1 torr. Then 200.0 mL of water is added to the container (without allowing any of the H2S to escape). A small amount of H2S dissolves in the water. When the system has reached equilibrium, the gas pressure in the container is 155.9 torr and the temperature is still 13.0ºC. The vapor pressure of water at this temperature is 11.2 torr. What is the molar...

0.924 moles of A (g) is placed in a 1.00 L container at 700 degrees Celsiusand...

0.924 moles of A (g) is placed in a 1.00 L container at 700 degrees Celsiusand a reaction occured. 38.8% of the gas A dissociated when equilibrium was established. 3 A (g) ⇌ 5 B (g) + 2 C (g). What is the value of the equilibrium constant, K, at this temperature? (Answer: K = 0.0241) **PLEASE SHOW WORK. THANKS**

Consider three 0.03 m^3 tanks filled with N2, Air and He (tank A, B and C...

Consider three 0.03 m^3 tanks filled with N2, Air and He (tank A, B and C respectively). Each tank is filled with a pressure of 400 kPa at room temperature, 298 K. Determine the mass of gas contained in each tank. Also determine the number of moles of gas in each tank.

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