The van der Waals equation of state for a real gas is n?a P+ v2 - nb]= At what pressure will 1.00 mole of CH4 be in a 10.0 L container at 298 K assuming CH4 is a real gas. (van der Waals constants for CH4 are a = 2.253 L2 atm mol-2, b = 0.04278 L mol-1) 2.43 atm (А) B 0.440 atm 24.5 atm (D 2.51 atm E) 2.28 atm

I need help with part A and B

Answer part a and b

The fermentation of glucose (wine making) reaction is shown below. During this process 780 mL of CO2 gas was produced at 37 oC and 1.00 atm. (R= 0.0821 LatmK-1mol-1)                                   C6H12O6(s)  +     6O2(g)      à      6CO2 (g)     +    6H2O (l)   a. Calculate the number of moles of CO2 produced in the above reaction?   b.What is the final volume, in liters, of the CO2 gas when measured at 22 oC and 675 mm Hg. ( 1 atm = 760 mm Hg)

I only need help with part b

Use the van der Waals equation of state to calculate the pressure of 3.30 mol of HI at 483 K in a 4.60 L vessel. Van der Waals constants can be found in the van der Waals constants table. P = atm Use the ideal gas equation to calculate the pressure under the same conditions. P = atm Under these conditions, would you expect HI or CCl, to deviate more from ideal behavior? Why? CCl because it occupies a larger volume and it has smaller dispersion forces between molecules. HI because it occupies a smaller volume and it has smaller dispersion forces between molecules. HI because it occupies a larger volume and it has smaller dispersion forces between molecules. CCI, because it occupies a larger volume and it has greater dispersion forces between molecules. HI because it occupies a smaller volume and it has greater dispersion forces between molecules. CCI, because it occupies a smaller volume and it has greater dispersion forces between molecules.

An average gas fireplace uses about 200 gallons (760,000 cm3) of propane gas per year. Assume that the propane, C3H8, behaves as a perfect gas for the conditions of this problem, which are 1.00 atm and 22°C. What is the mass of gas used?

The van der Waals equation of state was designed (by Dutch physicist Johannes van der Waals) to predict the relationship between pressure p, volume V and temperature T for gases better than the Ideal Gas Law does: n (p+₁ +²2) (v- (V-nb)=nRT The parameters a and b must be determined for each gas from experimental data. Use the van der Waals equation to answer the questions in the table below. What are the units of a? The van der Waals equation of state. R stands for the gas constant and n for moles of gas. What are the units of b? For ethane the numerical value of a is 5.507 and the numerical value of b is 0.0651. Use the van der Waals equation to calculate the pressure of a sample of ethane at 105.0 °C with a molar volume of 5.27 L/mol. Round your answer to the correct number of significant digits. Use the Ideal Gas Law to calculate the pressure of the same sample under the same conditions. Round your answer to the correct number of significant digits. 0 0 atm atm x10 DO X ロ・ロ

Ammonia, NH3, may react with oxygen to form nitrogen gas and water. 4 NH₂(aq) + 30₂(g) →→→ 2N₂(g) + 6H₂O(1) If 3.95 g NH3 reacts with 5.93 g O₂ and produces 0.850 L. N₂ at 295 K and 1.00 bar, how many moles of N₂ can be produced by each reactant? It may be useful to consult the periodic table. NH₂: 0₂: Based on the theoretical yields, which reactant is limiting? NH,(aq) 0₂(g) What is the percent yield of the reaction? percent yield: mol N₂ mol N₂ 28