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: n² p+a (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? What are the units of b? The van der Waals equation of state. R stands for the gas constant and n for moles of gas. 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 X 0.0 3

0.17 moles of hydrogen gas and 0.33 moles of nitrogen gas are created from thereaction 2NH3 (g) → 3H2 (g) + N2 (g). The final total pressure in the reaction vessel is0.75 atm. Calculate the partial pressure of the hydrogen gas at the end of the reaction.Assume the number of moles of NH3 (g), left after the reaction occurs, is negligible.

The density of a gas is 1.43 g/Lg/L at a temperature of 23 ∘C∘C and a pressure of 0.789 atmatm. Calculate the molar mass of the gas.

Sometimes in lab we collect the gas formed by a chemical reaction over water (see sketch at right). This makes it easy to isolate and measure the amount of gas produced. 2 Suppose the CO₂ gas evolved by a certain chemical reaction taking place at 40.0 °C is collected over water, using an apparatus something like that in the sketch, and the final volume of gas in the collection tube is measured to be 51.0 mL. g x10 X 歐 Sketch of a gas-collection apparatus S collected gas Calculate the mass of CO₂ that is in the collection tube. Round your answer to 2 significant digits. You can make any normal and reasonable assumption about 2 the reaction conditions and the nature of the gases. water chemical reaction

For many purposes we can treat ammonia (NH,) as an ideal gas at temperatures above its boiling point of – 33. °C. Suppose the temperature of a sample of ammonia gas is lowered from 15.0 °C to – 14.0 °C, and at the same time the pressure is increased by 15.0%. increase x10 Does the volume of the sample increase, decrease, or stay the same? decrease ? stays the same If you said the volume increases or decreases, calculate the percentage change in the volume. Round your answer to the nearest percent.

A 9.00 L tank at 19.4 °C is filled with 2.75 g of chlorine pentafluoride gas and 13.9 g of sulfur hexafluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the partial pressure of each gas in the tank. Be sure your answers have the correct number of significant digits. chlorine pentafiuoride partial pressure: sulfur hexafluoride partial pressure: ? atm

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: The van der Waals equation of state. R stands for the gas constant and n for (V-nb)=nRT moles of gas. The parameters a and b must be determined for each gas from experimental data. Use the van der Waals eguation to answer the questions in the table below. 6. -2 What are the units of a? Ра m mol 몸 3 -1 What are the units of b? m ·mol For ethane the numerical value of a is 5.507 and the numerical value of b is 0.0651. | atm Use the van der Waals equation to calculate the pressure of a sample of ethane at 75.0 °C with a molar volume of 4,10 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. atm

A container holds a mixture of gases with the following partial pressures: PO₂ = 40.3 kPa, PCO₂ = 0.89 kPa, PN₂ = 180.3 kPa, and Ptotal = 222.8 kPa. Calculate the pressure of the other gases as described by Dalton's law of partial pressures.

A sample of gas contains 0.1100 mol of CH4 (9) and 0.1100 mol of H₂O(g) and occupies a volume of 13.1 L. The following reaction takes place: CH4 (9) + H₂O(g) → 3H₂(g) + CO(g) Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant. Volume =

A student obtained a mass of 0.266 g CO2 during his experiment. The atmospheric pressure was 751.6 mmHg and the laboratory temperature was 24.1 °C. The flask used in the experiment had a volume of 146.5 mL. Calculate the molar mass of CO2 from the data. Hint: You cannot use the molar mass of CO2 in your calculation since this is what you are looking for... You need to used the ideal gas law to determine the number of moles of CO2, then do the ratio of grams of CO2 over moles of CO2 to determine the experimental molar mass of CO2.