Boyle's Law states that when a sample of gas is compressed at a constant temperature, the pressure P and volume V satisfy the equation PV = C, where C is a constant. Suppose that at a certain instant the volume is 600 cm3, the pressure is 120 kPa, and the pressure is increasing at a rate of 30 kPa/min. At what rate is the volume decreasing at this instant? cm3/min

A mixture of xenon and methane gases contains xenon at a partial pressure of 354 mm Hg and methane at a partial pressure of 380 mm Hg. What is the mole fraction of each gas in the mixture? хе Xxe XCH, =

I only need help with part b

A student has a 2.97 L bottle that contains a mixture of O2 , N2 , and CO2 with a total pressure of 4.70 bar at 298 K . She knows that the mixture contains 0.277 mol N2 and that the partial pressure of CO2 is 0.336 bar . Calculate the partial pressure of O2 .

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: 2 p+a (V-nb)=nRT The van der Waals equation of state. R stands for the gas constant and n for moles of gas. v? 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? For ammonia the numerical value of a is 4.169 and the numerical value of b is 0.0371. atm Use the van der Waals equation to calculate the pressure of a sample of ammonia at 195.0 °C with a molar volume of 4.12 L/mol. Round your answer to 3 significant digits. Use the Ideal Gas Law to calculate the pressure of the same sample under the same conditions. Round this answer to 3 significant digits also. || atm O

11. (a) In a 20.0 L steel container, we have only 77.7 g of CO2(g), 66.6 g of N2(g), and O2(g). The temperature is 25.0 ◦C and the total pressure is 8.88 atm. What mass of O2(g) do we have, and what is its partial pressure? The molar masses of C, N, and O are 12.01, 14.01, and 16.00 g/mol. (b)  The density of a sample of pure CH4(g) at a constant pressure of 1.00 atm is 0.666 g/L. What is the average speed, or root mean square speed, of the CH4(g) molecules in this sample? The molar masses of C and H are 12.01 and 1.01 g/mol.

The critical pressure, Pe, and the critical temperature, Te, of gas A are 3.040 × 10° Pa and 473 K, respectively. (i) Calculate the van der Waals constants, a and b, for this gas. (ii) Gas A obeys the van der Waals equation. Calculate the pressure exerted by one mole of gas A if the molar volume occupied by this gas is 2.75 L/mol at 298 K.

A 1.50-liter sample has a pressure of 138 kPa at 12°C. What temperature would this sample be if it expanded to 2.43 liters under a pressure of 236 kPa?