A sample of 3.00 g of SO21g2 originally in a 5.00-L vessel at21 °C is transferred to a 10.0-L vessel at 26 °C. A sample of2.35 g of N21g2 originally in a 2.50-L vessel at 20 °C is transferredto this same 10.0-L vessel. (a) What is the partialpressure of SO21g2 in the larger container? (b) What is thepartial pressure of N21g2 in this vessel? (c) What is the totalpressure in the vessel?

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.

1. Which diagrams showing relationships between pressure, volume, and temperature below is/are incorrect for ideal gases? A B C KKKK V P T/P D PV

For many purposes we can treat methane (CH,) as an ideal gas at temperatures above its boiling point of –161. °C. Suppose the temperature of a sample of methane gas is raised from 50.0 °C to 98.0 °C, and at the same time the pressure is decreased by 10.0%. O increase x10 Does the volume of the sample increase, decrease, or stay the same? O decrease O 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. |%

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.

A sample of 5.00 mL of diethylether (C2H5OC2H5,density = 0.7134 g/mL) is introduced into a 6.00-L vesselthat already contains a mixture of N2 and O2, whose partialpressures are PN2 = 0.751 atm and PO2 = 0.208 atm. The temperatureis held at 35.0 °C, and the diethylether totally evaporates.(a) Calculate the partial pressure of the diethylether.(b) Calculate the total pressure in the container.

A gas cylinder contains the following mixture of gases: 16 g SO2, 16 g CH4 and 20 g Ar. Which gas exerts the largest partial pressure in the container

Hydrogen gas can be formed by the reaction of methane with water according to the following reaction:  CH4(g) + H2O(g) --> CO(g) +3H2(g) In a particular sample, 25.5 L of methane gas (measured at 0.963 atm and 298 K) is mixed with 22.8 L of water vapor (measured at 0.924 atm and 398 K). The reaction generates 26.2 L of di-hydrogen gas at STP. What is the percent yield of the reaction??

A syringe contains 589 mL of CO at 325 K and 1.2 atm pressure. A second syringe contains 473 mL of N2 at 298 K and 2.6 atm. What is the final pressure if the contents of these two syringes are injected into a 1.00 L container at 0.00 ∘C?

A homeowner uses 4.00x10³ m³ of natural gas in a year to heat a home. Assume the gas is CH4 and that it behaves as a perfect gas. If the pressure is 1.00 atm and the temperature is 20.0°C, what is the mass of the gas used?