The flame produced by the burner of a gas (propane) grill is a pale blue color when enough air mixes with the propane (C3H8) to burn it completely. For every gram of propane that flows through the burner, what volume of air is needed to burn it completely? Assume that the temperature of the burner is 205.0°C, the pressure is 1.25 atm, and the mole fraction of O2 in air is 0.210.

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 74.0 °C to 57.0 °C, and at the same time the pressure is decreased by 15.0%. increase ]x10 ol Does the volume of the sample increase, decrease, or stay the same? decrease A 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. O O OD

A gaseous mixture contains 3.23 g of chloroform CHCl3 and 1.22 grams of methane CH4 . Assuming that both compounds are maintained as gases, determine the partial pressure of each component and the pressure exerted by the non-reacting gas mixture inside the 50.0 mL container at 275 °C.

A sample contianing 8.12g of solid CO2 is put in an empty sealed 5.4L container at a temperature of 250.1K. When all the solid CO2 becomes gas, what will be the pressure in the container? Use 0.08206 · L· atm · K . mol¯ for your gas constant.

The pressure of a sample of argon gas was increased from 1.81 atm1.81 atm to 6.65 atm6.65 atm at constant temperature. If the final volume of the argon sample was 18.2 L,18.2 L, what was the initial volume of the argon sample? Assume ideal behavior.

A piece of sodium metal reacts completely with water as follows: 2Na(s) + 2H,0(1) –→ 2NAOH(aq) + H2(g) The hydrogen gas generated is collected over water at 27.0°C. The volume of the gas is 179 mL measured at 0.983 atm. Calculate the number of grams of sodium used in the reaction. (The vapor pressure of water at 27.0°C = 0.0352 atm.) g

When solid calcium carbonate is reacted with aqueous hydrochloric acid, the products of the reaction include aqueous calcium chloride, liquid water, and gaseous carbon dioxide. Calculate the volume of CO₂ gas (in L) collected over water at 25.0 °C when 27.3 g of calcium carbonate is added to excess hydrochloric acid if the total pressure is 911 mm Hg. The vapor pressure of water at 25.0 °C is 23.8 mm Hg.

A mixture of 8.0 g CH4 and 8.0 g Xe is placed in a container and the total pressure is found to be 0.44 atm. Determine the partial pressure of CH4.

Consider a gas mixture composed of 0.200 mol N2, 0.0800 mol O2, and 0.0200 mol Ar.  The total pressure exerted by this mixture at 25°C is 1.068 atm.  Determine the partial pressure (in atm) of N2 in this mixture.

Consider the reaction between 50.0 mL of liquid methanol (CH3OH; d=0.850g/mol) and 22.8 L of O2 at 27 degrees C and a pressure of 2 atm. The products of the reaction are CO2 (g) and H2O (g). Calculate the mass of water formed if reaction goes to completion.