A sample of oxygen is collected over water at 24°C and 757 mm Hg in a 125-mL flask. The vapor pressure of water at 24°C is 22.4 mm Hg. The partial pressure is 734.6 mmHg. There are 4.96x10^-3 moles of dry gas collected. If 0.0205g of N2(g) are added to the flask at the same temperature, the partial pressure of nitrogen in the flask is 108.7 mmHg. What is the total pressure in the flask after nitrogen is added?

If 75.0 grams of carbonic acid are sealed in a 2.00 L soda bottle at room temperature (298.15 K) and decompose completely via the equation below, what would be the final pressure of carbon dioxide (in atm) assuming it had the full 2.00 L in which to expand? H¿CO3(aq) → H20 (1) + CO2(g)

Consider the following situation:  You have a 50 L tank of compressed air at 15 atm and 100 ºC.  You then pass the compressed air through a "titanium getter" which contains fragments of hot titanium metal.  The purpose of the "getter" is to remove oxygen gas from the sample as Ti reacts with oxygen to form solid TiO2 (known as titania).  Once the purified air is passed through the getter is it cooled back down to  100 ºC and fills another 50 L storage tank.  If air typically contains about 20% oxygen, what could the pressure in the storage tank be?     Question 2 options:   A)  12 atm   B)  15 atm   C)  18 atm   D)  24 atm

For many purposes we can treat ammonia (NH3) a as an ideal gas at temperatures above its boiling point of -33. °C. 3 Suppose the pressure on a 1.0 m sample of ammonia gas at -2.00°C is reduced to one-third its initial value. Is it possible to change the temperature of the ammonia at the same time such that the volume of the gas doesn't change? If you answered yes, calculate the new temperature of the gas. Round your answer to the nearest °C. yes no °C x10 S