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

a) What is the partial pressure of CO₂ at 468.2 K in a 25.0 L fuel combustion vessel if it contains 75.6 grams CO₂, 82.1 g H₂O, and 7.30 mol vaporized, yet uncombusted fuel? b) What is the molar mass of an unknown gas with a density of 4.35 g/L at 1.00 atm and 25.0 °C? c) How many moles of chlorine gas at 120. °C and 33.3 atm would occupy a vessel of 40.0 L? d) What is the pressure in a 5.00 L tank with 9.15 moles of oxygen at 39.3 °C?

When limestone (solid CaCO3) is heated, it decomposes into lime (solid CaO) and carbon dioxide gas. This is an extremely useful industrial process of great antiquity, because powdered lime mixed with water is the basis for mortar and concrete - the lime absorbs CO₂ from the air and turns back into hard, durable limestone. Suppose some calcium carbonate is sealed into a limekiln of volume 550. L and heated to 910.0 °C. When the amount of CaCO3 has stopped changing, it is found that 567. g have disappeared. P Calculate the pressure equilibrium constant K, this experiment suggests for the equilibrium between CaCO3 and CaO at 910.0 °C. Round your answer to 2 significant digits. Note for advanced students: it's possible there was some error in this experiment, and the value it suggests for K does not match the accepted value. K-0 P

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