A 2.99 L flask contains c6h6 at a pressure of 244 mm Hg and a temperature of 25 °C. Suppose o2 gas is added to the flask until c6h6 and o2 are in the correct stoichiometric ratio for the combustion reaction. At this point, what is the partial pressure of o2? Partial pressure = ___ mm Hg

For many purposes we can treat butane (C,H10) as an ideal gas at temperatures above its boiling point of -1. °C. Suppose the pressure on a 36.0 g sample of butane gas at 45.0°C is reduced to one-third its initial value. O yes Is it possible to change the temperature of the butane at the same time such that the volume of the gas doesn't change? O no If you answered yes, calculate the new temperature of the gas. Round your answer to the nearest °C.

2. If the excess salt is dissolved in water, it will reform carbamic acid. At 350K, carbamiC acid will decompose into NH3 (g) and CO2 (g). Assuming that the water vapor has no effect on the overall gas components or container volume, what is the final pressure in the container outlined in question 1 now? Question 1 for reference: A reaction of 5.35g of solid methyl lithium (CH3LI) reacts with 24.63g of solid carbamic acid (NH2COOH) at 200K to produce methane gas (CH4) and a dilithium carbamate salt (NHCO2Lİ2). If the completed reaction mixture heated to 35OK in a 2.6L container, what is the pressure in the container? The answer I got for this was 2.65 atm

Oxygen gas can be generated by heating potassium chlorate: heat 2KCI(s) + 30,(g) 2 KCIO, (s) 2KCI(s) + What volume of oxygen gas, collected by displacement of water and measured at 780.9 torr and 80.0 °C (vapor pressure of watergo.0 °C -355.63 torr), will be formed by the decomposition of 48.8 g of potassium chlorate? Be sure your answer has the correct number of significant figures. Note: Reference the Conversion factors for non-SI units and Fundamental constants tables for additional information.