A mixture of CH4(g) at 0.500 atm and O2(g) at 0.750 atm is present in a 3.00-L container at 28°C. The mixture is ignited by a spark and reacts according to the equation provided below. What is the total pressure in the container, now at 44°C, after the reaction is complete? The vapor pressure of water at 44°C is 68.26 mmHg.
The partial pressure of CH4(g) is 0.185 atm and that of O2(g) is 0.300 atm in a mixture of the two gases. a) What is the mole fraction of each gas in the mixture? b) If the mixture occupies a volume of 11.5 L at 65 degress C,
A bearthing mixture used by deep-sea divers contains helium, oxygen, and carbon dioxide. What is the partial pressure of oxygen at 1.2 atm if PHe = 0.98 atm and PCO2 = 0.04 atm? a) 1.02 atm b) 0.12 atm c) 0.94 atm d) 0.18 atm
Consider the reaction: SO2 (g) + NO2 (g) ==> SO3 (g) + NO (g) At T = 1000 K, where the reaction is exothermic with an equilibrium constant K = 9.00 The reaction vessel is charged initially with all four gases, each at a pressure
A 10.00g sample of a mixture of CH4 and C2H4react with O2 at 25C and 1 atm to produce CO2 and water. If the reaction produces 520kJ of heat what is the mass percent of CH4 in the mixture? I don't want the answer just how to o
A 10.0 gram sample of a mixture of CH4 and C2H4 reacts with oxygen at 25°C and 1 atm to product carbon dioxide gas and liquid water. If the reaction produces 520 kJ of heat, what is the mass percentage of CH4 in the mixture?
At 750°C, the Kp for the reaction 2 CO + O2➞ 2 CO2 is 2.72 x 10^11. ( 2.72 times ten to the eleventh) At that temperature, CO and O2 are added to a constant volume vessel. The initial pressure of the CO is 2.00 atm, and that of