A sample of automobile exhaust gas is analyzed at an Ontario Drive Clean center. The gas contains 487.4 ppm CO2, 10.3 ppb NO, and 4.2 ppb CO. Calculate the partial pressures (in kPa) of these gases if the exhaust is emitted at 102.4 kPa pressure. What is the partial pressure of CO2? What is the partial pressure of NO? What is the partial pressure of CO?

The hydrocarbon naphthalene was frequently used in mothballs until recently, when it was discovered that human inhalation of naphthalene vapors can lead to hemolytic anemia. Naphthalene is 93.71% carbon by mass, and a 0.256-mole sample of naphthalene has a mass of 32.8 g. What is the molecular formula of naphthalene? This compound works as a pesticide in mothballs by. sublimation of the .solid so that it fumigates enclosed spaces with its vapors according to the equation Naphthalene(s)naphthalene(g)K=4.29106(at298K) If 3.00 g solid naphthalene is placed into an enclosed space with a volume of 5.00 L at 25C, what percentage of the naphthalene will have sublimed once equilibrium bas been established?

Nitroglycerin decomposes into four different gases when detonated: 4 C3H5(NO3)3() 6 N2(g) + O2(g) + 12 CO2(g) + 10 H2O(g) The detonation of a small quantity of nitroglycerin produces a total pressure of 4.2 atm at a temperature of 450 C. (a) What is the partial pressure of N2? (b) If the gases occupy a volume of 1.5 L, what mass of nitroglycerin was detonated?

93 The complete combustion of octane can be used as a model for the burning of gasoline: 2C8H18+25O216CO2+18H2O Assuming that this equation provides a reasonable model of the actual combustion process, what volume of air at 1.0 atm and 25°C must be taken into an engine to burn 1 gallon of gasoline? (The partial pressure of oxygen in air is 0.21 atm and the density of liquid octane is 0.70 g/mL.)

Xenon and fluorine will react to form binary compounds when a mixture of these two gases is heated to 400C in a nickel reaction vessel. A 100.0-mL nickel container is filled with xenon and fluorine, giving partial pressures of 1.24 atm and 10.10 atm, respectively, at a temperature of 25C. The reaction vessel is heated to 400C to cause a reaction to occur and then cooled to a temperature at which F2 is a gas and the xenon fluoride compound produced is a nonvolatile solid. The remaining F2 gas is transferred to another 100.0-mL nickel container, where the pressure of F2 at 25C is 7.62 atm. Assuming all of the xenon has reacted, what is the formula of the product?

What possible uses exist for the natural gas liquids that are removed from natural gas during its processing?

Solve correctly please, need all subparts.

Part 5. Dalton's Law of Partial Pressures A sample of Argon gas is placed in a 5.0L container at 298K. The measured pressure is 1.0 atm. If Xenon gas is added to the same container containing the Argon, and the volume and temperature due not change, the pressure increases to 1.5 atm. From this data calculate the moles of argon and xenon present in the flask and the mole fraction of each gas.

A clean, dry and open empty flask is being heated in a water bath. Under which conditions before or after heating does the flask contain more gas molecules? Explain. The flask in problem 1 is allowed to cool back to room temperature. Account for the volume occupied by the gas and the number of gas molecules when the gas is cooled to room temperature. Why is it necessary to immerse the flask both in hot and cold water for 5 minutes before taking the temperature? The water levels inside and outside the flask when it was submerged in cold bath must be equal before the flask is removed. Explain. Name the factors that contributed to the difference between the measured and the computed values of the horizontal displacement (R). Show that during the motion of a simple pendulum the work done by the tension on the string is zero. Show that when a body of mass m is dropped from a height h, the sum of its kinetic and potential energies is constant at any instant and is equal to mgh. How much…

Q/ Gaseous hydrogen sulfide and gaseous sulfur dioxide are combined in a 250. mL flask. The gas mixture is heated to 100. °C where they react according to the following equation. 2 H2S(g) + SO2(g) → 3 S(s) + 2 H2O(l) a) If H2S has a partial pressure of 2.00 atm, and that of SO2 is 1.50 atm, determine the maximum yield possible of sulfur, in grams. Show all work.  b) If you collected 0.55 grams of sulfur, what was your percent yield for the reaction? Show all work.