A 4.96 g sample of toluene (formula C7H8), is mixed with 17.05 atm of O2 in a 1.75 L combustion chamber at 134.42 °C. The combustion reaction to CO2 and H20 is initiated and the vessel is cooled back to 134.42 °C. Report all answers to two decimal places in standard notation (i.e. 1.23 atm). 1. What is PcO2 (in atm) in the combustion chamber assuming the reaction goes to completion? Assume all water is water vapour and that the volume of the system does not change.

Background: Many metals react with hydrochloric acid to produce hydrogen gas and metal ions. In this Lab you will use Magnesium:    Mg(s)  + 2 H+(aq)  →    H2(g)  +   Mg2+(aq)    The moles of hydrogen gas produced can be determined using the Ideal Gas equation, PV = nRT.    Useful Information Pressure of water vapor at 18.8 °C = 16.3 torr   P(gases in buret) = P(hydrogen gas) + P(water vapor)   PV= nRT  where P is in atm, V is in L, and T is in K                                     TK = Tºc + 273    l.0 atm = 760 tor   R = 0.082 L atm /K mol                        Data   Volume of water added to the 50 mL buret that has uncalibrated bottom 1.0     mL         Buret reading after addition of 1.00 mL water  49.50 mL Mass of metal sample  0.038 g Temperature of water (and thus temperature of gases).  18.8 °C Buret reading of gases  36.9 mL Barometric pressure  760 torr   QUESTION   What is the partial pressure of water vapor at 18.8 °C? (1…

Determine the pressure of 2.581 moles of an ideal gas to THE WHOLE NUMBER in atm that has a volume of 395.0 mL at 292.2 K. R= 0.0821 Latm/(mol K)

Use the ideal gas law to verify the triple product rule.

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The human body burns glucose (C6H12O6) for energy according to this chemical reaction: C6H12O6+6O2→ 6CO2+6H2O The products of the reaction are carbon dioxide CO2 and water H2O Interestingly, all of the carbon dioxide and much of the water exits the body through the lungs: on every breath, the average person exhales 500.mL of air, which is typically enriched to 4% CO2 and 5% water vapor by volume. In short, when a person loses weight by dieting, the weight that is lost actually departs his body as a gas, every time he exhales. Each kilogram of body fat lost requires exhaling about 2.9kg of carbon dioxide. Calculate how many breaths it takes an average person to "exhale" 0.50kg  of fat. Round your answer to the nearest thousand. You'll need to know that the density of CO2 is 2.0 kg/m^3 .

For the following reaction: C3H8(g) + 3CO₂(g) + 4H₂O(1) 502(g) The change in gaseous moles, An = To maximize the product yield, the volume of the container should ◆ , so that the pressure will be (> →

Ammonia is among the top ten synthesized compounds. Its many uses include the manufacture of ammonium nitrate and other fertilizers. Ammonia decomposes at high temperatures. In an experiment to explore this behavior, 2.00 moles of gaseous NH3 are sealed in a rigid 1-liter vessel. The vessel is heated at 800 K and some of the NH3 decomposes in the following reaction: 2NH3(g) <--> N2(g)+3H2(g) The system eventually reaches equilibrium and is found to contain 1.74 mole of NH3. What is the value of KC for the decomposition reaction at 800K? What is the value of KP for the decomposition reaction at 800 K?

At 25 °C and 765.6 torr, a sample that is a gaseous compound containing carbon, hydrogen, and oxygen occupies a volume of 0.582 L. A mass of 1.103 g of this sample was burned in a bomb calorimeter, producing 1.294 g of liquid water and 2.108 g of gaseous carbon dioxide. The heat produced from the combustion raised the temperate of the calorimeter from 25 °C to 31.94 °C. a.) What is the percent elemental composition by mass of the unknown sample. b.) Determine the empirical formula of the sample.

What is the Qc for the following reaction, if a mixture contains gases with the following concentrations: CH4, 26 M; H2O, 24 M; CO, 26 M; H2 15 M, at a temperature of 760 0C? CH4(g) + H2O(g) CO(g) + 3H2(g)