The combustion of propane is described by the chemical equation C3H8 (g) + 5O2(g) → 3CO₂(g) + 4H₂O(g) . If we have a partial pressure of 0.375 bar of propane as the reactant, what partial pressure of oxygen will we need to have a perfect amount to consume all of the propane with no unreacted propane or oxygen left over at the end of the reaction? 1.13 kPa 0.0750 bar 0 0.375 bar 1.88 bar

A student has a 2.97 L bottle that contains a mixture of O2 , N2 , and CO2 with a total pressure of 4.70 bar at 298 K . She knows that the mixture contains 0.277 mol N2 and that the partial pressure of CO2 is 0.336 bar . Calculate the partial pressure of O2 .

What would Qc be if the volume of the container decreased by a factor of 3.444 for the following reaction? CO(g) + 3 H2(g) → CH4(g) + H2O(g)   KC = 3.917 at 1200oC

A 2.61 gram sample of a solid mixture contains NaClO3 as well as unreactive material. When heated, only the NaClO3 in the mixture decomposes to produce 992 milliliters of O2 gas at 225◦C and 772 mmHg according to the unbalanced equation NaClO3(s) −→ NaCl(s) + O2(g). What is the percent by mass of NaClO3 in the mixture?

The chlorination of methane occurs in a number of steps that results in the formation of chloromethane and hydrogen chloride. The overall reaction is 2CH, (g) +3 Cl, () 2CH,CI(g) + 2 HCI(g) + 2CI (g) Suppose that a chemist combines 273 mL of methane and 689 mL of chlorine at STP in a 2.00 L flask. The flask is then allowed to stand at 298 K. If the reaction reaches 75.0% completion, what is the total pressure in the flask? Pictal = atm What is the partial pressure of CH,? Pon, = atm What is the partial pressure of Cl, ?

The ideal gas law, R, can be experimentally determined. Use the data provided below from the reaction of potassium chlorate decomposing to form oxygen gas and potassium chloride to experimentally determine the value of R in units of L•atm/mol•K. 2KClO3 (s) → 2KCl (s) + 3O2 (g) The evolved oxygen is collected over water. The relevant data from the experiment is summarized below. Mass of KClO3 used 0.0665 g Initial volume reading 46.0 mL Final volume reading 64.2 mL Temperature 22.0°C Total pressure 772.0 mm Hg A table of vapor pressures of water is also available: Temperature (°C) Vapor Pressure of Water (mm Hg) 21 18.7 22 19.8 23 21.1 24 22.4 25 23.8 What is the volume (in L) of O2 gas formed in the experiment?   What is the dry pressure (in mm Hg) of O2 gas in the experiment?   What is the dry pressure (in atm) of O2 gas in the experiment? What is the temperature (in K) for the experiment? How many moles of KClO3 were used in this…

A reaction between liquid reactants takes place at - 14.0 °C in a sealed, evacuated vessel with a measured volume of 40.0 L. Measurements show that the reaction produced 36. g of chlorine pentafluoride gas. Calculate the pressure of chlorine pentafluoride gas in the reaction vessel after the reaction. You may ignore the volume of the liquid reactants. Be sure your answer has the correct number of significant digits. pressure: |II atm

17 The total pressure is distinct from the individual partial pressures of a mixture. O True O False 身

BIOL 1603: Org & Evol - Google x A ALEKS - Katie Matthews - Grac x Content app.101edu.co → C esc 1 F1 A glass container was initially charged with 1.50 moles of a gas sample at 5.00 atm and 21.7 °C. Some of the gas was released as the temperature was increased to 33.1 °C, so the final pressure in the container was reduced to 1.50 atm. How many moles of the gas sample are present at the end? Q 2 F2 W # 3 80 E $ 4 F4 R % 675 뽀 F5 T 6 X Question 38 of 66 F6 Y Aktiv Chemistry & 7 F7 U * 00 8 DII F8 ( 1 9 X a Amazon.com: wireles F9 0 1 2 4 7 +/- 0 7 F10 5 8 P

A sample of Cl2 with a pressure of 1.84 atm and a volume of 290 mL is allowed to react with excess Br2 at 182 °C. Br2 (g) +Cl2 (g) --> 2BrCl (g) Calculate the pressure of the BrCl produced in the reaction if it is transferred to a 2.16-L flask and cooled to 32 °C