A gas mixture contains 4.5 mol Br, and 33.1 mol F,. (a) Compute the mole fraction of Br, in the mixture. (b) The mixture is heated above 150°C and starts to react to give BrFs: Br2(g) + 5 F2(g) –→ 2 BrF;(g) At a certain point in the reaction, 2.2 mol BrF5 is present. Determine the mole fraction of Br2 in the mixture at that point.

A gas mixture contains 4.5 mol Br, and 33.1 mol F,. (a) Compute the mole fraction of Br, in the mixture. (b) The mixture is heated above 150°C and starts to react to give BrFs: Br2(g) + 5 F2(g) –→ 2 BrF;(g) At a certain point in the reaction, 2.2 mol BrF5 is present. Determine the mole fraction of Br2 in the mixture at that point.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

1. Calculate the volume of carbon dioxide adjusted to 25 °C and 1 atm, that plants need to make 1.00 g glucose, CóH12O6, by photosynthesis in the reaction 6CO2(g) + 6H20(I) C6H1206(s) + 602 (g).
1.25 L container holds a stoichiometric mixture* of ethene (CaH4), ethane (CaH6) and oxygen at a total pressure of 1.55 atm and a temperature of 24.5 °C. The mixture is ignited and completely combusts to form carbon dioxide and water. The water is removed from the vessel, leaving only carbon dioxide at a total pressure of 0.926 am at the same conditions. What is the mole fraction of oxygen in the original mixture?
A 0.210 g sample of a metal, M, reacts completely with sulfuric acid according to the reaction M(s)+H2SO4(aq)⟶MSO4(aq)+H2(g) A volume of 219 mL of hydrogen gas is collected over water; the water level in the collecting vessel is the same as the outside level. Atmospheric pressure is 1.0079 bar and the temperature is 25 °C. The vapor pressure of water at 25 °C is 0.03167 bar. Calculate the molar mass of the metal.
A student experimentally determines the gas law constant, R, by reacting a small piece of magnesium with excess hydrochloric acid and then collecting the hydrogen gas over water in a eudiometer. Based L-atm on experimentally collected data, the student calculates R to equal 0.0832 mol·K L-atm Ideal gas law constant from literature: 0.08206 mol·K (a) Determine the percent error for the student's R-value. Percent error = % (b) For the statements below, identify the possible source(s) of error for this student's trial. The student notices a large air bubble in the eudiometer after collecting the hydrogen gas, but does not dislodge it. The student does not clean the zinc metal with sand paper. The student does not equilibrate the water levels within the eudiometer and the beaker at the end of the reaction. The water level in the eudiometer is 1-inch above the water level in the beaker. The student uses the barometric pressure for the lab to calculate R.
- Exhaust gas from an automobile contains air and 10^-5 mole fractions of COin air at 25 degC and 1.2 atm. Express this concentration as a mass concentration (kg/m3).
A researcher put 0.640 mol PCl3 and 0.768 mol Cl2 into a 2.80 L vessel at a given temperature to produce phosphorus pentachloride, PCI5 : PCI3 (9) + Cl2 (9) =PCl; (g) What will be the composition of this gaseous mixture at equilibrium? K. = 25.6 at the temperature of this experiment. [PCI3] = M [Cl2] M [PCI5] =| M
Please answer it correctly
A mixture consiting of 1.000 mol H2O(g) and 1.000 mol CO(g) is placed ina reaction vessel of volume 10.00 L at 800. K. At equilibrium, 0.665 mol CO2(g) is present as a result of the reaction CO (g) + H2O (g)⇋ CO2(g)+H2(g). What are the value of KC at 800. K?