(a) F2(g) 2F(g) (b) 2CH4(8) C,H2(g) + 3H2(g)

For the reaction: 2 NO2 (g) + O2 (g) --> 2 NO3 (g) at 923 °C , Kc is 42.5. If 0.0500 moles of NO2 (g), 0.122 moles of O2 (g) and 0.300 moles of NO3 (g) are mixed in a 1.00 liter container at 923 °C, in what direction will the reaction proceed? (Show your calculation to prove that your answer is not a guess.)

Consider the following reaction where Kc = 55.6 at 698 K. H2(g) + I2(g)  ---->  2HI(g) A reaction mixture was found to contain 4.26×10-2 moles of H2(g), 4.04×10-2 moles of I2(g) and 0.270 moles of HI(g), in a 1.00 liter container. Is the reaction at equilibrium?If not, what direction must it run in order to reach equilibrium?The reaction quotient, Qc, equals _____   The reaction (fill in the blank) ____ A. must run in the forward direction to reach equilibrium.B. must run in the reverse direction to reach equilibrium.C. is at equilibrium.

5. Consider air (which consists of 79 mol% of N2 and 21 mol% of O2) at 300 K: (a) What is the self-collision rate of nitrogen molecules in number of collisions per m' per second? (b) What is the self-collision rate of oxygen molecules in number of collisions per m' per second? (c) What is the collision rate between oxygen and nitrogen molecules in number of collisions per m' per second? Hint: Use the hard-sphere model where all the collisions are effective. The diameters of oxygen molecules and nitrogen molecules are 3.61 Å and 3.75 Å, respectively. For self-collision scenarios, calculate reduced mass based on two molecules of the same size and mass and be mindful that the number of collisions is double counted.

Consider the following reaction where Kc 6.50x10-3 at 298 K. 2NOBr(g) 2NO(g) + Br2(g) A reaction mixture was found to contain 7.56×10-2 moles of NOBr(g), 2.06x10-2 moles of NO(g), and 3.67x10-2 moles of Br2(g), in a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Qc, equals The reaction A. must run in the forward direction to reach equilibrium. B. must run in the reverse direction to reach equilibrium. C. is at equilibrium.

Consider the reaction SO, Ch(g) S0, (g) + Ca(g) K-2.97 x 10 at 62s K In a reaction mbture at equilibrium, the partial pressure of SO, is 141 mbar and that of Cla ln 283 mbar Part A What is the partial pressure of SO, Cl,? Express your answer in bars to three significant figures. > View Available Hint(s) V AZ * O a ? bar P(SO,Cl) = Submit Besuest Answer Next>

Consider the following reaction where Ke- 7.00x10s at 673 K. NH4I(s)NHa(a) + HI(9) A reaction mixture was found to contain 5.24x102 moles of NH,I(s), 5.36x103 moles of NH3(g), and 8.37x103 moles of HI(g), in a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Qe equals The reaction A. must run in the forward direction to reach equilibrium. B. must run in the reverse direction to reach equilibrium. C. is at equilibrium.

As you are walking across your laboratory, you notice a 5.25 L flask containing a gaseous mixture of 0.0205 mole NO2 (9) and 0.750 mol N2O4 (q) at 25°C. 4 (g) Is this mixture at equilibrium? If not, will the reaction proceed towards forming more products, or more reactants? N2O4 4 (9) → 2NO2 (9) Ko = 4.61 x 103 at 25°C

6. Consider the following reaction: CO(g) + H2O(g) CO2(g) + H2(g) Ko = 0.58 at 1273 K* A sealed 4.00L vessel initially contains 1.00 mole CO2(g), 1.00 mole H2(g), 0.600 moles CO(g), and 0.600 moles of H2O(g). Calculate the moles of H2(g) present at equilibrium. The NG Reference: General Chemistry 8th Ed: Ebbing and Gammon: 2005 by Houghton Mifflin. New York. page 654, print 68

A methanol synthesis reaction will be run in a container with a moveable piston to allow for changes in volume. The gas phase reaction is illustrated below: CO(g) + 2H2(g) = CH3OH(g) At equilibrium, the reaction is run at 400K in a 10L flask; there are 3.09 moles of CO and 1.11 moles H₂ initially. At constant volume, 0.830 mol H2(g) is added to the reaction. Solve for the partial pressures of the gases in the container when the reaction returns to equilibrium. Really not sure how I should solve this problem, please help me out my showing step by step what I should do. Thanks :)