0.200 moles N2O4 were placed in a 2.00-L container, and at certain temperature the equilibrium set up with N2O4 measured at 0.0090 M:
N2O4(g) 2 NO2(g)
(a) Calculate the amount (in grams) of NO2 at equilibrium.
(b) Calculate the percent of the initial N2O4 dissociated into nitrogen dioxide.
(c) Determine Kc for the above rxn at that temperature. (Use ICE table)
d) If after the equilibrium set up, the system was compressed to one half of its initial volume, where will the equilibrium shift?
LEFT RIGHT NO CHANGE NOT ENOUGH INFORMATION
(e) If the volume has not changed, but the partial pressure of argon was increased twice, how would that affect equilibrium shift?
LEFT RIGHT NO CHANGE NOT ENOUGH INFORMATION
(f) Calculate the Kp value for this rxn.
0.200 moles N2O4 were placed in a 2.00-L container, and at certain temperature the equilibrium set...
Nitrogen dioxide dimerizes according to the following reaction: 2NO2(g)⇌N2O4(g) Kp=6.7at298K A 2.35-L container contains 0.057 mol of NO2 and 0.084 molof N2O4at298K. Calculate Kc for the reaction. Express the equilibrium constant with respect to concentration to three significant figures. Calculate Q for the reaction. Express the reaction quotient to three significant figures.
At a particular temperature, Kp = 0.260 for the reaction N2O4 ---> <--- 2NO2 1. A flask containing only N2O4(g) at an initial pressure of 4.20 atm is allowed to reach equilibrium. Calculate the total pressure in this flask at equilibrium. 2. With no change in the amount of material in the flask, the volume of the container in question is decreased to 0.400 times the original volume. Assuming constant temperature, calculate the (new) total pressure, at equilibrium.
At a particular temperature, Kp-0.39 for the reaction below. N204(g) 2 NO2(g) (a) A flask containing only N204 at an initial pressure of 4.8 atm is allowed to reach equilibrium. Calculate the equilibrium partial pressures of the gases. N2O4 NO2 atm (b) A flask containing only NO2 at an initial pressure of 9.6 atm is allowed to reach equilibrium. Calculate the equilibrium partial pressures of the gases. No2 (e) From your answers to parts (e) and (b), does it matter...
At a certain temperature, 0.680 mol of SO3 is placed in a 2.00-L container. At equilibrium, 0.120 mol of O2 is present. Calculate Kc.
1. The following gas phase equilibrium is established in a 2.0 L container: 2 C120 (g) 2 Cl2 (g) + O2(g) AH = - 161 kJ/mole State the direction the equilibrium will shift when the following changes (stresses) are made. Shift (right, left, or no shift) a) Increase [Cl20] b) Increase partial pressure of 02 c) Decrease the concentration of Cl2 d) Decrease the volume of the container to 1.0L e) Increase the temperature (no change in P) f) Add...
At a certain temperature, 0.620 mol of SO3 is placed in a 4.00-L container. At equilibrium, 0.100 mol of O2 is present. Calculate Kc. 2SO3 (g) ----> 2SO2(g) + O2(g) Kc =?
At a certain temperature, 0.720 mol SO, is placed in a 2.00 L container. 2 S03 (g) = 2 802(g) + O2(g) At equilibrium, 0.140 mol O, is present. Calculate Kc. Kc = .02117
At a certain temperature, 0.720 mol of SO3 is placed in a 2.00-L container. 2SO3(g) <=> 2SO2(g) + O2(g) At equilibrium, 0.100 mol of O2 is present. Calculate Kc
1. 1.75 moles of H202 were placed in a 2.50 L reaction chamber at 307°C. After equilibrium was reached, 1.20 moles of H202 remained. Calculate the equilibrium constant, Kc, for the reaction. 2. Phosgene, COCl,, a poisonous gas, decomposes according to the equation COC2(g) CO(g)+ Cl2(g) Calculate Kp for this reaction if Kc- 0.083 at 900°C. K K.(PT) 3. Calculate Kc for the reaction 2HI(g) H2(g) +12(g) given that the concentrations of each species at equilibrium are as follows: [HI...
36) At a certain temperature a reaction has K = 2.06 x 101. If all four gases have an initial concentration of 0.800M, what are the equilibrium concentrations? x = change in concentration. Choose all the correct answers. SO3 (g) + NO (g) <--> SO2 (g) + NO2 (g) (Select 6)(6pts) O [SO3) = [NO] = 1.101 M x=0.454 O Q = 1.0 [SO2] = [NO2] = 0.499 M OK=[SO3][NOJ/ [S02] - [NO2] [SO3] = [NO) = 0.499 M O...