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5. Carbonyl fluoride, COF2, can be prepared by the following reaction? CO2(8) + CF4(g) < +...
Carbonyl fluoride, COF2, is an important intermediate used in the production of fluorine-containing compounds. For instance, it is used to make the refrigerant carbon tetrafluoride, CF4 via the reaction 2COF2(g)⇌CO2(g)+CF4(g), Kc=8.90 If only COF2 is present initially at a concentration of 2.00 M, what concentration of COF2 remains at equilibrium? Express your answer with the appropriate units.
Tall- Carbonyl fluoride, COF2, is an important intermediate used in the production of fluorine-containing compounds. For instance, it is used to make the refrigerant carbon tetrafluoride, CF4 via the reaction 2COF2(9) = CO2(g) + CF4(9), K= 7.80 at 850 K If only COF2 is present initially at a pressure of 260 kPa, what is the partial pressure of COF2 at equilibrium? You can convert the units of pressure from kPa to bar, using the relation 1 kPa = 0.01 bar....
A. Carbonyl fluoride, COF2, is an important intermediate used in the production of fluorine-containing compounds. For instance, it is used to make the refrigerant carbon tetrafluoride, CF4 via the reaction 2COF2(g)⇌CO2(g)+CF4(g), Kc=7.80 If only COF2 is present initially at a concentration of 2.00 M, what concentration of COF2 remains at equilibrium? B. Consider the reaction CO(g)+NH3(g)⇌HCONH2(g), Kc=0.820 If a reaction vessel initially contains only CO and NH3 at concentrations of 1.00 M and 2.00 M, respectively, what will the concentration of...
Part A: Carbonyl fluoride, COF2, is an important intermediate used in the production of fluorine-containing compounds. For instance, it is used to make the refrigerant carbon tetrafluoride, CF4 via the reaction 2COF2(g)?CO2(g)+CF4(g), Kc=5.10 If only COF2 is present initially at a concentration of 2.00 M, what concentration of COF2 remains at equilibrium? Express your answer with the appropriate units. Part B: Consider the reaction CO(g)+NH3(g)?HCONH2(g), Kc=0.770 If a reaction vessel initially contains only CO and NH3 at concentrations of 1.00...
Part A Carbonyl fluoride, COF2, is an important intermediate used in the production of fluorine-containing compounds. For instance, it is used to make the refrigerant carbon tetrafluoride, CF4 via the reaction 2COF2(g)?CO2(g)+CF4(g), Kc=4.20 If only COF2 is present initially at a concentration of 2.00 M, what concentration of COF2 remains at equilibrium? Express your answer with the appropriate units. [COF2] = Part B Consider the reaction CO(g)+NH3(g)?HCONH2(g), Kc=0.820 If a reaction vessel initially contains only CO and NH3 at concentrations of 1.00...
3a. Determine the equilibrium pressures of all the reactants and products for the equilibrium described below if you start with an initial pressure of carbon dioxide and carbon tetrafluoride each at 0.750 atm with no COF2 present. You can assume that the temperature is constant at 1550K. (12 points) 2COF2(g) CF4(g) + CO2(g) KP = 0.168 at 1550K Initial pressures: PCO2 = PCF4 = 0.750 atm; PCOF2 = 0.000 atm 3b. What is the value of KC for this reaction?...
9. Consider the following reaction: inputted, <GO CaO(s) + CO2(g) - CaCO3(s); AG° = -130.9 kJ at 298 K At what partial pressure of CO2(g) will the reaction no longer be spontaneous at 298 K? (R- 0.0821 L.atm/(K.mol) = 8.31 J/(K.mol)) a. 1.59 x 108 atm b. 1.00 atm c. 6.28 x 10 atm d. 8.77 x 1022 atm e. 1.14 x 10-23 atm
84. Hydrogen can be extracted from natural gas according to the reaction: CH4(8) + CO2(g) = 2 CO(g) + 2 H2(g) Ky = 4.5 x 102 at 825 K An 85.0-L reaction container initially contains 22.3 kg of CH4 and 55.4 kg of CO2 at 825 K. Assuming ideal gas behavior, calcu- late the mass of H, (in g) present in the reaction mixture at equi- librium. What is the percent yield of the reaction under these conditions? CaO(s) :...
At 1000 K, Kp = 19.9 for the following reaction: Fe2O3(s)+3CO(g)⇌2Fe(s)+3CO2(g) What are the equilibrium partial pressures of CO and CO2 if CO is the only gas present initially, at a partial pressure of 0.982 atm ?
Using the following two reactions and their equilibrium constants: Cs) + CO2(g) +200 K= 2.4 X 10-9 COC12(e) < CO(g) + Cl2(g) K = 8.8 X 10-13 Calculate K for this reaction: C(s) + CO2(g) + 2C12(e) H2COC12(e)