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3. Determine the equilibrium concentrations of all the reactants and products...
The initial concentrations or pressures of reactants and products are given for each of the following...
The initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and determine the direction in which each system will proceed to reach equilibrium. 2NH3(g)⇌N2(g)+3H2(g)Kc=17; [NH3] = 0.20 M, [N2] = 1.00 M, [H2] = 1.00 M (b) 2NH3(g)⇌N2(g)+3H2(g)KP=6.8×104; NH3 = 3.0 atm, N2 = 2.0 atm, H2 = 1.0 atm (c) 2SO3(g)⇌2SO2(g)+O2(g)Kc=0.230; [SO3] = 0.00 M, [SO2] = 1.00 M, [O2] = 1.00 M (d) 2SO3(g)⇌2SO2(g)+O2(g)KP=16.5; SO3 = 1.00...
9. Find the equilibrium concentrations for all reactants and products in the following equilibrium reaction. The...
9. Find the equilibrium concentrations for all reactants and products in the following equilibrium reaction. The initial concentration of the N2 is 0.78M and the initial concentration of O2 is 0.21M. There is no product initially. The equilibrium constant is K = 2.36 x 10-5. If you make any assumptions you are required to prove that they were valid! N2 + O2 yield 2 NO The equilibrium concentration of the N2 is __________________________ The equilibrium concentration of the O2 is...
3a. Determine the equilibrium pressures of all the reactants and products for the equilibrium described below...
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?...
A chemical reaction has reached equilibrium when A) the concentrations of reactants and products are equal. B) all...
A chemical reaction has reached equilibrium when A) the concentrations of reactants and products are equal. B) all reactants have been converted to products. all products have been removed from the reaction mixture. D) the catalyst has been used up. E) the rate of the forward reaction equals the rate of the reverse reaction. 6) An equilibrium in which all the components are gases is a A) heterogeneous equilibrium. D) homogeneous B) liquid C) catalytic E) reversible 7) The equilibrium...
What is the final concentration of D at equilibrium if the initial concentrations are [A] =...
What is the final concentration of D at equilibrium if the initial concentrations are [A] = 1.00 M and [B] = 2.00 M ?The reversible chemical reaction A+B⇌C+D has the following equilibrium constant: Kc=[C][D][A][B]=5.3 Gaseous hydrogen iodide is placed in a closed container at 425∘C, where it partially decomposes to hydrogen and iodine: 2HI(g)⇌H2(g)+I2(g) At equilibrium it is found that [HI]= 3.55×10−3M, [H2]= 4.82×10−4M , and [I2]= 4.82×10−4M. What is the value of Kc at this temperature? b The reversible...
The initial concentrations or pressures of reactants and products are given for each of the following...
The initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and determine the direction in which each system will proceed to reach equilibrium. (d) 2SO3 (g) ⇌ 2SO2 (g) + O2 (g) KP = 16.5; initial pressures: SO3 = 1.00 atm, SO2 = 1.00 atm, O2 = 1.00 atm (e) 2NO(g) + Cl2 (g) ⇌ 2NOCl(g) Kc = 4.6 × 104 ; [NO] = 1.00 M, [Cl2] = 1.00...
Lab Exercise #2: Equilibria Problems 1.2S02e) 22S03(e) at 1500 K: If the equilibrium concentrations are [SO2]...
Lab Exercise #2: Equilibria Problems 1.2S02e) 22S03(e) at 1500 K: If the equilibrium concentrations are [SO2] = 0.424 [ 2. We place 10.0 moles of N20 into a 2.00 L flask at 300 K. At equilibrium 2.20 moles remain. O2]-0.212 [SO3] = 0.076, find the Kc Given the following reaction, what is the Kc and the concentrations of N2 and O2? 3. Indicate whether the reaction will proceed right or left, and which concentrations will decrease or increase: 2HI(g) 근...
3. a) Write the equilibrium equation for the following reaction N2(g) + 3 H2(g) <-> 2...
3. a) Write the equilibrium equation for the following reaction N2(g) + 3 H2(g) <-> 2 NH3(g) b) An equilibrium mixture at 500 K has the following concentrations: [N2] = 3.0 x 10-2 M [H2] = 3.7 x 10-2 M [NH3] = 1.6 x 10-2 M, calculate the equilibrium constant, Kc c) Calculate the Kp for this reaction d) Is the equilibrium mixture mostly reactants or products? e) Does this reaction go to nearly 100% completion? Explain f) If Qc...
reactants or products. 10. Determine the concentration (M) of H2 gas in an equilibrium mixture that...
reactants or products. 10. Determine the concentration (M) of H2 gas in an equilibrium mixture that contains 7.5 g of CO and 10.0 g of CH3OH at 25oC. The volume of the container is 2.5L. Kc = 7.5 at 25oC CO(g) + 2 H2(g) ⇄ CH3OH(g)
1. The initial concentrations or pressures of reactants and products are given for each of the...
1. The initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and use it to determine the direction in which each system will proceed to reach equilibrium. Write "R" if the reactions shifts to the right towards products or "L" if it shifts left towards reactants. A. {NO} = 1.00 M, {Cl2} = 1.00 M, {NOCl} = 0.00 M; K = 4.6 x 104 2NO(g)+Cl2(g)<->2NOCl(g) B. {SO3} = 2.00...
A chemical reaction has reached equilibrium when A) the concentrations of reactants and products are equal. B) all reactants have been converted to products. all products have been removed from the reaction mixture. D) the catalyst has been used up. E) the rate of the forward reaction equals the rate of the reverse reaction. 6) An equilibrium in which all the components are gases is a A) heterogeneous equilibrium. D) homogeneous B) liquid C) catalytic E) reversible 7) The equilibrium...
Lab Exercise #2: Equilibria Problems 1.2S02e) 22S03(e) at 1500 K: If the equilibrium concentrations are [SO2] = 0.424 [ 2. We place 10.0 moles of N20 into a 2.00 L flask at 300 K. At equilibrium 2.20 moles remain. O2]-0.212 [SO3] = 0.076, find the Kc Given the following reaction, what is the Kc and the concentrations of N2 and O2? 3. Indicate whether the reaction will proceed right or left, and which concentrations will decrease or increase: 2HI(g) 근...
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