N2(g) + O2(g) equilibrium reaction arrow 2 NO(g); Kc = 5.6 ✕ 10−4 at 2098 K...
N2(g) + O2(g) equilibrium reaction arrow 2 NO(g); Kc = 5.6 ✕ 10−4 at 2098 K
(a) What is the value of Kc for the reaction 2 NO(g) equilibrium reaction arrow N2(g) + O2(g) at the same temperature?
(b) What is the value of Kc for the reaction 1/2 N2(g) + 1/2 O2(g) equilibrium reaction arrow NO(g) at the same temperature?
(c) Does the equilibrium in (a) favor the reactant or the products? reactant products
(d) Does the equilibrium in (b) favor the reactants or the product? reactants product
(e) Consider the original reaction. If pN2 = 0.310 atm, pO2 = 2.22 atm, and pNO = 0.134 atm, is the system at equilibrium? If not, will the system shift to the left or to the right in order to achieve equilibrium? The system is not at equilibrium; therefore, the system (shifts left/ Shifts right)
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N2(g) + O2(g) equilibrium reaction arrow 2 NO(g); Kc = 5.6 ✕
10−4 at 2098 K...
ΔH is positive for the equilibrium N2 (g) + O2 (g) ↔ 2 NO (g). If...
ΔH is positive for the equilibrium N2 (g) + O2 (g) ↔ 2 NO (g). If we lower the temperature, (A) the equilibrium shifts to the left (more N2 + O2 gases formed) (B) the equilibrium shifts to the right (more NO gas formed) (C) Equilibrium does not shift because there are the same number of molecules on left side as on the right (D) Equilibrium does not shift because temperature does not affect the reaction rates why?
The equilibrium constant, Kc, for the following reaction is 1.31×10-2 at 700 K. NH4I(s) (forward/reverse arrow)NH3(g)...
The equilibrium constant, Kc, for the following reaction is 1.31×10-2 at 700 K. NH4I(s) (forward/reverse arrow)NH3(g) + HI(g) 1. Calculate Kc at this temperature for the following reaction: NH3(g) + HI(g) (forward/reverse arrow)NH4I(s) Kc = 2. The equilibrium constant, Kc, for the following reaction is 2.03 at 677 K. 2NH3(g) (forward/reverse arrow)N2(g) + 3H2(g) Calculate Kc at this temperature for: N2(g) + 3H2(g) (forward/reverse arrow)2NH3(g) Kc =
Nitrogen and oxygen react at high temperatures. N2(g) + O2(g) equilibrium reaction arrow 2 NO(g) ΔH...
Nitrogen and oxygen react at high temperatures. N2(g) + O2(g) equilibrium reaction arrow 2 NO(g) ΔH = 182.6 kJ (a) Write the expression for the equilibrium constant (Kc) for this reversible reaction. (Concentration equilibrium expressions take the general form: Kc = [C]c / [A]a . [B]b. Subscripts and superscripts that include letters must be enclosed in braces {}.)
Part A N2(g)+3Br2(g)⇌2NBr3(g) K=[NBr3]2[N2][Br2]3 K=[N2][Br2]3[NBr3]2 K=[NBr3][N2][Br2] K=[NBr3]2[N2][Br2]3 Part B C(s)+O2(g)⇌CO2(g) K=[CO2][O2] K=[O2][CO2] K=[CO2][O2] K=[CO2][O2][C] When heated,...
Part A N2(g)+3Br2(g)⇌2NBr3(g) K=[NBr3]2[N2][Br2]3 K=[N2][Br2]3[NBr3]2 K=[NBr3][N2][Br2] K=[NBr3]2[N2][Br2]3 Part B C(s)+O2(g)⇌CO2(g) K=[CO2][O2] K=[O2][CO2] K=[CO2][O2] K=[CO2][O2][C] When heated, carbon reacts with water to produce carbon monoxide and hydrogen. C(s)+H2O(g)+heat⇌CO(g)+H2(g) Part C What effect does each of the following changes have on the equilibrium? Drag the appropriate stresses to their respective bins. add H2O, Add heat, lower temperature, remove CO Categories: Equilibrium shifts to products, Equilibrium shifts to reactants, Equilibrium doesn't shift
The reaction N2(g)+O2(g)⇌2NO(g) is carried out at a temperature at which Kc = 0.050. The reaction mixture...
The reaction N2(g)+O2(g)⇌2NO(g) is carried out at a temperature at which Kc = 0.050. The reaction mixture starts with only the product, [NO] = 0.0300 M , and no reactants. Part A Find the equilibrium concentrations of N2 at equilibrium. Express your answer to two significant figures and include the appropriate units. [N2] = Part B Find the equilibrium concentrations of O2 at equilibrium. Part C Find the equilibrium concentrations of NO at equilibrium. Express your answer to two significant figures...
1. The initial concentrations of reactants and products for this reaction are given below. N2(g) +...
1. The initial concentrations of reactants and products for this reaction are given below. N2(g) + O2(g) ⇄ 2NO(g) Calculate Q for this reaction. Answer this to one decimal place (e.g. 10.2) The initial concentration of N2 is 1.0 M The initial concentration of O2 is 1.0 M The initial concentration of NO is 2.5 M 2. The reaction below is not at equilibria and Q = 1.7. The equilibrium constant is K = 0.230. 2SO3(g) ⇌ 2SO2(g) + O2(g)...
The reaction N2(g) + O2(g) ⇄ 2 NO(g) contributes to air pollution whenever a fuel is...
The reaction N2(g) + O2(g) ⇄ 2 NO(g) contributes to air pollution whenever a fuel is burned in air at a high temperature, as in a gasoline engine. At 1500 K, Kc = 1.0×10-3. Suppose a sample of air has [N2] = 0.70 mol/L and [O2] = 0.20 mol/L before any reaction occurs. Calculate the equilibrium concentrations of reactants and products after the mixture has been heated to 1500 K. [N2] = M [O2] = M [NO] = M
1- The equilibrium constant, Kc, for the following reaction is 1.80×10-2 at 698 K. 2HI(g) -------->...
1- The equilibrium constant, Kc, for the following reaction is 1.80×10-2 at 698 K. 2HI(g) --------> H2(g) + I2(g) Calculate the equilibrium concentrations of reactant and products when 0.395 moles of HI are introduced into a 1.00 L vessel at 698 K. [HI] = M [H2] = M [I2] = M 2- student ran the following reaction in the laboratory at 1090 K: 2SO3(g) ----------> 2SO2(g) + O2(g) When he introduced SO3(g) at a pressure of 1.05 atm into a 1.00...
For the reaction N2(g) + 3 H2(g) equilibrium reaction arrow 2 NH3(g) at 25.0°C, the Kc...
For the reaction N2(g) + 3 H2(g) equilibrium reaction arrow 2 NH3(g) at 25.0°C, the Kc of the reaction is 5.4 ✕ 105. Use the given concentrations to determine the following. [N2] = 0.0028 M [H2] = 0.0045 M [NH3] = 0.30 M (a) Determine Q at this time. (Omit units.)
Nitric oxide (NO) reacts readily with chlorine gas as follows: 2NO(g)+Cl2(g)⇌2NOCl(g) At 700 K the equilibrium...
Nitric oxide (NO) reacts readily with chlorine gas as follows: 2NO(g)+Cl2(g)⇌2NOCl(g) At 700 K the equilibrium constant Kp for this reaction is 0.26. Predict the behavior of each of the following mixtures at this temperature. A) PNO=0.15atm, PCl2=0.31atm and PNOCl=0.11atm reaction will shift to the left (toward reactants) reaction will shift to the right (toward products) reaction is at equilibrium B) PNO=0.12atm, PCl2=0.10atm, and PNOCl=0.050atm reaction will shift to the left (toward reactants) reaction will shift to the right (toward...
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