CO(g) + O2(g) -------------> 2CO2(g)
Kc = [CO2]^2/[CO][O2]
= (8.8)^2/(1.1)*(1.1) = 64
2N2(g) + O2(g) -----------> 2NO2(g)
Kc = [NO2]^2/[N2][O2]^3
= (0.02)^2/(1.8)^2 *2 = 6.2*10^-5
Reaction1 with Kc = 64.0> Reaction 2 ,with Kc = 6.2*10^-5 >>>>>answer
Plz any doubt comment on the BOX
sic Equilibrium Calculations 25 of 33 below the reaction. Rank the extent of each rea refers...
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...
3. Assuming that the system is at equilibrium, (1) which of the following reaction goes essentially to completion? easily detectable? (1) are (3) (2) which does not take place to a significant extent? (3) which equilibria (2) 2 BrCl(g) Ke 7.0 Kc 1.3 x 1069 Kc 0.154 Ke 4x 10-18 2 Cl2(g) Br2(g) + a. CO2(8) + O2(g) b. C(graphite) 2 CH4(8) 3 H2(8) C2H2(e) с. 2 Brig) d. Br2(g) Ke 1.0 x 10-95 F2(g) Hа() 2 HF(g) е.
help me by showing the work please Given the following information, Kc 2.0 x 10-38 Kc 2.4 x 101 2 NO(g) O2(g) 2 NO2 find the value of Ke for the following reaction: NO(g) + 03(g) NO2(g) + O2(g) A. 5.6 x 10-17 B. 3.5 x 1025 C. 9.0 x 1040 D. 1.1 x 10-4 practice Given the following information at 25°C, 2 NOCIg)2 NO(g) + Cl2(g) Kc 4.0 x 102 moV/L find the value of K for this reaction...
Name: 1. An exothermic reaction is allowed to reach equilibrium. If the temperature of the reaction mixture is decreased, the equilibrium will shift towards the product side: True False [1pt] 2. For the reaction C(s) + H2O(g) CO(g) + H2(g) a decrease in concentration of C(s) will cause the reaction to shift to the left oTrue False [1pt] 3. Define the following terms: [1.5pts] a. Activation Energy b. Exothermic Reaction c. Equilibrium [1p) 4. Determine the equilibrium constant K C(s)...
2. How is the equilibrium-constant expression (Kc) for the reaction: 2NO(a) = N2() + Ke=0.145; related to the following reaction? O2 (a) N2(a) + O2(a) = 2NO(a) K=.............. (b) 4NOQ = 2Nz () + 2O2(g) Kos......... (c) NO) 1/2 N2(0)+ 1/2O2(0) K3= +++ (d) 1/2 N2(a) + 1/2O2(a) = NO) Ke=.............. 3. Given Kc or ko for the following reactions, what is the value of Koor K? (a) l2(g) + Cl2(a) = 2ICIOX Kc = 2.0 x105 at 25°C (b)...
The equilibrium constant, Kc, for the following reaction is 10.5 at 350 K. 2CH2Cl2(g) >>CH4(g) + CCl4(g) Calculate the equilibrium concentrations of reactant and products when 0.327 moles of CH2Cl2 are introduced into a 1.00 L vessel at 350 K. [CH2Cl2] = M [CH4] = M [CCl4] = M The equilibrium constant, Kc, for the following reaction is 1.29×10-2 at 600 K. COCl2(g) >>CO(g) + Cl2(g) Calculate the equilibrium concentrations of reactant and products when 0.275 moles of COCl2(g) are...
6 The decomposition of ozone in the upper atmosphere is catalyzed by NO. The overall reaction and rate law are: rate k[O][NO] Os(g)+O(g)+20;(g); Write a possible mechanism that is consistent with rate law and identify an intermediate in the reaction. 7. A possible mechanism for the iodide ion catalyzed decomposition of hydrogen peroxide in aqueous solution is: -slow H2O:(aq) +I(aq)H;O(1) + 0I°(aq) -fast H20:(aq) +Or(aq)H:O()) +02(g)+l'(aq) What is: iv) the catalyst? iv) the intermediate ii) the rate law i) the...
Please answer all six thanks 1) The equilibrium constant for the following reaction is 2.90×10-2 at 1.15×103K. 2SO3(g) ------------------->2SO2(g) + O2(g) If an equilibrium mixture of the three gases in a 17.3 L container at 1.15×103K contains 0.437 mol of SO3(g) and 0.422 mol of SO2, the equilibrium concentration of O2 is M. 2) A student ran the following reaction in the laboratory at 1100 K: 2SO3(g) -------------------->2SO2(g) + O2(g) When she introduced 7.74×10-2 moles of SO3(g) into a 1.00 liter...
An equilibrium mixture of Co, O2 and CO2 at a certain temperature contains 0.0010 M CO2 and 0.0100 M 02. At this temperature, Kc equals 1.4 x 10^2 for the reaction: 2 CO(g) + O2(g) = 2 CO2(g). What is the equilibrium concentration of CO? O a. 7.1 x 10-7 Ob.1.4 x 10-2 M O c. 8.4 x 10-4 M d. 1.2 * 10-1 M
the equilibrium constant is given for two of the reactions below. Determine the value of the missing 23) - equilibrium constant A(g) +B(g) - AB(g) AB(g) + A(g) - A2B(g) 2 A(g) +B(g) - A2B(g) Ke=0.24 Ke = 3.8 Ke=? A) 0.63 B) 4.0 C) 16 D) 0.91 E) 3.6 24) 24) Determine the value of Kp for the following reaction, at 300K, if the equilibrium concentrations are as follows: (N2leq -1.5M, [H2leq = 1.1 M, (NH3 leq = 0.47...