13. Determine the concentration of each substance in each of the following equilibrium reactions. a. N2(g)...
Consider the equilibrium 4. N2(g) 02(g) Br2(g) 2NOBr (g) Calculate the equilibrium constant Kp for this reaction, give the following information (298.15 K) NO (g) +1/2Br2(g) NOBr(g) Ke 4.5 2 NO (g)N2(g) 02(g) Ke 3.0 x 102 5. For the BrCl decomposition reaction 2BrCl(g) Br2(g Cl2(g) Initially, the vessel is charged at 500 K with BrCl at a partial pressure of 0.500 atm. At equilibrium, the partial pressure of BrC is 0.040 atm. Calculate Kp value at 500K Consider the...
Ch. 13 NAME 1. Consider the reaction: 2NO (g)+ 2H:(g) N2(g)+ 2H O (g) At a certain temperature, the equilibrium concentrations are [NO]-0.31 M [H2]-0.16 M [N2] 0.082 M and [H:0]-4.64 M (a) Write the equilibrium expression for the reaction. (b) Determine the value of the equilibrium constant 2. The equilibrium constant Kc for the following reaction is 150.7 at 1 15°C: 12 (g) + Br2 (g) ←→ 2 IBr(g) 2.00 moles of each gas (l2, Br: and IBr) are...
2. Determine Ke for the reaction (Answer: 9.7x10-16): 2 N2(g) + 1/2O2(g) + Brz(g) $ NOBr (g) From the following information (Hint: Manipulate the equations first, then manipulate K values): 2 NO(g) 5 N2(g) + O2(g) NO (g) + Br2 (g) $ NOBr (g) Ke=2.1x1030 Ko=1.4
The following reactions have the indicated equilibrium constants at a particular temperature: N2(g) + O2(g) = 2NO(g) Ke = 4.3 x 10-25 2NO(g) + O2(g) + 2NO:(8) K-6.4 x 10 Determine the values of the equilibrium constants for the following equations at the same temperature: (a) 4NO(g) = N2(g) + 2NO:(g) x 10 (b) 4NO:() = 2N:(0) + 40:(8) x 10 (c) 2NO(g) + 2NO3(g) = 30:(g) + 2N:(g) x 10
The following reactions have the indicated equilibrium constants at a particular temperature: N2(g) + O2(g) = 2NO(g) Ke = 4.3 x 10-25 2NO(g) + O2(g) + 2NO:(8) K-6.4 x 10 Determine the values of the equilibrium constants for the following equations at the same temperature: (a) 4NO(g) = N2(g) + 2NO:(g) x 10 (b) 4NO:() = 2N:(0) + 40:(8) x 10 (c) 2NO(g) + 2NO3(g) = 30:(g) + 2N:(g) x 10
z 5. Consider the following equilibria in aqueous solution at room temperature: 2NO(g) = N2(g) + O2 (8) K= 1.0 x 10" N2(g) + O2 (6) + Br2 (8) = 2NOBrg) K = 2.0 x 10" Find the numerical value of K for the reaction 2 NOBr (g) = 2 NO (g) + Br2 (g) a) 2.0 x 103 b) 5.0 x 1056 C) 1.0 x 1030 d) 5.0 x 10-4
The equilibrium constant, Kc, for the following reaction is 1.28×10-3 at 231 K. 2NOBr(g) goes to 2NO(g) + Br2(g) . When a sufficiently large sample of NOBr(g) is introduced into an evacuated vessel at 231 K, the equilibrium concentration of Br2(g) is found to be 0.200 M. Calculate the concentration of NOBr in the equilibrium mixture. __M
Tutored Practice Problem 15.2.3 COUNTS TOWARDS GRADE Manipulate equilibrium constant expressions. The equilibrium constant for the following reaction is 2.18x10-3 at-24°C. 2 NOBr(g)2 NO(g) + Br2(g) K-2.18x103 at -24 °C Calculate the equilibrium constant for the following reactions at -24 °C. (a) 2 NO(g) +Br2g NOBr(g) K- (b) NOBr(g)_NO(1/2 Br2(g) K- Check & Submit Answer Show Approach
Determine the equilibrium concentration of each species for the following reaction: C O ( g ) + H 2 O ( g ) ⇌ C O 2 ( g ) + H 2 ( g ) K c = 0.64 Given the the starting concentrations of each species are as follows: [CO] = 1.1 M, [H2O] = 0.11 M, [CO2] = 3.7 M, and [H2] = 4.6 M
Question 47 Which reaction shown will have the highest concentration of products at equilibrium? O N2(g) + 3H2(g) + 2NH3(g) K=0.278 • 2502(g) + O2(g) + 2503(g) K=1.7 x 106 O2HBr(g) + H2(g) + Br2(g) K= 7.7 x 10-11 O2NOCI(g) 2NO(g) + Cl2(g) K=1.8 x 10-2 !! Proctorio is sharing your screen Stop she OPCI(8) EPC13(g) + Cl2(8) K= 1.1 x 10-2 DLL (intel CORE i5 10TH GEN weak as: NH3 СА. Сон Printplof Chemistry weak acid : HT H3...