18. Equation of reaction : Cl2 + 2 NO 2 NOCl
Initial conc. of NOCl = 2.00 M
Equilibrium conc. of Cl2 = 0.979 M
From the equation, [NO] = 2 * [Cl2] = 2 * 0.979 = 1.958 M
Concentration of NOCl reacted = moles of NO formed = 1.958 M
Equilibrium [NOCl] = inititial - reacted = 2.0 - 1.958 = 0.042
Writing the equation for K: K = [NOCl]2 / ([Cl2] * [NO]2] = 0.0422 / (0.979 * 1.9582) = 4.70 * 10-4 M-1
18. Consider the equilibrium When 2.000 MNOCI is placed in an empty tank at 500,0 K...
6. In this experiment 2.00 mols of NOCI are placed in a 1.00L equilibrium is achieved, nitrogen monoxide NO and chlorine gas equilibrium concentration of NO is 0.66 M. Calculate Kc for this placed in a 1.00 L flask @ 298 K. After ad chlorine gas Cl, form. The alculate Kc for this equilibrium reaction: ? 2 NOCI (g) = 2 NO(g) + Cl2 (8) 3. eaction vessel is charged with hydrogen iodide and heated in a sealed tube to...
please show work for these problems, correct answers are circled 18. Consider the following equilibrium: Clip) + 2NO) = 2NOCK If 12.0 moles of Cly, 10.24 moles of NO and 2.00 moles NOCI are placed in a 2.00 L container and the system moves to the right to get to equilibrium If there are 100 moles NOCI acquilibrium, calculate the key A 0.006 B5.58 19. What will cause the value of key for an exothermic reaction to decrease? A increasing...
Consider the following system at equilibrium: 2 NO2(g)⇄ N2O4(g) If 2.00 M NO2 is placed in a flask and allowed to react. At equilibrium, 1.80 M NO2 is present. A. Calculate the equilibrium concentration of N2O4. B. Calculate the equilibrium constant, K
Consider the following reaction for which K 1.60 x 10 at some temperature 2 NOCl (g) ㄹ 2 NO (g) + Cl2(g) In a given experiment, 0.935 moles of NOCI(g) were placed in an otherwise empty 1.51 L vessel. Complete the following table by entering numerical values in the Initial row and values containing the variable "x" in the Change and Equilibrium rows. Define 2x as the amount (mol/L) of NOCI that reacts to reach equilbrium. Include signs in the...
Consider the slowing equilibrium: 2NOC(g) =2NO(g) + Cl2(g) with K = 1.6 x 10 Segiment 100 mole of pure NOCI and 1.00 mole of pure Cly are placed in 100.container Reference: Ref 13-6 Tundles of NO react, what is the equilibrium concentration of Cl2? 01-2
2. The compound NOCI decomposes to nitric oxide and chlorine according to the following equation: 2 NOCI (g) 2 NO (g+ Cl (g) Suppose that 0.480 mol NOCI is placed in a 5.00-L flask at a given temperature. When equilibrium has been established, is found that the concentration of NO is 0.0196 M. Calculate the equilibrium constant for this reaction.
At a certain temperature K = 0.500 for the following reaction: SO3 (g) + NO (g) ⇌ NO2 (g) + SO2 (g) If 0.200 mol of SO3 and 0.200 mol of NO are placed in a 2.000 L container and allowed to come to equilibrium, what will be the concentration of SO2?
Consider the reaction: NiO(s)+CO(g)⇌Ni(s)+CO2(g) Kc=4000.0 at 1500 K When calculating the answer, do not round to the appropriate number of significant figures until the last calculation step. Part A If a mixture of solid nickel(II) oxide and 0.11000 M carbon monoxide is allowed to come to equilibrium at 1500 K, what will be the equilibrium concentration of CO2?
please show all work thanks B. Consider the system N2 (9) 3H2 (g) 2 NHs (9) dbie of NHs was placed in a 2.000 liter flask at 25°C. When equilibrium at that temperature, it was determined that the ammonia was reduced A 2.568-g sample was reached N to 75.0% of its original value. 1. Calculate K for the decomposition of 2.00 moles of ammonia at 25.0°C. 2. Calculate K for the decomposition of 2.00 moles of ammonia at NH3 is...
Part A Consider the reaction between NO and Cl, to form NOCI: 2NO(g) + Cl (9) 2NOCI (9) A reaction mixture at a certain temperature initially contains only (NO) = 0.70 M and (Cly) = 0.55 M. After the reaction comes to equilibrium, the concentration of NOCI is 0.23 M. You may want to reference (Page 688) Section 15.6 while completing this problem. Find the value of the equilibrium constant (K) at this temperature. Express your answer using two significant...