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answer both If a 1.0 L flask is filled with 0.22 mol of N2 and 0.22...
Suppose a 250 ml flask is filled with 1.0 mol of NO and 0.70 mol of NO . The following reaction becomes possible: NO3(8) + NO(g) - 2NO(8) The equilibrium constant K for this reaction is 5.78 at the temperature of the flask. Calculate the equilibrium molarity of NO3. Round your answer to two decimal places. Ом 3 ? Expiat tion Check 20:30 MCGHE AB
1.Initially, 0.64 mol of PCl5 is placed in a 1.0 L flask. At equilibrium, there is 0.12 mol of PCl3 in the flask. What is the equilibrium concentration of PCl5? 2.What is the equilibrium concentration of Cl2? 3.What is the numerical value of the equilibrium constant, Kc, for the reaction?
Suppose a 500. ml flask is filled with 0.10 mol of H, and 1.0 mol of HCl. The following reaction becomes possible: H2(g) +C1, (g) = 2HCl(g) The equilibrium constant K for this reaction is 4.69 at the temperature of the flask. Calculate the equilibrium molarity of HCl. Round your answer to two decimal places. x 6 ?
For the reaction N2(g) + O2(g) 2NO(g), Kc = 4.0 at a particular temperature. In a 1.0-L container, 1.0 mol of N2 and O2 are mixed. Determine the concentration of NO once equilibrium is reached at the given temperature. =________ Please explain so I understand
Suppose a 500. mL flask is filled with 1.6 mol of O, and 0.70 mol of NO. The following reaction becomes possible: N2(g)02g)2NO (g) The equilibrium constant K for this reaction is 9.43 at the temperature of the flask Calculate the equilibrium molarity of NO. Round your answer to two decimal places. Ом X
A 3.00 L flask containing 2.0 mol of O2 and 1.0 mol of N2 is in a room that is at 22.0˚C. a. What is the total pressure in the flask? b. What fraction of the total pressure in the flask is due to N2? c. If the temperature of the flask is lowered, what happens to the pressure inside the flask? d. On a molecular level, explain why the pressure changes as you predicted in part (c). e. If...
A 2.0 L flask is filled with 0.30 mol SO3 , 0.40 mol of SO2 and 0.50 mol of O2 and allowed to reach equilibrium. Assume the temperature of the mixture is chosen so that Kc = 0.34. Predict the effect on the concentration of SO3 as the equilibrium is achieved by using Q, the reaction quotient. 2SO3(g) —> 2SO2(g) + O2(g)
P26. (Sec. 14.4) A 3.50 L reaction vessel is initially filled with 0.125 moles of N2 and 0.115 moles of O2 at 2000 °C. What are the molar concentrations of N2, O2, and NO at equilibrium? Hint: ICE Table] N:(g) +02(g) 2NO(g) Ke 0.109 a) [N2]-0.2121 M, [02]-0.3187 M, and [NO]-0.08421 M b) [N2] -0.03086 M, [O2]-0.02801 M, and [NO] 0.0097 M c [N2]-0.09258 M, [O2]-08403 M, and [NO] 0.0291 M d) [N2] 0.01543 M, [O2]-0.01401 M, and [NO]-0.00485 M...
1. At a particular temperature, a 3.0-L flask contains 2.4 mol Cl2, 1.0 mol NOCI, and 4.5 x 10-3 mol NO. Calculate K at this temperature for the following reaction: 2NOCI(g) — 2NO(g) + C13(g) 2. At a particular temperature, 8.0 mol NO2 is placed into a 1.0-L container and the NO2 dissociates by the reaction: 2NO,(8) 2NO(g) + 0,(8) At equilibrium the concentration of NO(g) is 2.0 M. Calculate K for this reaction. 3. Ammonia is produced by the...
1. At a particular temperature, a 3.0-L flask contains 2.4 mol Cl2, 1.0 mol NOCI, and 4.5 x 10-3 mol NO. Calculate K at this temperature for the following reaction: 2NOCI(g) — 2NO(g) + C13(g) 2. At a particular temperature, 8.0 mol NO2 is placed into a 1.0-L container and the NO2 dissociates by the reaction: 2NO,(8) 2NO(g) + 0,(8) At equilibrium the concentration of NO(g) is 2.0 M. Calculate K for this reaction. 3. Ammonia is produced by the...