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If 0.300 mol of N2O4 is added to a 500 mL flask, what will be the...
Suppose a 500. mL flask is filled with 1.4 mol of NO and 0.60 mol on NO2. The following reaction becomes possible: NO3(g) + NO(g) <--> 2NO2(g) The equilibrium constant K for this reaction is 0.162 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places.
Suppose a 500. ml flask is filled with 1.3 mol of NO, and 1.5 mol of NO. The following reaction becomes possible: NO2(g) +NO(g) + 2NO2(g) The equilibrium constant K for this reaction is 9.06 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. i M x 6 ?
4) A 1.000 L flask is charged with 0.375 moles of gaseous N2O4 which is in equilibrium with gaseous NO2 with ΔH = 58.02 kJ/mol and ΔS = 176.6 J/(mol*K). What is the pressure in the flask at 300. K? (15 pts) (Hint – Solve for G, solve for K, solve equil. concentrations, and then how many moles of gas are there?)
28. 10. 10 mol of N,Q, is added to IL flask, what will be the concentrations atequilibrium? (quadratie equation required) N20, 2NO Initial Change Equilibrium 29. Find concentrations at equilibrium HA - HA 0.20 0 0 K. - 16 x 10 Initial Concentrations Change Equilibrium
Suppose a 500 ml flask is filled with 1.2 mol of NO, and 0.40 mol of NO the following reaction becomes possible: NO,() +NO(g) - 2NO(g) The equilibrium constant K for this reaction is 7.29 at the temperature of the flask Calculate the equilibrium molarity of NO. Round your answer to two decimal places
Suppose a 500. mL flask is filled with 1.7 mol of O_2 and 1.1 mol of NO. The following reaction becomes possible: N_2(g) + O_2(g) 2NO(g) The equilibrium constant K for this reaction is 3.80 at the temperature of the flask. Calculate the equilibrium molarity of NO.
Suppose a 500. ml flask is filled with 0.90 mol of NO, and 0.80 mol of NO. The following reaction becomes possible: NO2(g) + NO(g) + 2NO, (g) The equilibrium constant K for this reaction is 8.41 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. IM x 3 ?
Suppose a 500. mL flask is filled with 2.0 mol of I_2 and 0.40 mol of HI. The following reaction becomes possible: H_2(g) + IK_2(g) 2HI(g) The equilibrium constant K for this reaction is 9.22 at the temperature of the flask. Calculate the equilibrium molarity if I_2.
Suppose a 500. mL flask is filled with 0.70 mol of H2 and 0.60 mol of HI. The following reaction becomes possible: -2H1(g) The equilibrium constant K for this reaction is 2.38 at the temperature of the flask. Calculate the equilibrium molarity of H2. Round your answer to two decimal places.
Suppose a 500. mL flask is filled with 0.50 mol of H2 and 1.9 mol of HI. The following reaction becomes possible: H2(g)+12g2HIg The equilibrium constant K for this reaction is 4.94 at the temperature of the flask. Calculate the equilibrium molarity of H2. Round your answer to two decimal places.