17. A chemical reaction involves the combination of 0.200 mol of hydrogen and 0.200 mol of nitrogen in a rigid 2.00 L container at 773 K, represented by the following equation: 3H2(g) + N2(g) ⇌ 2NH3(g). At equilibrium the system contains 0.050 mol of ammonia. Use an ICE table to determine the equilibrium concentrations of hydrogen and nitrogen. Note: Show all calculations, follow the rules of significant figures, and box your final answer. (3 marks)

At 400 K, an equilibrium mixture of H2, 12, and HI consists of 0.065 mol H2, 0.079 mol 12, and 0.13 mol HI in a 4.50-L flask. What is the value of K, for the following equilibrium? (R= 0.0821 L atm/(K • mol)) 2HI(g) = H2(g) + 12(8) 0.29 8.2 0.039 O 26 3.4

Note:- • Do not provide handwritten solution. Maintain accuracy and quality in your answer. Take care of plagiarism. • Answer completely. • You will get up vote for sure.

Phosphorus pentachloride is formed when phosphorus trichloride and chlorine react according to the following reaction. PCI2(g) + Cl2(g) ⇌ PCI5(g) The equilibrium constant for the reaction is Kc = 43.7 at 130 °C. If 0.587 mo/ of phosphorus trichloride is added to 0.423 mol of chlorine in a 1.26-L reaction vessel and allowed to react at this temperature, what is the equilibrium concentration (in mol/L) of chlorine? Report your answer to THREE significant figures.

Consider the following reactions: CO (g) + H2O (g) <-> CO2 (g) + H2 (g)    |         Kp(1)= 0.694 at 1200.K C3H8 (g) + 3 H2O (g) <-> 3 CO (g) + 7 H2 (g) | Kp(2)= 8.175 x 1015 at 1200.K   Write the overall equation for the reaction of propane and steam to produce carbon dioxide and hydrogen. Calculate Kp for the overall process at 1200. K. What molecule(s) in the steps are reaction intermediate(s)? If 0.500 atm of CO2, H2, C3H8, and H2O are initially placed in the same container, then given your answer in part a., determine which direction the reaction will shift in order to establish equilibrium.

A 10.0 L reaction vessel at 489°C contained 0.100 mol H2, 0.361 mol I2, and 1.27 mol HI. Assuming that the substances are at equilibrium, find the value of K. at 489°C for the reaction of hydrogen and iodine to give hydrogen iodide. The equation is H2 (g) + I2 (9) = 2HI(9) K. =

In an experiment to study the formation of HI(g),H2(g) + I2(g) ⇌ 2 HI(g)At equilibrium, {H2} = 0.0137, {I2} = 0.0627 and {HI} = 0.0268. Calculate the value of Kc.

Use the References to access important values if needed for this question. The equilibrium constant, K for the following reaction is 6.50×10 at 298K. 2NOBR(g)=2NO(g) + Br,(g) If an equilibrium mixture of the three gases in a 17.2 L container at 29SK contains 0.369 mol of NOBR(g) and 0.435 mol of NO, the equilibrium concentration of Br, is M.

In an experiment, 0.37 mol H2 and 0.37 mol Br2 are mixed in a 1.00-L container (without any product initially), and the reaction forms HBr. Br2 (g) + H2 (g) ⇌ 2 HBr (g). If Kc = 64 for this reaction, determine the equilibrium concentration of HBr with 2 SIGNIFICANT FIGURES.

N2(g) +3H2(g) 2NH3 (g) what is the value of K. at 500 °C if the equilibrium concentrations are as follows: H2 = 0.50 M , N2] = 0.60 M , and [NH3] = 2.2 M ? Express the equilibrium constant to two significant figures. ? Ke =