i) the equilibrium constant is given by
ii) for the second reaction mixture
Since Q<K the reaction is not equilibrium.
Consider the following reaction at 600K: A reaction mixture at equilibrium at 600K contains 0.170 bar...
IV Consider the reaction: H_2 (g) + I_2 (g) = 2 HI(g) A reaction mixture in a 4.25 L flask at a certain temperature initially contains 0.668 g H_2 (g) and 86.9 g of I_2 (g). At equilibrium, the flask contains 78.4 g HI. Calculate K_c degree for this reaction at this temperature.
A student ran the following reaction in the laboratory at 677 K: 2HI(g) H_2(g) + I_2(g) When she introduced HI(g) at a pressure of 5.32 atm into a 1.00 L evacuated container, she found the equilibrium partial pressure of HI(g) to be 4.22 atm. Calculate the equilibrium constant, K_p, she obtained for this reaction. K_p =
At 400 K, an equilibrium mixture of H_2, I_2, and HI consists of 0.068 mol H_2, 0.075 mol I_2, and 0.13 mol HI in a1.00-L flask. What is the value of K_p, for the flowing equilibrium? (R = 0.0821 L middot atm (K - mol)) 2HI_(g) Rightwardsharpoonoverleftwardsharpoon H_2 (g) + I_2 (g) A) 0.039 B) 3.4 C) 26 D) 0.29 E) 8.2 If K = 0.150 for A_2 + 2B Rightwardsharpoonoverleftwardsharpoon 2AB, what is the value of K for the...
The equation for the formation of hydrogen iodide from H_2 and l_2 is: H_2(g) + I_2(g) 2 HI(g) The value of K_p for the reaction is 69.0 at 790.0 degree C. What is the equilibrium partial pressure of HI in sealed reaction vessel at 790.0 degree C if the initial partial pressures of H_2 and l_2 are both 0.1800 atm an initially there is no HI present?
a) H2(g) + 12 (g) = 2 HI(g) (3 points) A reaction mixture at equilibrium at 175 K contains Pue = 0.958 am, Pe=0.877 atm, and Pu=0.020 atm. A second reaction mixture, also at 175 K. contains Pie Pe=0.621 atm, and Pm 0.101 atm. Is the second reaction mixture at equilibrium? (Show all work for full credit) a IT b) (7 points) If not at equilibrium, what will be the partial pressure of HI when the reaction reaches equilibrium at...
Hydrogen iodide undergoes decomposition according to the equation 2HI(g) reversiblearrow H_2(g) + I_2(g) The equilibrium constant K_P at 500 K for this equilibrium is 0.060. Suppose 0.316 mol of HI is placed in a 8.00-L container at 500 K. What is the equilibrium partial pressure of I_2(g)? (R = 0.0821 L middot atm/(K middot mol)) 0.040 atm 0.020 atm 0.062 atm 0.0078 atm 0.32 atm
The equilibrium constant, K. for the following reaction is 0.636 at 600 K COC13(Q)= CO(g) + Cl() Calculate the equilibrium partial pressures of all species when COCK() is introduced into an evacuated flask at a pressure of 1.62 atm at 600K atm PcoCl, " Рco Рci, atm 8 more group attempts remaining Retry Entire Group Submit Answer
Determining the Equilibrium Constant K_p: Methane (CH_4) reacts with hydrogen sulfide to yield H_2 and carbon disulfide, a solvent used in manufacturing rayon and cellophane: CH_4(g) + 2H_2S(g) Equilibrium CS_2(g) + 4 H_2(g) What is the value of K_p at 1000 K if the partial pressures in an equilibrium mixture at 1000 K are 0.20 atm of CH_4, 0.25 atm of H_2S, 0.52 atm of CS_2, and 0.10 atm of H_2?
At 850 K, the value of the equilibrium constant K_p for the ammonia synthesis reaction: is 0.2010. If a vessel contains an initial reaction mixture in which (N_2) = 0.0100 M, [H_2) = 0.0200 M, and [N_2H_2] = 0.000200 M, what will the (N_2H_2] be when equilibrium is reached?
The equilibrium constant, K_c, for the following reaction is 55.6 at 698 K: H_2(g) + I_2(g) 2HI(g) Calculate the equilibrium concentrations of reactants and product when 0.351 moles of H_2 and 0.351 moles of I_2 are introduced into a 1.00 L vessel at 698 K. [H_2] = M [I_2] = M [HI] = M