![5) During an where the following reaction came to equilibrium. etion K s49.5 at the temperature of the experiment. were the equilibrium concentrations of H2, Ia, and HI? H2(g) + 12(g)与2H1(g) a) What [12] = [H11-](http://img.homeworklib.com/questions/ea565d10-4544-11eb-a416-d3db0d46ce39.png?x-oss-process=image/resize,w_560)
Homework Answers
H2(g) + I2(g) <------> 2HI(g)
Kc = [ HI ]^2/[ H2 ] [ I2 ] = 49.5
Initial concentration
[ H2 ] = (0.986mol/1.95L)×1L = 0.5056M
[ I2 ] = ( 0.493mol/1.95L)×1L = 0.2528M
[ HI ] = 0
concentration at equillibrium
[ H2 ] = 0.5056 - x
[ I2 ] = 0.2528 - x
[ HI ] = 2x
Therefore,
(2x)^2 /(0.5056 - x ) × ( 0.2528 - x) = 49.5
4x^2/(0.1278 -0.5056x - 0.2528x + x^2) = 49.5
4x^2/(x^2 - 0.7584x + 0.1278 ) = 49.5
45.5x^2 - 37.5408x + 6.3261=0
x = 0.2361
Therefore,
Equillibrium concentrations are
[ H2 ] = 0.5056 - 0.2361= 0.2695M
[ I2 ] = 0.2528 - 0.2361 = 0.0167M
[ HI ] = 2×0.2361 = 0.4722M
Add Answer to:
During an experiment, 0.986 mol H_2 and 0.493 mol I_2 were placed in a 1.95 L...
The equilibrium constant, K_c, for the following reaction is 55.6 at 698 K: H_2(g) + I_2(g)...
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
K_c for the reaction of hydrogen and iodine to produce hydrogen iodide, H_2 (g) + I_2...
K_c for the reaction of hydrogen and iodine to produce hydrogen iodide, H_2 (g) + I_2 (g) 2HI (g) is 54.3 at 430 degree C. Determine the initial and equilibrium concentration of HI if initial concentrations of H_2 and I_2 are both 0.10 M and their equilibrium concentrations are both 0.043 M at 430 degree C. [HI]_i = M [HI]_e = M
At a particular temperature, K = 1.00 Times 10^2 for the following reaction. H_2(g) + I_2(g)...
At a particular temperature, K = 1.00 Times 10^2 for the following reaction. H_2(g) + I_2(g) 2 HI(g) IN an experiment, 1.39 mol H_2, 1.39 mol HI are introduced intoa 1.00-L, container, Calculate the concentrations of all species when equilibrium is reached. H_2 M I_2 M HI M
At 400 K, an equilibrium mixture of H_2, I_2, and HI consists of 0.068 mol H_2,...
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...
IV Consider the reaction: H_2 (g) + I_2 (g) = 2 HI(g) A reaction mixture in...
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.
Suppose a 500. mL flask is filled with 2.0 mol of I_2 and 0.40 mol of...
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.
K_c for the reaction of hydrogen and iodine to produce hydrogen iodide, H_2(g)+I_2(g) doubleheadarrow 2HI(g) is...
K_c for the reaction of hydrogen and iodine to produce hydrogen iodide, H_2(g)+I_2(g) doubleheadarrow 2HI(g) is 54.3 at 430 degree C. Determine the initial and equilibrium concentration of H_2and I_2 are both 0.11 M and their equilibrium concentrations are both 0.048 M at 430 degree
Consider the following reaction: H_2 (g) + I_2 (g) Equilibrium 2 HI (g) Complete the following...
Consider the following reaction: H_2 (g) + I_2 (g) Equilibrium 2 HI (g) Complete the following table. Assume that all concentrations are equilibrium concentrations in M. Part A Find K_c at 25 degree C. Express your answer using three significant figures. K_c = _______ Part B Find [H_2] at 340 degree C. Express your answer using two significant figures. [H_2] = _______ M Part C Find [HI] at 445 degree C. Express your answer using three significant figures. [HI] =...
Hydrogen iodide undergoes decomposition according to the equation 2HI(g) reversiblearrow H_2(g) + I_2(g) The equilibrium constant...
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
A 1.00-L flask is filled with 1.00 moles of H_2 and 2.00 motes of I_2. The...
A 1.00-L flask is filled with 1.00 moles of H_2 and 2.00 motes of I_2. The value of the equilibrium constant for the reaction of hydrogen and iodine reacting to form hydrogen iodide is 50.5 under the given conditions. What are the equilibrium concentrations of H_2, I_2, and HI in moles/L?
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
K_c for the reaction of hydrogen and iodine to produce hydrogen iodide, H_2 (g) + I_2 (g) 2HI (g) is 54.3 at 430 degree C. Determine the initial and equilibrium concentration of HI if initial concentrations of H_2 and I_2 are both 0.10 M and their equilibrium concentrations are both 0.043 M at 430 degree C. [HI]_i = M [HI]_e = M
At a particular temperature, K = 1.00 Times 10^2 for the following reaction. H_2(g) + I_2(g) 2 HI(g) IN an experiment, 1.39 mol H_2, 1.39 mol HI are introduced intoa 1.00-L, container, Calculate the concentrations of all species when equilibrium is reached. H_2 M I_2 M HI M
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...
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.
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.
K_c for the reaction of hydrogen and iodine to produce hydrogen iodide, H_2(g)+I_2(g) doubleheadarrow 2HI(g) is 54.3 at 430 degree C. Determine the initial and equilibrium concentration of H_2and I_2 are both 0.11 M and their equilibrium concentrations are both 0.048 M at 430 degree
Consider the following reaction: H_2 (g) + I_2 (g) Equilibrium 2 HI (g) Complete the following table. Assume that all concentrations are equilibrium concentrations in M. Part A Find K_c at 25 degree C. Express your answer using three significant figures. K_c = _______ Part B Find [H_2] at 340 degree C. Express your answer using two significant figures. [H_2] = _______ M Part C Find [HI] at 445 degree C. Express your answer using three significant figures. [HI] =...
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
A 1.00-L flask is filled with 1.00 moles of H_2 and 2.00 motes of I_2. The value of the equilibrium constant for the reaction of hydrogen and iodine reacting to form hydrogen iodide is 50.5 under the given conditions. What are the equilibrium concentrations of H_2, I_2, and HI in moles/L?
Most questions answered within 3 hours.
-
A sock stuck to the side of a clothes-dryer barrel has a
centripetal acceleration of 24...
asked 4 minutes ago -
A perfect gas undergoes an isentropic process such that its
volume doubles. If the ratio of...
asked 24 minutes ago -
list the elements in groups 3A to 6A in the same order as in the
periodic...
asked 33 minutes ago -
Estimating effect size. Peng and Chen (2014)
evaluated effect size estimates for various tests. In their...
asked 43 minutes ago -
Write a script in MySQL that creates and calls a stored
procedure name test. This procedure...
asked 44 minutes ago -
If we test the following: H0: μ = 17
vs. H1: μ ≠ 17 and the...
asked 54 minutes ago -
in the past year TVG had revenues of 3 million, cost
of goods sold of $25...
asked 1 hour ago -
4) In a polypeptide, which bond cannot rotate because of its
partial double bond character?
The...
asked 1 hour ago -
Assume that in the short run L = 1,000 and K = 100. 1. What is...
asked 1 hour ago -
At a given temperature, 2.06 atm of H2 and 3.7 atm of Br2 are
mixed and...
asked 1 hour ago -
Sodium reacts with Hydrochloric acid to form sodium chloride and
hydrogen gas. 2Na(s)+ 2 HCl(aq)-> 2...
asked 1 hour ago -
The following circuits (1 & 2) are combined to form a
series-parallel circuit and resulting circuit...
asked 1 hour ago