1mol of H2, 2.0mol of I2, 3mol of HI are injected into 1 Litre flask. What...
1mol of H2, 2.0mol of I2, 3mol of HI are injected into 1 Litre flask. What will be the equilibrium concentration of H2, I2, HI at 490^C? The equilibrium constant for the reaction is 45.9.
Homework Answers
![Ans Kc - 45.9 H₂ Iz 2 HI - 2 3 initial mole at eluilibrium |-X 3 + 2x 2-x Kc = [HI]2 [H22 Iz usog = (3+2x)? (1-x) (2-x) X = 0](http://img.homeworklib.com/questions/09d13220-2080-11eb-9f2a-15bd8fa038ce.png?x-oss-process=image/resize,w_560)
Add Answer to:
1mol of H2, 2.0mol of I2, 3mol of HI are injected into
1 Litre flask. What...
The following reaction was performed in a sealed flask at 999 degreesCelsius. H2 (g) + I2...
The following reaction was performed in a sealed flask at 999 degreesCelsius. H2 (g) + I2 (g) 2 HI (g) Kc = 222. If H2 and I2 are both 0.15 M at equilibrium, what is the concentration of HI at equilibrium?
Suppose that 0.1000 mole each of H2 and I2 are placed in 1.000-L flask, stoppered, and...
Suppose that 0.1000 mole each of H2 and I2 are placed in 1.000-L flask, stoppered, and the mixture is heated to 425oC. At equilibrium, the concentration of I2 is found to be 0.0210 M. a) What are the equilibrium concentrations of H2 and HI, respectively? Calculate Kc for the following reaction at 425oC. H2(g) + I2(g) ⇄ 2 HI(g) b) If the initial concentrations of H2 and I2 are 1.000 M each, and the initial concentration of HI is 0.000,...
Suppose a 500.mL flask is filled with 1.7mol of I2 and 0.80mol of HI. The following...
Suppose a 500.mL flask is filled with 1.7mol of I2 and 0.80mol of HI. The following reaction becomes possible: H2(g)+I2(g) > 2HI(g). The equilibrium constant K for this reaction is 0.142 at the temperature of the flask. Calculate the equilibrium molarity of HI. Round your answer to two decimal places.
A sealed tube initially contains 9.84x10-4mol of H2and 1.38x10-3mol of I2. It is kept at 350C...
A sealed tube initially contains 9.84x10-4mol of H2and 1.38x10-3mol of I2. It is kept at 350C until the reaction H2(g) + I2(g) <=> 2HI (g) comes to equilibrium. At equilibrium 4.73x10-4moles of I2 are present. Calculate the number of moles of H2 and HI at equilibrium and the equilibrium constant Kc for the reaction. (please provide steps on how to approach this problem) I noticed that the system is not initially at equilibrium so i used ICE method to find...
An equilibrium mixture contains 0.950 mol HI, 0.490 mol I2, and 0.290 mol H2 in a...
An equilibrium mixture contains 0.950 mol HI, 0.490 mol I2, and 0.290 mol H2 in a 1.00-L flask. What is the equilibrium constant for the following reaction? 2HI(g) H2(g) + I2(g) K = How many moles of I2 must be removed in order to double the number of moles of H2 at equilibrium? mol I2
A flask containing 0.10 atm of H2(g) and excess I2(s) is heated and allowed to reach...
A flask containing 0.10 atm of H2(g) and excess I2(s) is heated and allowed to reach equilibrium according to the reaction below. The equilibrium constant is 0.25 at this temperature. What is the partial pressure of HI(g) at equilibrium? 2HI(g) --> H2(g) + I2(s) Please help and show work. Thank you
consider the equilibrium reaction of H2 (g) + I2 (g) <-----> 2 HI (g) it has...
consider the equilibrium reaction of H2 (g) + I2 (g) <-----> 2 HI (g) it has an equilibrium constant Kc = 54.3 at 430°C. if the initial concentration of [HI]0 = 2.000 M. what are the equilibrium concentrations?
The following reaction: H2 (g) + I2 (g) ⇋ 2 HI (g) Has an equilibrium constant...
The following reaction: H2 (g) + I2 (g) ⇋ 2 HI (g) Has an equilibrium constant of 30.5 under certain conditions. If initial concentrations of reactants and product are: [H2] = 0.100 M; [I2] = 0.100 M; and [HI] = 0.250 M, what will be the equilibrium concentration of HI?
Consider the reaction: H2(g)+I2(g)⇌2HI(g) A reaction mixture in a 3.69 −L flask at 500 K initially...
Consider the reaction: H2(g)+I2(g)⇌2HI(g) A reaction mixture in a 3.69 −L flask at 500 K initially contains 0.377 g H2 and 17.93 g I2. At equilibrium, the flask contains 17.72 g HI. Calculate the equilibrium constant at this temperature.
Given the reaction below, H2 (g)+ I2 (g)⇌ 2 HI (g) Kc = 50.5 What was...
Given the reaction below, H2 (g)+ I2 (g)⇌ 2 HI (g) Kc = 50.5 What was the initial mass of HI (g) placed in a sealed 1.50 L flask which resulted in 0.025 mol of each of H2 (g) and I2 (g) being found in the flask at equilibrium?
Most questions answered within 3 hours.
-
Where is the error in this code sequence?
String s1 = "Hello";
String s2 = "ello";...
asked 11 months ago -
Financial data for Joel de Paris, Inc., for last year
follow:
Joel de Paris, Inc.
Balance...
asked 11 months ago -
Consider this reaction:
Al2(SO4)3 (aq)+ BaCl3
(aq) Al2Cl6 (aq)- +
3BaSO4(s) . What is the...
asked 11 months ago -
Suppose that Savneet is considering increasing her
recent random sample from 20 car rentals to 40...
asked 11 months ago -
Trucks arrive at an unloading terminal at an average rate of 120
per hour.
Trucks arrive...
asked 11 months ago -
Why are methanol and ethanol completely soluble in water while
octanol is not very little soluble....
asked 11 months ago -
A facilities manager at a university reads in a research report
that the mean amount of...
asked 11 months ago -
When the CuSO4 is rehydrated by adding water to the anhydrous
compound, is this an endothermic...
asked 11 months ago -
A ray of sunlight is passing from diamond into crown glass; the
angle of incidence is...
asked 11 months ago -
A block of mass 0.249 kg is placed on top of a light, vertical
spring of...
asked 11 months ago -
how do the kidneys compensate in the presences of acidosis
a) trigger hyperventilate
b) reserve acid...
asked 11 months ago -
Question 501 pts
The rental rate of capital to the firm increases. Which of the
following...
asked 11 months ago