O KINETICS AND EQUILIBRIUMCalculating equilibrium composition from an equilibrium constantSuppose a 250. mL flask is filled with 0.20 mol ofand 0.40 mol of HI. The following reaction becomes possible:H,(2) +I,(g) = 2HI(g)The equilibrium constant K for this reaction is 8.17 at the temperature of the flask.Calculate the equilibrium molarity of HI. Round your answer to two decimal places.

Answer: In this question we have use the equilibrium constant expression to find out the amount of…

Suppose a 250. mL flask is filled with 0.20 mol of H, and 0.40 mol of HI. The following reaction becomes possible: H,(2) + I,(2) = 2HI(g) The equilibrium constant K for this reaction is 8.17 at the temperature of the flask. Calculate the equilibrium molarity of HI. Round your answer to two decimal places.

Suppose a 250. mL flask is filled with 0.20 mol of H, and 0.40 mol of HI. The following reaction becomes possible: H,(2) + I,(2) = 2HI(g) The equilibrium constant K for this reaction is 8.17 at the temperature of the flask. Calculate the equilibrium molarity of HI. Round your answer to two decimal places.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 62QRT

See similar textbooks

Similar questions

At a certain temperature, K=0.29 for the decomposition of two moles of iodine trichloride, ICl3(s), to chlorine and iodine gases. The partial pressure of chlorine gas at equilibrium is three times that of iodine gas. What are the partial pressures of iodine and chlorine at equilibrium?
A sample of gaseous nitrosyl bromide (NOBr) was placed in a container tiued with a frictionless, massless piston, where it decomposed at 25C according to the following equation: 2NOBr(g)2NO(g)+Br2(g) The initial density of the system was recorded as 4.495 g/L. After equilibrium was reached, the density was noted to be 4.086 g/L. a. Determine the value of the equilibrium constant K for the reaction. b. If Ar(g) is added to the system at equilibrium at constant temperature, what will happen to the equilibrium position? What happens to the value of K? Explain each answer
A common type of reaction we will study is that having a very small K value (K 1). Solving for equilibrium concentrations in an equilibrium problem usually requires many mathematical operations to be perfomed. However, the math involved when solving equilibrium problems for reactions having small K values (K 1) is simplified. What assumption is made when solving the equilibrium concentrations for reactions with small K values? Whenever assumptions are made, they must be checked for validity. In general, the 5% rule is used to check the validity of assuming x (or 2 x, 3x, and so on) is very small compared to some number. When x (or 2 x. 3x. and so on) is less than 5% of the number the assumption was made against, then the assumption is said to be valid. If the 5% rule fails, what do you do to solve for the equilibrium concentrations?
The diagram represents an equilibrium mixture for the reaction N2(g) + O2(g) ⇌ 2 NO(g) Estimate the equilibrium constant.
Consider the following reaction at 1000 C: NO(g)+12 Cl2(g)NOCl(g) (a) Write an equilibrium constant expression for the reaction and call it K'. (b) Write an equilibrium constant expression for the decomposition of NOCl to produce one mole of chlorine gas. Call the constant K. (c) Relate K' and K.
At 2300 K the equilibrium constant for the formation of NO(g) is 1.7 103. N2(g) + O2(g) 2 NO(g) (a) Analysis shows that the concentrations of N2 and O2 are both 0.25 M, and that of NO is 0.0042 M under certain conditions. Is the system at equilibrium? (b) If the system is not at equilibrium, in which direction does the reaction proceed? (c) When the system is at equilibrium, what are the equilibrium concentrations?
A solution is prepared by dissolving 0.050 mol of diiodocyclohexane, C5H10I2, in the solvent CCl4.The total solution volume is 1.00 L When the reaction C6H10I2 C6H10 + I2 has come to equilibrium at 35 C, the concentration of I2 is 0.035 mol/L. (a) What are the concentrations of C6H10I2 and C6H10 at equilibrium? (b) Calculate Kc, the equilibrium constant.