At 613 K, K. 0.064 for the reaction Fe,O3(s) + 3H,(g) Z 2Fe(s) + 3H,O(g) a) What are the units of K, ? b) If the reaction is carried out in such a way that the partial pressure of hy- drogen at equilibrium is 1.00 atm, what is the concentration of hydro- gen in moles liter-1? c) What is the concentration of water vapor at equilibrium, in moles liter- and in atmospheres?

At 613 K, K. 0.064 for the reaction Fe,O3(s) + 3H,(g) Z 2Fe(s) + 3H,O(g) a) What are the units of K, ? b) If the reaction is carried out in such a way that the partial pressure of hy- drogen at equilibrium is 1.00 atm, what is the concentration of hydro- gen in moles liter-1? c) What is the concentration of water vapor at equilibrium, in moles liter- and in atmospheres?

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 13CR

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?
Show that the complete chemical equation, the total ionic equation, and the net ionic equation for the reaction represented by the equation KI(aq)+I2(aq)KI3(aq) give the same expression for the reaction quotient. KI3 is composed of the ions K+ and I3-.
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?
For the system SO3(g)SO2(g)+12 O2(g)at 1000 K, K=0.45. Sulfur trioxide, originally at 1.00 atm pressure, partially dissociates to SO2 and O2 at 1000 K. What is its partial pressure at equilibrium?
Nitric oxide and bromine at initial partial pressures of 98.4 and 41.3 torr, respectively, were allowed to react at 300. K. At equilibrium the total pressure was 110.5 torr. The reaction is 2NO(g)+Br2(g)2NOBr(g) a. Calculate the value of Kp. b. What would be the partial pressures of all species if NO and Br2, both at an initial partial pressure of 0.30 atm, were allowed to come to equilibrium at this temperature?
What is the pressure of BrCl in an equilibrium mixture of Cl2, Br2, and BrCl if the pressure of CI2 in the mixture is 0.115 atm and the pressure of Br2 in the mixture is 0.450 atm? Cl2(g)+Br2(g)2BrCl(g)KP=4.7102
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
At 1100 K, KP = 0.25 for the reaction 2SO2(g)+O2(g)2SO3(g) Calculate the equilibrium partial pressures of SO2, O2, and SO3 produced from an initial mixture in which PSO2=PO2=0.50atm and PSO3=0. (Hint: If you don t have a graphing calculator, then use the method of successive approximations to solve, as discussed in Appendix 1.4.)
5.16. In atmospheric chemistry, the following chemical reaction converts , the predominant oxide of sulfur that comes from combustion of S-containing materials, to , which can combine with to make sulfuric acid (and thus contribute to acid rain): (a) Write the expression for K for this equilibrium. (b) Calculate the value of for this equilibrium using the values in Appendix 2. (c) Calculate the value of K for this equilibrium. (d) If of and of are enclosed in a system in the presence of some liquid, in which direction would the reaction move?