The reaction N204(g) * 2NO2(3) has a K, = 0.140 at 25 °C. In a reaction vessel containing the gases in equilibrium at that temperature, the partial pressure of N204 was 0.325 atm. (a) What was the partial pressure of NO2 in the reaction mixture? pressure of NO2 = atm (b) What was the total pressure of the mixture of gases? total pressure = i atm

The reaction N204(g) * 2NO2(3) has a K, = 0.140 at 25 °C. In a reaction vessel containing the gases in equilibrium at that temperature, the partial pressure of N204 was 0.325 atm. (a) What was the partial pressure of NO2 in the reaction mixture? pressure of NO2 = atm (b) What was the total pressure of the mixture of gases? total pressure = i atm

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 7QRT

See similar textbooks

Similar questions

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-.
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?
Suppose a reaction has the equilibrium constant K = 1.3 108. What does the magnitude of this constant tell you about the relative concentrations of products and reactants that will be present once equilibrium is reached? Is this reaction likely to be a good source of the products?
. What does it mean to say that a state of chemical or physical equilibrium is dynamic?
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?
Write an equation for an equilibrium system that would lead to the following expressions (ac) for K. (a) K=(Pco)2 (PH2)5(PC2H6)(PH2O)2 (b) K=(PNH3)4 (PO2)5(PNO)4 (PH2O)6 (c) K=[ ClO3 ]2 [ Mn2+ ]2(Pcl2)[ MNO4 ]2 [ H+ ]4 ; liquid water is a product
Describe a nonchemical system that is not in equilibrium, and explain why equilibrium has not been achieved.
Explain why the development of a vapor pressure above a liquid in a closed container represents an equilibrium. What are the opposing processes? How do we recognize when the system has reached a state of equilibrium?
At 1 atm and 25 C, NO2 with an initial concentration of 1.00 M is 3.3103 decomposed into NO and O2. Calculate the value of the equilibrium constant for the reaction. 2NO2(g)2NO(g)+O2(g)