Refer to theunbalancedchemical equation below for the following questions.N2(g) +02(g)=_NO(g)Write the equilibrium expression for this reactionAt equilibrium, the concentration of N2 is 5.32x10-3 M, O2 is 3.28 x10-3 Mand that of NO is 6.19 x10-6 M. Evaluate the equilibrium constant for thisreaction.Describe what is favored at equilibrium, reactants or products. Explain howyou know, please.

#Q.1: The given unbalanced equation is: N2(g) + O2(g) ⇌ NO(g) In order to write the equilibrium…

Refer to the unbalanced chemical equation below for the following questions. _02(g)= _N2(g) + _NO(g) Write the equilibrium expression for this reaction At equilibrium, the concentration of N2 is 5.32x10-3 M, 02 is 3.28 x10-3 M and that of NO is 6.19 x10-6 M. Evaluate the equilibrium constant for this reaction. Describe what is favored at equilibrium, reactants or products. Explain how you know,|please.

Refer to the unbalanced chemical equation below for the following questions. _02(g)= _N2(g) + _NO(g) Write the equilibrium expression for this reaction At equilibrium, the concentration of N2 is 5.32x10-3 M, 02 is 3.28 x10-3 M and that of NO is 6.19 x10-6 M. Evaluate the equilibrium constant for this reaction. Describe what is favored at equilibrium, reactants or products. Explain how you know,|please.

Living By Chemistry: First Edition Textbook

1st Edition

ISBN:9781559539418

Author:Angelica Stacy

Publisher:Angelica Stacy

ChapterU6: Showtime: Reversible Reactions And Chemical Equilibrium

Section: Chapter Questions

Problem SI4RE

See similar textbooks

Similar questions

A mixture of N2, H2, and NH3 is at equilibrium [according to the equationN2(g)+3H2(g)2NH3(g)] as depicted below: The volume is suddenly decreased (by increasing the external pressure) and a new equilibrium is established as depicted below: a. If the volume of the final equilibrium mixture is 1.00 L, determine the value of the equilibrium constant, K. for the reaction. Assume temperature is constant. b. Determine the volume of the initial equilibrium mixture assuming a final equilibrium volume of 1.00 L and assuming a constant temperature.
How does equilibrium represent the balancing of opposing processes? Give an example of an “equilibrium” encountered in everyday life, showing how the processes involved oppose each other.
In Section 13.1 of your text, it is mentioned that equilibrium is reached in a closed system. What is meant by the term closed system. and why is it necessary to have a closed system in order for a system to reach equilibrium? Explain why equilibrium is not reached in an open system.
. What does it mean to say that a state of chemical or physical equilibrium is dynamic?
Consider the following equilibrium: COBr2(g) CO(g) + Br2(g)Kc = 0.190 at 73 C (a) A 0.50 mol sample of COBr2 is transferred to a 9.50-L flask and heated until equilibrium is attained. Calculate the equilibrium concentrations of each species. (b) The volume of the container is decreased to 4.5 L and the system allowed to return to equilibrium. Calculate the new equilibrium concentrations. (Hint: The calculation will be easier if you view this as a new problem with 0.5 mol of COBr2 transferred to a 4.5-L flask.) (c) What is the effect of decreasing the container volume from 9.50 L to 4.50 L?
Consider an equilibrium mixture of four chemicals (A. B. C. and D. all gases) reacting in a closed flask according to the following equation: A+BC+Da. You add more A to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is re-established? Justify your answer. h. You have the original set-up at equilibrium, and add more D to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is re-established? Justify your answer.
During an experiment with the Haber process, a researcher put 1 mol N2 and 1 mol H2 into a reaction vessel to observe the equilibrium formation of ammonia, NH3. N2(g)+3H2(g)2NH3(g) When these reactants come to equilibrium, assume that x mol H2 react. How many moles of ammonia form?
. For the reaction 3O2(g)2O3(g)The equilibrium constant, K, has the value 1.121054at a particular temperature. a. What does the very small equilibrium constant indicate about the extent to which oxygen gas, O2(g), is converted to ozone gas, O3(g), at this temperature? b. If the equilibrium mixture is analyzed and [O2(g)]is found to be 3.04102M, what is the concentration of O3(g) in the mixture’?
Colorless N2O4 gas decomposes to form red-brown colored NO2 gas. Describe how the concentrations of N2O4 and NO2 would change increase or decrease as equilibrium was established in a sealed container that initially contained only N2O4. What observation would indicate that equilibrium had been established?