Ch.14 - Chemical EquilibriumWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: For the following reaction, Kp = 8,532 at a given temperature.2 NO(g) + Cl2(g) <=> 2 NOCl(g)At equilibrium, PNO = 0.734 and PCl2 = 0.303. What is the equilibrium partial pressure of NOCl?Give your answer to 3 significant figures.

Problem

For the following reaction, Kp = 8,532 at a given temperature.

2 NO(g) + Cl2(g) <=> 2 NOCl(g)

At equilibrium, PNO = 0.734 and PCl2 = 0.303. What is the equilibrium partial pressure of NOCl?

Give your answer to 3 significant figures.

Solution

We’re being asked to determine the equilibrium partial pressure of NOCl.


We are given the equation: 

2 NO(g) + Cl2(g) ↔ 2 NOCl(g)


Recall that the equilibrium constant is the ratio of the products and reactants

We use Kp when dealing with pressure and Kc when dealing with concentration:


Kp=PproductsPreactants     Kc=[products][reactants]


Note that solid and liquid compounds are ignored in the equilibrium expression.


Solution BlurView Complete Written Solution