Purchase Solution

Equilibrium Constant of SO2 and SO3

Not what you're looking for?

Ask Custom Question

The standard free energies of formation of SO2(g) and SO3(g) are -300.4 and -370.4kJ mol-1, respectively. Calculate the value of the equilibrium constant at 25'C for the reaction

2SO2(g) + O2(g) <=======> 2SO3(g)

Purchase this Solution
Solution Summary

The equilibrium constant is calculated from thermodynamic data.

Solution Preview

dG reaction = -RTlnK

dG reaction = dG formation of products - dG formation ...

Purchase this Solution
Free BrainMass Quizzes
Match Elements with their Symbols

Elements are provided: choose the matching one- or two-letter symbol for each element.

Thermochemistry

The quiz helps in revising basic concepts about thermochemistry.

Periodic table

Functional groups in Organic Chemistry

You will be tested on the names of functional groups in Organic Chemistry. It is very important to know the functional groups to understand Organic reactions.

Organic Chemistry Naming: Alkanes

This is a quiz which is designed to assist students with learning the nomenclature used to identify organic compounds. This quiz focuses on the organic compounds called Alkanes.

View More Free Quizzes
Related BrainMass Solutions

  • Calculating Equilibrium Concentrations

    What are the equilibrium concentrations of all reactants and products if the initial concentrations are [SO2]o = [NO2]o = 3.00 x 10-3 M and [NO]o = [SO3]o = 4.00 x 10-2 M? The value of the equilibrium constant for the reaction is 85.0 at 460 C.

  • General Chemistry problems

    Consider the following equilibrium. 2 SO2(g) + O2(g) 2 SO3(g) From which of the following starting conditions would it be impossible for this equilibrium to be achieved? a. 0.25 mol SO2(g) and 0.25 mol O2(g) in a 1.0-L container b.

  • 10 Chemistry Problems on half-life and formation

    a. 0.25 mol SO2(g) and 0.25 mol O2(g) b. 0.75 mol SO2(g) c. 0.25 mol SO2(g) and 0.25 mol SO3(g) d. 0.50 mol O2(g) and 0.50 mol SO3(g) e. 1.0 mol SO3(g) Please refer to the attached file.

  • Concentration

    26156 Concentration Reaction Systems At 700 K, the reaction 2SO2(g) + O2(g) = 2SO3(g) has the equilibrium constant Kc = 4.3 x 10^6, and the following concentration are present:[SO2] = 0.010 M: [SO3] = 10.M : [O2] =0.010 M When the reaction system reaches

  • Equilibrium Constant Calculation

    256 Again we first need to use ΔG°= ΔH° - T ΔS° with T in units of Kelvin And then second ΔG°= - RT ln Keq with T in units of Kelvin and R the gas constant R= (-8.31451*10-3 kJ mol-1 K-1) Now first we need to calculate the heat (enthalpy) change

  • Calculating Equilibrium Constants

    S + (3/2)O2 + SO3 --> SO3 + SO2 + 1/2 O2.... (EQUATION 1) You can see that certain things will subtract out on both sides and give you S + O2 --> SO2.... (EQUATION 2) Now look back at equation 1...

  • Equilibrium Pressures of Gas

    [SO3] M [NO] M [SO2] M [NO2] M First you need to write an equilibrium expression with the products on top and reactants on bottom: You know that both SO2 and NO2 will lose x concentration and SO3 and NO will gain x:

  • Reaction Kinetics, Rate Laws and Equilibrium

    At 700 K, the reaction 2SO2(g) + O2(g) 2SO3(g) has an equilibrium constant Kc = 4.3 x 106, and the following concentrations are present: [SO2] = 0.10 M [SO3] = 10 M [O2] = 0.10 M Is the mixture at equilibrium?

  • Equilibrium Constant and LeChatelier's Principle

    257921 Equilibrium Constant and LeChatelier's Principle 1, Calculate Ke for the following (equilibrium concentrations given below substances) a) PCl5 (g) + heat ↔ PCl3 (g) + Cl2 (g) [0.105] [0.219] [0.219

View More Related Solutions