Purchase Solution

equilibrium concentration when breaking HBr to H2 and Br2

Not what you're looking for?

Ask Custom Question

The Kc for HBr(g) breaking into Br2 and H2 is 2.18 e 6 at 760 degrees C.

If we start with 2.50 moles in a 12.0 Liters reaction vessel calculate the concentrations of H2, Br2 and HBr at equilibrium.

Could you show me how to set up the problem?

Purchase this Solution
Solution Summary

The solution explains how to calculate the equilibrium concentration when breaking HBr to H2 and Br2 from the definition of equilibrium constant.

Solution Preview

Please see the attached file for detailed solution.

The Kc for HBr(g) breaking into Br2 and H2 is 2.18 e 6 at 760 degrees C.

If we start with 2.50 moles in a 12.0 ...

Purchase this Solution
Free BrainMass Quizzes
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.

Periodic table

Thermochemistry

The quiz helps in revising basic concepts about thermochemistry.

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.

General Chemistry - Classification of Matter

This test will assess your knowledge on the classification of matter which includes elements, compounds and mixtures.

View More Free Quizzes
Related BrainMass Solutions

  • Given Kc starting with certain moles in container, calculate concentration

    H2(g)+Br2(g) f/r 2HBr(g) Let us assume the concentration of H2 and Br2 at equilibrium be x/12.

  • Equilibrium Concentrations

    The concentrations of H2 and Br2 will be 1.41*10-4 M. The concentration of HBr will be 0.208 M. This makes sense because the equilibrium constant is so large that the equilibrium will shift almost entirely to the product side.

  • Concentration and equilibrium

    15033 Concentration and equilibrium At 1495 degrees Celcius Kc for H2 + Br2 > 2HBR = 3 x 10 to the 4th power. H2 = .10 M Br2 = .20M What eqation(s)would I use or steps would I take to find the concentration of HBr?

  • Ke for Equilibrium Concentrations

    Increase in HBr concentration will cause the equilibrium to shift to the left (i.e. backward reaction). 4.

  • Concentrations and Solutions

    Starting with 3.20 moles of HBr in a 12.0-L reaction vessel, calculate the concentrations of H2, Br2, and HBR at equilibrium. 4) Assuming equal concentrations of conjugate base and acid, which one of the following mixtures is suitable for making

  • Dimerization of C5H6

    526407 Dimerization of C5H6 Suggest a method for measuring the rate of the following reactions: i) 2H2O2(aq) ------> 2H2O (l) + O2(g) ii) HBr(g) -----------> H2(g) + Br2(g) (colorless)............(colorless)....

  • 10 Chemistry Problems on half-life and formation

    The rate of disappearance of HBr in the gas phase reaction 2HBr(g) ® H2(g)+Br2(g) is 0.301 M s-1 at 150ºC. The rate of appearance of Br2 is _____M s-1.

  • Chemistry Sample Solution: Entropy For Reaction

    7203 Chemistry Sample Solution: Entropy For Reaction Calculate "delta" S for the following reaction: H2(g) + Br2(l) --> 2HBr(g) given: S[H2(g)] = 0.131 kJ/K S[Br2(l)] = 0.152 kJ/K S[HBr(g)] = 0.199kJ/K a. 0.482 kJ/K b. 0.681 kJ/K c. 0.115 kJ/K d. -0.084

  • Calculating delta S

    Solution: S for reaction = 2* S(HBr) -S(H2) -S(Br2) =2*0.199 - 0.131 -0.152 =0.398 - 0.283 =0.115 Hence option ( c) is correct This solution provides a quick equation and answer for finding delta S in a reaction.

View More Related Solutions