Help Solving Chemistry Equilibrium Problems Before Test Tomorrow

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SUMMARY

This discussion focuses on solving chemistry equilibrium problems, specifically involving the reactions of phosphorus (P4), hydrogen (H2), nitrogen (N2), oxygen (O2), ammonia (NH3), and hydrochloric acid (HCl). The participant seeks assistance with three specific equilibrium calculations, including the equilibrium concentrations of P4 and H2 when 1.6 moles of PH3 are formed, and the moles of N2 in a closed system with given amounts of O2 and NO. The participant provides their calculated answers and seeks confirmation of their accuracy.

PREREQUISITES
  • Understanding of chemical equilibrium concepts
  • Familiarity with the equilibrium constant (K) and its application
  • Knowledge of stoichiometry in chemical reactions
  • Ability to perform calculations involving moles and concentrations
NEXT STEPS
  • Study the calculation of equilibrium constants for various reactions
  • Learn how to set up and solve equilibrium expressions
  • Explore the Le Chatelier's principle and its applications
  • Practice solving equilibrium problems involving multiple reactants and products
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Chemistry students, educators, and anyone preparing for chemistry tests or exams focused on equilibrium reactions.

DLxX
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Ive already done these problems and I think I'm doing them correctly, but I can't be 100% sure since I don't have the answers. Please help if you can since I have my test tommorow. Thanks

Here are some of the questions

1. If 2.6 moles of P4 and 3.6 moles of H2 are reacted till the following equilbirum is established P4 + 6H2 <===> 4PH3 , and if at equilbrium 1.6 moles of PH3 are formed, how many moles of P4 and H2 are in the equilibrium mixture?

(I got .4 and 2.4)





2. At 2000C k=6.2 x 10^-4 for the system N2 + O2 <==> 2NO. How many moles of N2 will exist in equilbrium in a 50 Liter box with .0062 mole of O2 and .0010 mole of NO?

(I got .258 mole)




3. If for the system NH4Cl (s) <=====> NH3 (g) + HCl (g) K=1.0 x 10^-4 . Find the moles of NH3 in a 100 liter container if initially there were 10.0 moles of NH3 added to 10 moles of HCl?

(I got .1)
 
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I got 2.2 and 1.2 moles for P4 and H2, resp. 0.4 and 2.4 moles are really present, but they are reacting amounts of them, so you will subtract these from the beginning amounts, i.e., 2.6 and 3.6 moles, resp.

I don't have enough time to look at the remaining questions, sorry.
 
1. If 2.6 moles of P4 and 3.6 moles of H2 are reacted till the following equilbirum is established P4 + 6H2 <===> 4PH3 , and if at equilbrium 1.6 moles of PH3 are formed, how many moles of P4 and H2 are in the equilibrium mixture?

I'm not going to check all of your answers for you, you can correspond with the following and ask any questions.

for the first question

[tex]K= \frac{[2.6moles-x][3.6-6x]^{6}}{[4x]^{4}}[/tex]