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Solving Equilibrium

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Question: 4HCl + O2 > 2Cl2 + 2H2O

HCl is at 2.30 atm, O2 is at 1.00 atm and they both react at 750 K. Equilibrium pressure of Cl2 is .93 atm. How do you go about finding the Kp at 750 K?

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https://brainmass.com/chemistry/chemical-equilibrium/solving-equilibrium-15032

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For a reaction of the type, aA + bB ---- cC + dD involving gases, we have, Kp = {[pC]^c * [pD]^d }/[pA]^a ...

Solution Summary

The following solution is comprised of an explanation of how to go through the following chemistry-based question step-by-step. The solution is about 50 words.

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Aqueous Ionic Equilibrium

1- Consider the following titration curve of a weak acid titrated with strong base. At which point(s) on the graph is the solution a buffer? (see attachment for image)

2- Which of the following solutions has the highest buffer capacity? Choose from:
0.100 M NaCl / 0.100 M NaOH
pure H2O
0.050 M NaCN / 0.050 M HCN
0.100 M HCl / 0.100 M NaOH
0.025 M NaCN / 0.025 M HCN

3- A student adds solid silver chloride (AgCl) to each of two beakers: one containing 1.0 L of pure water, and one containing 1.0 L of 0.500 M NaCl. In which will AgCl be more soluble, and why? Choose from:
0.500 M NaCl: the sodium ions in the solution will complex with the chloride, allowing more AgCl to dissolve.
0.500 M NaCl: in the 0.500 M NaCl solution, the chloride ions that are already present will increase the amount of AgCl that dissolves by decreasing the value of
Neither: AgCl is completely insoluble, and will not dissolve in either.
Pure H2O: in the 0.500 M NaCl solution the chloride ions that are already present will inhibit the AgCl from dissolving by increasing the value of Q.
Both: AgCl is freely soluble in both.

4- Determine the pH of each solution.
0.16M KCHO 2
0.16M KCHO 2
0.25M KI

5- Ammonia, NH 3 , is a weak base with a K b value of 1.8×10 −5 .
What is the percent ionization of ammonia at this concentration?

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