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| From:  Albert1145 (Original Message) | Sent: 9/3/2008 9:48 AM |
Q1) A salt M2X3 has a Ksp value of 8.44x10-15. What is the millimolar (mM) concentration of X2-in a saturated solution of this salt?
I got 0.0018
Q2) What is the percent of CsCl by mass in a 0.86 M CsCl solution that has a density of 1.091 g/mL?
I got 13.58
Q3) If the change in entropy of the surroundings for a process at 455 K and constant pressure is -345 J K-1, what is the quantity of heat absorbed by the system in kilojoules?
I have no idea how to do this one
Q4) How is the equilibruim position of this reaction affected by increasing the pressure?
C(s) + H2O(g) + heat <-> Co(g) + H2(g)
I'm thinking since solids don't participate in the reaction, the equation will increase in its reactant because less molecules in the system will reduce its pressure.
Q5) At a particular temperature, K=3.75 for the following:
So2(g) + No2(g) <-> SO3 + NO(g)
Would the equilibruim shift if the gases in the flask were compressed?
If what I'm thinking in question 4 is correct, then I suppose the equation will not shift in any direction.
Albert |
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