Tuesday
July 22, 2014

Posts by Raskin


Total # Posts: 13

Chemistry
Calculate the theoretical pH after 2.50 mL and 9.50 mL of NaOH has been added in both the titration of HCl and of HC2H3O2. Given: Molarity of all chemicals are 0.1 M HCl and HC2H3O2 are 8ml prepared in 100ml water.

Chemistry
Deriving Chem Beer's Law's Equation By comparing the absorbance of each trial solution, Aeq, to the absorbance of the standard solution, Astd, [FeNCS2+]eq can be determined. Two Beer’s Law equations can be written, one for the trial (Aeq = ε[FeNCS2+]eql), one...

Chemistry
Yes i think this was a trick question, the solid just needs to be completely ignored. This question isn't part of a database unfortunately, just a practice question for exam

Chemistry
Another Equilibrium Question! The following reaction is at equilibrium in a closed 20.0-L container. At equilibrium, the pressures of NH3 and HCl are both equal to 0.00552 atm, and the mass of NH4Cl (s) is 35.4 g. Calculate the equilibrium pressure of NH3 after 11.3 g of NH4Cl...

Chemistry Equilibrium Constant
Nevermind I got it, with x = 0.099999 then I just use what I have in the ICE chart and plug it in to solve for Kp, Thanks for all the help!

Chemistry Equilibrium Constant
Hmm I'm still confused at what to plug in for pHI^2 and pH2 for solving Kp

Chemistry Equilibrium Constant
Or do I solve for x, using the given pressure of I2 at equilibrium, so should it be 1E-5 = 0.1 - x? (solve for x)

Chemistry Equilibrium Constant
So instead of using 0.1 for I2, I want to use 1E-5 for I2 when solving for KP?

Chemistry Equilibrium Constant
The reaction is I2(g) + H2(g) -> 2HI(g)

Chemistry Equilibrium Constant
The initial pressures for I2 (g), H2(g), and HI(g) were Pi2 = 0.100 atm, Ph2 = 0.200 atm, and Phi = 0 atm, respectively. After the system came to equilibrium, the pressure of I2 (g) became very low, PI2 = 1.00 x 10^-5 atm. Calculate the equilibrium constant Kp for this reaction

Chemistry
The equilibrium constant Kc for the following reaction is equal to 0.20 at 250°C. Calculate the equilibrium constant Kp for the reverse reaction at the same temperature. COCl2 (g) = CO (g) + Cl2 (g) My Answer: To find the reverse reaction of Kc, it should be 1/0.2 = 5, so ...

chemistry
Nevermind this was answered here jiskha com/display.cgi?id=1332104707

chemistry
The Equilibrium Constant Kp for the following reaction is 4atm^2 at 300K. AB(s) -> A(g) + B(g) What is the equilibrium pressure of A(g) and B(g) above AB(s) at 300K? What is Kc at 300K?

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