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April 20, 2014

Search: If the KC at this temperature is 1.7x10^2, what is the equilibrium concentration of N2 ?

Number of results: 1,027

CHEMISTRY
If an explanation for correct answer could be provided, that would be great! Which equilibrium constant indicates that the reaction will produce mostly products? a. Kc = 3.46x10-6 b. Kc = 1.96x10+7 c. Kc = 0.319 d. Kc = 0.37
Sunday, April 6, 2014 at 11:41am by Chemistry

chemistry check my work
Of course you realize you can't control the spacing on the board; therefore, you must time everything as a line format. When taking 1/2 the equation, Kc becomes the sqrt Kc. When reversing, Kc becomes 1/Kc.
Wednesday, April 14, 2010 at 10:02pm by DrBob222

Chemistry
Kp=Kc(RT)^delta(N) .25=Kc(.08206*1100)^(2-3) .25=Kc(90.27)^-1 .25=Kc 1.108*10^-2 divide both sides by 1.108*10^-2 22.6=Kc it may be off a bit because i didnt account for significant figures
Tuesday, July 31, 2007 at 2:00pm by sammy

Chemistry
This must be a multipart question sincer the Kc data for HCl is not relevant. You have 2ICl ==> I2 + Cl2 and you want the reverse of that. Just take the reciprocal of Kc for the forward rxn or Kc reverse = 1/Kc forward
Thursday, March 13, 2014 at 2:37am by DrBob222

Chemistry
Kc = (NO)^2/(N2)(O2) Substitute the values from the problem into the Kc expression and solve for Kc. It's that simple.
Wednesday, April 27, 2011 at 10:14pm by DrBob222

Chemistry
For the question about the 2, no everything would stay the same. And you can see why with the answer to th second question. Let's look at it the other way. NH4HS(s) ==> NH3(g) + H2S(g) Then Kc = products/reactants and (NH3)(H2S) = Kc. Since NH4HS is a solid, by definition ...
Sunday, March 18, 2012 at 5:07pm by DrBob222

CHEM
Do you want Kc? That is Kp = Kc(RT)^delta n. Substitute and solve for Kc.
Sunday, January 8, 2012 at 3:36pm by DrBob222

Chem
Write the equation. Write the expression for Kc. Substitute into Kc and calculate the reaction quotient, Q. Compare that with Kc. If Q<Kc, it means the numerator is too small, the denominator is too large, and the reaction will go to the right. If Q>Kc, it means the ...
Monday, March 22, 2010 at 10:24pm by DrBob222

Chem Check
Consider the following gas phase reaction: 3A(g)+ 2B(g) <==> 1C(g)+4D(g). At 181.1C, Kp=270.91. Calculate Kc under these conditions. My answer: change of n = (1+4)-(3+2)=0 kp=kc(RT)^(change of of n) 207.91=kc(.0821)(454.1)^0 Therefore, kc=270.91 Is this correct? yes, Kp=...
Friday, February 9, 2007 at 9:13am by Marisol

chemistry
Given Kc values: N2(g)+1/2 O2(g)<->N2O(g) Kc=2.7* 10^-18 N2O4(g)<->2NO2(g) Kc=4.6*10^-3 1/2N2(g)+O2(g)<->NO2(g) kc=4.1*10^-9 What is the Kc value for: 2N2O(g)+3O2(g)<->2N2O4(g)
Monday, February 9, 2009 at 4:41pm by Juliet

Chemistry
Which statement about Kc is wrong? A. Kc is always a constant B. For some reactions, Kc increases with temperature increase C. For some reactions, Kc decreases with temperature decrease D. For some reactions, Kc changes when pressure is changed A is incorrect. Kc stays ...
Wednesday, January 31, 2007 at 12:40pm by Joe

Chemistry
Write the Kc expression. Set up an ICE chart. Plug into Kc expression and solve for Kc.
Thursday, March 4, 2010 at 6:19pm by DrBob222

Chemistry(Please check)
The equilibrium constant, Kc for the system, CaO(s) + CO2(g) == CaCO3(s), is A. Kc = (CaO) (CO2) / (CaCO3) B. Kc = (CO2) C. Kc = (CaCO3)/(CaO) D. Kc = (CaCO3) / (CaO) (CO2) E. Kc = 1 / (CO2) My answer is (CaCo3) / (CaO)(CO2). Would you agree?
Saturday, March 3, 2012 at 10:04pm by Hannah

AP CHEMISTRY
Kc=[PH3][BCl3] since those are both equal concentratons, then x^2=Kc x= sqrt Kc b. mass of PH3+massBCl3=2xVolume=2*.450*sqrtKc
Monday, February 6, 2012 at 7:12pm by bobpursley

Chemistry
I would first convert Kp to Kc using Kp = Kc(RT)^delta n, then see your next post to adjust for the equation. It appears to me to be reversed and 1/2; therefore, K'c = 1/(sqrt Kc).
Saturday, May 28, 2011 at 2:32pm by DrBob222

AP Chemistry
Given: 2N2(g) +O(2) --> 2N2O(g) Kc =1.2x10^(-35) N2O4(g) --> 2NO2(g) Kc = 4.6x10^(-3) 1/2N2(g) + O2(g) --> NO2(g) Kc= 4.1x10^(-9) Calculate Kc for the reaction between one mole of dinitrogen oxide gas and oxygen gas to give nitrogen tetroxide gas.
Wednesday, August 17, 2011 at 10:00pm by Matt

Chemistry
equation 1--reverse it and take 1/2. Then Kc for the new rxn is 1/sqrt Kc = k1 equation 2--reverse it. Kc for new reaction is 1/Kc = k2. Add the two new equations to obtain the desired equation. Kc for the new equation is k1*k2.
Wednesday, February 29, 2012 at 9:21am by DrBob222

Chemistry(Please help, thank you!)
Using this data, 2 NO(g) + Cl2(g) == 2 NOCl(g) Kc = 3.20 X 10-3 NO2(g) == NO(g) + O2(g) Kc = 3.93 calculate a value for Kc for the reaction, NOCl (g) + O2 (g) == NO2 (g) + Cl2 (g) I do not understnad how I am suppose to use the Kc values given if they give you a new ...
Wednesday, March 14, 2012 at 9:04pm by Hannah

CHEMISTRY
Method for getting correct answer? Thank you! Initially there were equilibrium concentrations of 0.1887 M A, 0.1042 M B. Which of the equations below is correct if the pressure decreased by a factor of 2.40? Use the reaction below. 6A(g) ↔ 5 B(g) Qc = 0.42 Kc Qc = 0.45 ...
Sunday, April 6, 2014 at 12:11pm by Chemistry

CHEMISTRY
Method for getting correct answer? Thank you! Initially there were equilibrium concentrations of 0.1887 M A, 0.1042 M B. Which of the equations below is correct if the pressure decreased by a factor of 2.40? Use the reaction below. 6A(g) ↔ 5 B(g) a. Qc = 0.42 Kc b. Qc = ...
Sunday, April 6, 2014 at 3:43pm by Chemistry

chemistry
Given the equilibrium constant values: N2 + 1/2O2 >>> N2O ; kc = 2.7 * 10^-18 N2O4>>>>2NO2 kc=4.6*10^-3 1/2N2 + O2>>>NO2 kc = 4.1 * 10^-9 What is a value of Kc for this reaction? 2N2O + 3O2 >>> 2N2O4
Wednesday, March 10, 2010 at 3:48am by abe

Chemistry
I'm not sure I follow your thinking. Kp = Kc(RT)^dn Kc = Kp(RT)^dn Kc = 1.2E-2(0.08205*1338)^(3-2) Kc = 1.2E-2(o.08205*1338) = ?? Then K'c = (1/sqrt Kc)
Saturday, May 28, 2011 at 2:32pm by DrBob222

Ap Chem
Why is it possible for Kp to be less than Kc? If this is the case then when Kc>1 it favors products, but if Kp <1 than how can that reaction favor products? Or does that rule only apply for Kc
Sunday, October 9, 2011 at 10:11am by Jane

Ap Chem
Why is it possible for Kp to be less than Kc? If this is the case then when Kc>1 it favors products, but if Kp <1 than how can that reaction favor products? Or does that rule only apply for Kc
Sunday, October 9, 2011 at 10:47am by Jane

chemistry
Kc = (right side)/(left side) with coefficients as exponents. Kc = (CO)^2(O2)/(CO2)^2 Plug in values and calculate. If k is >1, products favored. If Kc<1, reactants favored.
Friday, March 2, 2012 at 6:50pm by DrBob222

chem
I need to know exactly what your problem is in working this. Part a is just a matter of plugging into the Kc expression and solve for Kc. Part b appears to me nothing more than adding 1.5 to the I2 equilibrium amount and recalculating Kc (which would now be called Q).
Monday, November 19, 2012 at 12:26pm by DrBob222

CHEM
How are the forward and reverse rate constants for a one-step reaction related to the equilibrium constant for the reaction? A)Kc = kf x kr B) Kc = kf - kr C) Kc = kf + kr D) Kc = kf/kr
Saturday, May 29, 2010 at 4:53pm by Adam

Chemistry
Kp = Kc(RT)^delta n. delta n = product mols - reactant mols = 4-2 = 2 7.7E24 = Kc(0.08206*298)^2 Kc = ?
Tuesday, December 10, 2013 at 4:06am by DrBob222

College Chemistry Help Asap!
Determine the values of Kp that correspond to the following values of Kc a)CO(g) + Cl2(g) <===> COCl2(g) Kc= 1.2 x 10^3 at 668 K b)2 NO(g)+ Br2(g)<===> 2 NOBr(g) Kc= 1.32 x 10^-2 at 1000 K c) 2 COF2(g)<===> CO2(g)+ CF4(g) Kc= 2.00 at 1000 degrees Celsius
Monday, November 15, 2010 at 9:53am by shanice

Chemistry
The reaction, 2 SO3(g) == 2 SO2(g) + O2(g) is endothermic. Predict what will happen if the temperature is increased. A. the pressure decreases B. more SO3(g) is produced C. Kc increases D. Kc decreases E. none of the above I chose that Kc will increase. Would you agree?
Saturday, March 3, 2012 at 10:11pm by Hannah

Chemistry....Please help
Given the equilibrium constant values: 1.N2(g)+ 1/2O2(g)<---> N2O(g) KC=2.7*10^{-18} 2.N2O4(g)<----> 2NO2(g) KC= 4.6*10^{-3} 3. 1/2N2(g)+ O2(g)<----> NO2(g) KC=4.1*10^{-9} ----------------------------- 2N2O(g)+ 3O2 (g) <----> 2N2O4(g) I need help i dunt...
Sunday, February 8, 2009 at 3:29pm by Saira

Chemistry
As an environmental chemist, you want to find the Kc for the following reaction: 2 NO2 (g) ⇌ N2 (g) + O2 (g) Kc = ? Use the following data to find the unknown Kc : N2(g) + O2(g) ⇌ NO (g) Kc = 4.8 x 10-10 2 NO2(g) ⇌ 2 NO (g) + O2 (g) Kc = 1.1 x 10-5
Thursday, February 9, 2012 at 6:18pm by Daniel

Chemistry
Kc = (CO)^2(O2)/(CO2)^2 Convert grams given to moles. moles = grams/molar mass. Convert to molarity from moles/5.0, then substitute into the Kc expression above and calculate Kc.
Sunday, February 27, 2011 at 11:52pm by DrBob222

Chemistry(Please respond, thank you!)
Using this data, 2 NO(g) + Cl2(g) == 2 NOCl(g) Kc = 3.20 X 10-3 NO2(g) == NO(g) + O2(g) Kc = 3.93 calculate a value for Kc for the reaction, NOCl (g) + O2 (g) == NO2 (g) + Cl2 (g) So I understand that 2NO + Cl2 + 1/2O2 = NO2 + 1/2 Cl2 but I do not understand how you use ...
Thursday, March 15, 2012 at 1:54pm by Hannah

Chem II
Yes, I can explain. Both of us made the same mistake and I wouldn't have noticed it if you hadn't reposted. Reread the question. It is NOT (as I first read it) Kp = Kc (Look at my first response and you can see I am always talking about equal). The question reads Kp < Kc. ...
Wednesday, June 25, 2008 at 1:43pm by DrBob222

College Chemistry 2 - Equilibrium Constants/Conc.
I think you read your calculator wrong for CH3OH. I have 7.79E-4. Also I assume K is Kc and not Kp. .................2H2 + CO ==> CH3OH You don't need the "change in concn". Kc = (CH3OH)/(H2)^2(CO) You have Kc, C3OH and H2, solve for CO.
Friday, March 4, 2011 at 7:56pm by DrBob222

Chemistry
Write the Kc expression, substitute the numbers given and solve for Kc.
Wednesday, March 21, 2012 at 9:46pm by DrBob222

Chemistry
A ==> 2B Kc = (B)^2/(A) Kc = (0.154)^2/(0.381) You do the math.
Tuesday, November 29, 2011 at 8:15pm by DrBob222

Chemistry
Do you want Kp or Kc. You can calculate Kc without changing to atm.
Wednesday, February 27, 2013 at 8:45pm by DrBo222

Chemistry
Kc = (PCl3)(Cl2)/(PCl5) = 4.2 x 10^-2 With Kc equal to less than 1, that means that the numerator is smaller than the denominator and that means the reactants will be larger than the products. A second reason, and you need to Kc value, all materials are gaseous and the side ...
Saturday, February 27, 2010 at 9:16am by DrBob222

chemistry
what is Kc for 2NOBr-->2NO+Br2 when the temperature is 1000K and the Kc is 1.3x10^-2
Sunday, February 26, 2012 at 8:15pm by Anonymous

Chemistry
Kp = Kc (RT) (exponent = (2+1)-2) 0.700 = Kc (R * 319) not sure what R is or how to figure it out????
Sunday, November 27, 2011 at 4:14pm by Tina

Chemistry
If Kc = 0.480 at 40.C and Kc = 0.630 at 90.C, what is ΔH for the reaction? X<---->Y
Saturday, March 10, 2012 at 12:35am by Andrew

Chemistry
Kc is not 0.379. I thought we went over this. You had Kc right at the beginning as 0.514.
Tuesday, February 5, 2013 at 10:56pm by DrBob222

chem 2
Kp = Kc*(RT)^delta n where dn = nproducts-nreactants Substitute and solve for Kc.
Sunday, October 6, 2013 at 1:58am by DrBob222

Chemistry
And this one too! I thought it should also have a Kc expression but my notes only mentioned the Kp expression: ( that weird arrow is the forward backward arrow for a reversible reaction) H2(g) + Br2(l) --><-- 2HBr2(g) Kc = [HBr]^2 / [Br][H2] Please tell me if im right! I...
Friday, September 10, 2010 at 3:12am by Riley

chemistry
If you want Kp is it Kp = (PCl5)/(PCl3)(Cl2) Substitute and solve for Kp. I assume Keq is Kc although I don't know that. You can convert Kp to Kc by Kp = Kc(RT)delta n</sup) where delta n = #n products- #n reactants = 1-2 = -1
Wednesday, October 19, 2011 at 3:23pm by DrBob222

chemistry
You don't say if 2.0 x 10^-8 is Kp or Kc. Your balanced equation is ok but thereafter is not. 2CO2 ==> 2CO + O2 If the K you omitted is Kc, then, initial: (CO2) = 2.0 (CO)=0 (O2)=0 change: (CO) = +x (O2) = +x (CO2) = -2x equilibrium: (CO) = +x (O2) = +x (CO2) = 2.0 - 2x Now...
Sunday, March 1, 2009 at 8:41pm by DrBob222

chemistry
............H2 + I2 ==> 2HI Equil......4.4..3.2....1.5 Substitute into Kc expression and solve for kc.
Saturday, May 5, 2012 at 4:28pm by DrBob222

Chemistry
I have Kc= [(0.065)(0.130)^2]/(0.190^2) Kc= 0.030429 This answer was incorrect. Can you please help correct me?
Friday, March 8, 2013 at 10:35pm by Joseph

CHEMISTRY
0.00436 is close but not quite correct. To prove that substitute back into the Kc expression and see if you get 0.5. You don't. I think you obtain 0.55. I solved the cubic equation and obtained 0.003959 (which of course is too many significant figures) but if you substitute ...
Saturday, October 15, 2011 at 9:18pm by DrBob222

chemistry check my work
If this is the equation, 2NO + 2H2 --> N2 + 2H2O and H2O is a gas, then the Kc expression is (N2)(H2O)^2/(NO)^2(H2)^2. I think you had (H2) and not (H2)^2 If we take half the equation, we don't split the way we write molecules. It would look this way. 1/2 NO + H2 ==>1/2 ...
Wednesday, April 14, 2010 at 10:02pm by DrBob222

Chemistry
No and no. First, since the values quoted are equilibrium values, we need to calculate Kc (by the way, 80 is not an equilibrium value). ............N2 + O2 ==> 2NO equil.......0.1..0.1.....0.5 Kc = (NO)^2/(N2)(O2) Kc = (0.5)^2/(0.1)(0.1) Kc = 25 is what I have. Then we set ...
Monday, March 5, 2012 at 10:52pm by DrBob222

Chemistry
(x)/(.00125-x)(.00000025-x)=Kc How do I solve for x or Kc?
Sunday, February 28, 2010 at 8:43pm by Koo

Chemistry
Is the Kc you list as 0.120 Kp or Kc?
Monday, September 16, 2013 at 8:56pm by DrBob222

chemistry, plz check work
NH3+H2S-->NH4HS <-- Kc=400 at 35 Celsius what mass of NH4HS will be present at equilbrium? My work NH3 H2S NH4HS initial 2 mol 2 mol 2 mol change -x -x +x equilibrium 2-x 2-x 2+x Kc=[NH4HS]/[NH3][H2S] 400=(2+x)/[(2-x)(2-x)] 400=(2+x)/(4-4x+x^2) 1600-1600x+400x^2=2+x 1598...
Monday, March 2, 2009 at 1:26am by Anonymous

Chemistry
so for the Kc value it would change correct? I did this: Kc = [PCl3][Cl2]/[PCl5] = [0.30][0.12]/[0.72] = 0.05
Sunday, July 19, 2009 at 6:18pm by Lena

chem Help
Substitute the equilibrium concentrations into the Kc expression and solve for Kc. Use this below. ...........N2 + O2 ==> 2NO I.......0.200..0.200....0.800 C.........+x...+x.......-2x E.....0.200+x..0.200+x...0.800-2x Substitute the E line into Kc expression along with the ...
Tuesday, April 1, 2014 at 11:57am by DrBob222

Chemistry
Determine Kc for the following reaction: 1/2N2(g) + 1/2O2(g)+ 1/2Br(g) <-> NOBr(g) from the following information (at 298K) 2No(g) <-> N2(g) + O2(g) Kc = 2.1x10^30 NO(g) + 1/2Br2(g) <-> NOBr(g) Kc = 1.4
Wednesday, May 25, 2011 at 10:40pm by K

Chemistry II
Kc=(x)(x)/(1-x)(1-x) What is x in this equation and is is 4.0 Kc?
Sunday, April 11, 2010 at 6:11pm by curtis

Chemistry(Please help)
First you need to work on the Kp expression. SOLIDS aren't used (pure liquids aren't either) so the expression is 1/pCO2 = Kp. The problem tells you that AT EQUILIBRIUM [CO2] = 0.150M. I would calculate Kc from Kc = 1/([CO2] then convert to Kp by Kp = Kc(RT)Dn
Wednesday, March 14, 2012 at 9:51pm by DrBob222

Chem II
You look at the equation for converting Kp to Kc (or Kc to Kp). One of them is as follows: Kp = Kc(RT)delta n Therefore, the ONLY difference between Kp and Kc is the (RT)^delta n part. So if delta n is zero; i.e., the same number of mols on each side, then delta n = 0, any ...
Wednesday, June 25, 2008 at 1:43pm by DrBob222

Chemistry
I need to calculate the valueof Kc for 5 test tubes for an experiment that I completed on determination of Kc. The equation used was Fe^3+ + SCN^-= FeSCN^2+ After creating an ice table for the first test tube my values for Fe and SCN were 6.5e-4M and for FeSCN I got 5.7e-5M. ...
Tuesday, March 6, 2012 at 3:16pm by Hannah

Chemistry
Is this Kc or Kp = 0.12? I will assume it is Kc. What is the reaction for K. I will assume it is cyclohexane ==> methyl cyclopentane K = 0.12 = (mcyp)/(cyh) Set up an ICE chart. ...........mcyh ==> mcyp initial....0.036....0 change.....-x.......x equil.....0.036-x...x ...
Tuesday, May 24, 2011 at 2:33pm by DrBob222

Chemistry(Please check)
I need to calculate the valueof Kc for 5 test tubes for an experiment that I completed on determination of Kc. The equation used was Fe^3+ + SCN^-= FeSCN^2+ After creating an ice table for the first test tube my values for Fe and SCN were 6.5e-4M and for FeSCN I got 5.7e-5M. ...
Tuesday, March 6, 2012 at 12:27pm by Hannah

Chemistry
Yeah I did all the previous things to find Kc and I got kc = 0.012. But you know how for to get the other kc you said I would have to do 1/sqrt Kc, I know that I would do that because the product is H2S and I would do the inverse because it is reversed and I would sqrt because...
Saturday, May 28, 2011 at 2:32pm by K

Chemistry - Kc question
What would happen to Kc values in an experiment if the Beer's law constance (k) value used was low ( e.g you used 4000/M when the actual constant had a value of 5000/M)? Explain your answer Absorbance = k*length cell*concentration Cell length is constant. You read an ...
Sunday, August 5, 2007 at 2:09pm by matt

Chem II
No, looking at wrong page in homework, on this problem, I subbed everything into the Kp=Kc(RT)delta n, and then tried to isloate Kc, but I don't think I am right
Wednesday, June 25, 2008 at 1:46pm by Ken

Chemistry
...........N2 + O2 ==> 2NO E.........0.1....0.1....0.4 add 0.3.................0.7 new I.....0.1....0.1....0.7 C..........+x......+x....-2x new E....0.1+x..0.1+x...0.7-2x Use the first E line to calculate Kc. Substitute the equilibrium conditions and solve for kc. Then ...
Sunday, February 17, 2013 at 2:49pm by DrBob222

Chem 2
First Kc must determined. .........N2O4 ==> 2NO2 Kc = (NO2)^2/(N2O4). Substitute the equilibrium numbers and solve for Kc. Then set up an ICE cart for the remainder of the problem. ............NO2 ==> 2NO2 initial....0.55......0.25 add....................0.1 change...
Monday, March 5, 2012 at 7:58pm by DrBob222

Chemistry
Frankly I don't know how to answer the question. Is this Kc or is it Kp? The problem calls it Keq and gives moles. Moles can't go in the Keq expression. It must be molarity for Kc or partial pressure for Kp. With no volume given mols can't be converted to M nor to pressure. Is...
Sunday, April 8, 2012 at 4:50pm by DrBob222

Chemistry
What do you mean you don't know where to start. This is just a case of substitute and solve. 7.7E24 = Kc(0.08205*298)^(4-2) Solve for Kc.
Wednesday, April 16, 2014 at 12:52am by DrBob222

Chemistry
Write the expression for Kc. Kc = (Ag^+)^2(OH^-)^2 Substitute H^+ for a pH of 10.50 and solve for (Ag^+)
Monday, October 25, 2010 at 2:15pm by DrBob222

Chemistry Help
For the first Kc I got .514 For the second Kc I got .129. How do I find the mols afterwards?
Tuesday, February 5, 2013 at 9:07pm by Anon

chemistry
Using this data, 2 NO(g) + Cl2(g) == 2 NOCl(g) Kc = 3.20 X 10-3 NO2(g) == NO(g) + O2(g) Kc = 3.93 calculate a value for Kc for the reaction, NOCl (g) + O2 (g) == NO2 (g) + Cl2 (g) A. 20.2 B. 2.06 X 10-4 C. 4.49 D. 4.84 X 10-3 E. 0.223 eliminated down to b or d but going ...
Monday, March 12, 2012 at 5:34pm by bob

Chemie
the equilibrium constant is the ratio of the concentration product of the product and the reactant of a particular reaction. i.e. Kc = [NH4+]/[NH3][H+] where Kc is 4.5e8.
Sunday, June 16, 2013 at 12:06am by bonjo

AP CHEM!
I'm not so sure about E, but if you do the ICE chart, and equate Kc to 5, you can solve by plugging in the values of your Equilibrium concentrations into your Kc equation(again, refer to b). My answer is 0.118M CO, but I could be wrong.
Tuesday, April 3, 2007 at 10:07pm by Not Sure

Chemistry
If Kc = 0.450 at 40 degrees C and Kc = 0.545 at 90 C, what is the delta H for the reaction? X <---> Y ____ kJ would this problem include using a van hoff factor..?
Tuesday, March 6, 2012 at 5:13pm by Eric

Chemistry
First, convert mols to M. (HI) = 7/10 = 0.7M (I2) = 1/10 = 0.1M (H2) = 1/10 = 0.1M Next calculate the Kc. 2HI ==>H2 + I2 Kc = (H2)(I2)/(HI)^2 Kc = (0.1)(0.1)/(0.7)^2 = approx 0.02 Then do and ICE chart. ............2HI ==> H2 + I2 I...........0.7....0.1...0.1 add...
Wednesday, April 16, 2014 at 4:49pm by DrBob222

Chemistry
There is only one Kc; that is 0.514. If you plug in (0.6)(0.6)/(1.4) you get 0.257 = the reaction quotient. That is smaller than Kc which means the reaction will shift to the right to re-establish equilibrium. I have set up the ICE chart for that equilibrium also. Kc = 0.514...
Tuesday, February 5, 2013 at 9:07pm by DrBob222

Chemistry
Given the general equation: 3x +4y <-> 2x, kc= 4.5 E-5 a. What is the kp? b. What does Kc equal for 2xy <-> 3x + 4y? c. What does Kc equal for 6xy <-> 9x +12y?
Sunday, October 2, 2011 at 8:23pm by Anonymous

chemistry
No negatives are involved. When reversing Keq, it is k' = 1/Keq. My instruction was that k1 = 1/sqrt Kc. You took 1/2 of it; that's to get the coefficients right when you add one equation to the other but k1 = 1/sqrt Kc. [When taking 1/2 of an equation, k1 is sqrt Kc. Then ...
Monday, March 12, 2012 at 9:10pm by DrBob222

Chemistry
If that is an all gaseous reaction the expression you wrote is correct However, if Si and SiO2 are solids, then Kc = 1/(O2) since the solids are not included in the Kc.
Tuesday, May 7, 2013 at 11:31am by DrBob222

Chemistry
delta Gorxn = (n*DGoproducts)-(DGoreactants), then delta Go = -RT*lnKp. I would then convert this to Kc by Kp = Kc(RT)delta n I don't know what you mean by (e). .............2NO2 ==> N2O4 initial......1 mol.....0 change......-2x........x equil........1-2x.......x Kc = (N2O4...
Thursday, October 20, 2011 at 8:53pm by DrBob222

Chem
(S2) = 11.0mols/5.20L = approx 2 but you need to be more accurate. .........S2 + C ==> CS2 I mols...2..xs...0 C.......-x..xs...x E......2-x..xs...x Kc = (CS2)/(S2) note:C doesn't appear in the Kc exprssion because it is a solid. Substitute the E line into Kc expression and ...
Monday, February 10, 2014 at 9:55pm by DrBob222

chemistry. please help!!!
Kc =[ Fe+3] / [Fe+2][Ag+] You must be given the equilibrium constant or have access to enough information to calculated it. Since you have the initial concentrations of Fe^+2, Ag^+ and Fe^+3 with a known Kc, you can set up a table of data leadinf to an equation for changes in...
Thursday, March 26, 2009 at 11:51pm by GK

Chemistry
I converted Kp to Kc also but didn't arrive at the same answer. I think your Kc = Kp(RT)^-delta n is correct. But delta n is 1-2 = -1 so Kc = Kp(RT)^(-)(-1). and that makes Kc about 25. Check me out on that. (Z)/(X)(Y) and Q = 1 which is too small so the reaction will shift to...
Monday, March 5, 2012 at 10:03pm by DrBob222

Chemistry
Kp = Kc(RT)n(prod)-n(react) Substitute and solve for Kc. I have estimated the answer at about 0.03. Post your work if you get stuck.
Sunday, November 27, 2011 at 4:14pm by DrBob222

chemistry
Do you have a constant for toluene? (Henry's Law constant?) p = Kc*C p/Kc = C
Tuesday, June 5, 2012 at 2:04pm by DrBob222

Chemistry
a. mols H2S = grams/molar mass = 3.40/34 = 0.1 Surely I don't need to write the Kc expression for you. b. ..........2H2S ==> 2H2 + S2 initial..0.1........0.....0 change....2x.......2x.....x equil...0.1-2x.....2x.....x From the problem, (S2) = x = 0.0372. Therefore, (H2) is ...
Monday, April 9, 2012 at 8:58pm by DrBob222

Chemistry
At 1100 K, Kp=0.25 for the following reaction. 2SO2(g) + O2(g) (reversible arrows) 2SO3(g) What is the value of K at this temperature? Do you mean what is the value of Kc? If so, use the Kp to Kc conversion formula. What is the Kp to Kc conversion formula? We were never given ...
Monday, July 30, 2007 at 7:37pm by Taasha

AP Chemistry
I would like to know if this is Kc or Kp. I will assume Kc and you want to know the x of 1-x although that's a funny way of asking. Perhaps I've misinterpreted the question. ........F2 ==> 2F I......1.00.....0 C......-x.......2x E.....1-x......2x
Tuesday, November 26, 2013 at 8:16pm by DrBob222

chemistry...Please Help
I posted this below and received help but im still lost and worked out the problem but am getting the wring answer: -------------------- Given the equilibrium constant values: 1.N2(g)+ 1/2O2(g)<---> N2O(g) KC=2.7*10^{-18} 2.N2O4(g)<----> 2NO2(g) KC= 4.6*10^{-3} 3. ...
Monday, February 9, 2009 at 6:39pm by Saira

chemistry
Kc = cocns products/concns reactants Raise each to power of the coefficients. Kp is same except partial pressure instead of concn. Solids are not included in either Kc or Kp.
Thursday, March 8, 2012 at 3:45pm by DrBob222

Chemistry
I have made mistakes like that but in this case I didn't. It could be either way. Which ever way you do it will work out. If you assume you started with HI, then 2HI ==> H2 + I2 and the EQUILIBRIUM MIXTURE will be as given. Then you work out Kc for that reaction. You add ...
Wednesday, April 16, 2014 at 4:49pm by DrBob222

College Chemistry Lab
For the first one, Absorbance = kc A = 0.585, solve for k, c =- 2.50 x 10^-6M Use k in the second run of the concd stuff. A = kc You will get a concn that must be adjusted because of the dilution. How much was it diluted. From 5 to 150 mL; therefore, the concn will whatever ...
Tuesday, March 16, 2010 at 7:29pm by DrBob222

Chemistry
I'm doing chemical equilibrium, and there's a question in my lecture notes. Can someone check my answers and tell me if i'm right or wrong? Thanks! The Kc expression for this reversible reaction: 3Fe(s) + 4H2O (g) --><-- Fe3O4(s) + 4H2 (g) is [H2]^4 / [H2O]^4 Am I ...
Friday, September 10, 2010 at 3:12am by Riley

Chemistry
Calculate Kc. CH_4(g) + H_2O(g) <-> CO(g) + 3H_2(g) Kp= 7.7 x 10^24 at 298K. Should I use the formula Kp= Kc(RT)^Deltang If so I have no idea where to start.
Wednesday, April 16, 2014 at 12:52am by Savannah

Chemistry Honors
I assume that is a 2.0L container but you omitted the unit. M NH3 = mols/L = 12.0/2.0 = 6.0M ........2NH3 ==> N2 + 3H2 I......6.0.......0.....0 C......-2x.......x.....3x E......6.0-2x....x.....3x Kc = (N2)(H2)^3/(NH3)^2 The problems tells you H2 at equil is 6.0mols; ...
Saturday, July 20, 2013 at 5:20pm by DrBob222

Chemistry
The equilibrium constant Kc for the following reaction is equal to 0.20 at 250C. 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 the ...
Sunday, March 18, 2012 at 10:16pm by Raskin

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