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April 19, 2014

Search: Chemistry - Kp

Number of results: 101,184

Chemistry
The problem gives you the Kp at 400 C. We presume the reaction is at the same temperature as Kp is given Kp = pNH3*pHI NH4I(s) ==> NH3(g) + HI(g) ..............p.......p Substitute p into Kp expression and solve for p.
Thursday, March 8, 2012 at 7:42pm by DrBob222

Chemistry
I think you are missing the boat. Kp for 2NO + O2 ==> 2NO2 Kp = 1.48E3 You want Kp for 2NO2 ==> 2NO which is just the reverse of the original equation. For that the new Kp = 1/old Kp (i.e., just the reciprocal of old Kp).
Tuesday, March 9, 2010 at 5:06pm by DrBob222

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
Kp = pNH3*pH2S Substitute partial pressures and solve for Kp. Then convert Kp to kc by Kp = Kc*RTdelta n
Tuesday, February 19, 2013 at 1:34pm by DrBob222

chemistry
It's easier than it looks on the surface. Let's call Kp = 3.5 x 10^4 the original Kp. The second equation is just 1/2 of the first one; therefore, new Kp = (original Kp)1/2. If you had 2N2 + 6H2 <==> 4NH3, then new Kp = (original Kp)2 . In other words, just raise the ...
Thursday, November 29, 2007 at 5:30pm by DrBob222

Chemistry
Nitrogen dioxide, a pollutant in the atmosphere, can combine with water to from nitric acid. One of the possible reactions is shown below. Calculate ∆G0 and Kp for this reaction at 25oC and comment of on the spontaneity of the reaction (MUST plot the data and find ...
Thursday, April 18, 2013 at 11:02am by Yasemine

College Chemistry
Determine the values of Kc that correspond to the following values of Kp (a) SO2Cl2(g)--->SO2(g) + Cl2(g) Kp= 2.9 x 10^-2 at 303 K (b) 2 NO2 (g)--->2NO(g)+O2(g) Kp= 0.275 at 700 K (c)CO(g) + Cl2(g)---> COCl2(g) Kp= 22.5 at 395 degree Celsius
Wednesday, October 27, 2010 at 3:30pm by Shanice

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

Chemistry
At 389K, this reaction has a Kc value of 0.0682. 2X(g) + 2Y(g) <-> Z(g) .. Calculate Kp at 389K. Kp= this is what I did.. can somebody confirm or find any mistakes in my thought process? Kp = Kc(R)(T)^Delta n Delta n = (1)-(2+2) = -3 Kp = (0.0682)(0.08206)(398K)^-3 = 0....
Monday, March 5, 2012 at 8:35pm by Tracy

Chemistry
Kp = 4 AB(s) ==> A(g) + B(g) Kp = pA*pB If we let p = partial pressure of A, p also will be the partial pressure of B; therefore, p*p = Kp. Solve for p.
Saturday, March 17, 2012 at 7:10pm by DrBob222

Chemistry
Kp = pO2^1/2 Plug in you value of Kp and solve for pO2.Wouldn't pO2 = (Kp)^2
Friday, July 12, 2013 at 1:03pm by DrBob222

Chemistry(Please respond, thank you!)
For the system CaO(s) + CO2(g) = CaCO3(s), I added 1.00 mol of CaO(s) to 1.00L of 0.500M CO2(g) at 200 oC. At equilibrium the [CO2] = 0.150M. What is the value of Kp for this reaction? Kp would = CaCO3/(CaO)(CO2) I do not know what to do with the 0.500M and 1.00mol. Chemistry...
Thursday, March 15, 2012 at 1:02pm by Hannah

Chemistry
What is the value of Kp for the reaction: NO2(g)+CO(g)->NO(g)+CO2(g) Given the following information: 2NO2(g)->NO3(g)+NO(g) Kp=2.72x10^(-4) 2NO2(g)+2CO2(g)->2NO3(g)+2CO(g) Kp=5.73
Sunday, November 27, 2011 at 10:09pm by Tanya

Chem
Which direction will the following reaction in a 5.0 L flask proceed if Qp = 0.013? 2H2O(g) = 2H2(g) + O2(g) Kp = 1.6 x 10-5 Choose one answer. a. to the right because Q > Kp b. to the left because Q > Kp c. to the right because Q < Kp d. to the left because Q < Kp...
Wednesday, March 24, 2010 at 11:28pm by CC

Chemistry
Kp = pNH3*pH2S Then Kp = Kc(RT)^delta n
Friday, January 4, 2013 at 8:45pm by DrBob222

Chemistry
The K is just the equilibrium constant, not Kp. Do you have to convert the K to Kp?
Friday, February 14, 2014 at 3:25pm by Anonymous

Chemsitry
Nitrogen dioxide, a pollutant in the atmosphere, can combine with water to from nitric acid. One of the possible reactions is shown below. Calculate ∆G0 and Kp for this reaction at 25oC and comment of on the spontaneity of the reaction (MUST plot the data and find ...
Friday, April 19, 2013 at 11:32am by Yasemine

Chemistry
..........PCl5 ==> PCl3 + Cl2 I.........0.54......0......0 C..........-p.......p......p E.......0.54-p Ptotal = 0.85 = 0.54-p+p+p p = 0.31 atm. pPCl5 = 0.23 pPCl3 = 0.31 pCl2 = 0.31 Substitute these values into Kp expression and solve for Kp. Kp = Kc*RTdeltan . Substitute ...
Wednesday, February 13, 2013 at 7:09pm by DrBob222

Chemistry
What is included in the Kp expression - partial pressures of the components. The partial pressure of a solid does not change, so does not appear in Kp. This is the same with Kc as solids do not appear in Kc. Liquids do not appear in Kp either.
Friday, September 10, 2010 at 3:12am by Dr Russ

CHEMISTRY
Kp = 4 = partial pressure of A x partial pressure of B 4=p*p 4 = p^2 p=2 atm partial pressure A = 2 atm at eqilibrium. partial pressure of B = 2 atm at equilibrium. Kp = Kc(RT)delta n You know Kp and you know R and T. You can calculate delta n (it's mols reactants - moles ...
Sunday, March 18, 2012 at 5:05pm by DrBob222

Chemistry
MF17083:For the following reaction find Kp at 25°C and indicate whether Kp should increase or decrease as the temperature rises. NH4HS(s) <===> H2S(g) + NH3(g); DH° = 83.47 kJ and DG° = 17.5 kJ at 25°C. - A. B. C. D. E. F. Kp = - A. B. C. D. E. F. Kp ________ as the ...
Friday, April 27, 2007 at 12:52pm by Chris

Chemistry
The equilibrium constant for the reaction 2NO(g) + O2(g) <--> 2NO2(g) is Kp=1.48x10^4 at 184C. Calculate Kp for 2NO2(g) <--> 2NO(g) + O2(g). I know the equation is Kp=Kc(RT)x Delta n Kp is what we're solving for Kc= I can't seem to find. R=.0821 T=184+273 Delta n= ...
Tuesday, March 9, 2010 at 5:06pm by Anonymous

I don't know how to do this question, I understand we have to use ICE but I keep getting the wrong answer when I solve for x, it's just not working for me. Consider the following reaction: A(g) -> 2B (g) Find the equilibrium partial pressures of A and B for each of the ...
Friday, February 24, 2012 at 10:15pm by Student

Chemistry
Set up an ICE chart and substitute into the Kp expression, then solve for x. For converting Kp to Kc, look in your text or notes for the formula to do that.
Wednesday, March 24, 2010 at 9:03am by DrBob222

chemistry help!!!!!
Consider the following reaction: Find the equilibrium partial pressures of A and B for each of the following different values of Kp. Assume that the initial partial pressure of B in each case is 1.0 atm, and that the initial partial pressure of A is 0.0 atm. Make any ...
Sunday, March 11, 2012 at 9:57pm by student

Chemistry
At 319K the decomposition of dinitrogen tetroxide occurs with the following Kp: 2NO2(g)<>2NO(g)+O2(g) Kp=.700 What is the value of Kc for this reaction?
Sunday, November 27, 2011 at 4:14pm by Tina

chemistry
What's with the picture stuff? Just put an arrow there. NH4I(s) ==> NH3(g) + HI(g) .............p..........p Kp = pNH3*pHI = 0.215 (what? atm?) Substitute into Kp and solve for p.
Thursday, March 8, 2012 at 3:26pm by DrBob222

Chemistry/Equilibrium calculations
I noticed I rewrote the Kp as 1x10^-22 instead of 1x10^-13. Sorry. In the comparison of Kp with Qp for the reverse reaction we have: Kp=10^13 > Qp=10^5, leading to the conclusion that CO is still changing to CO2 as it escapes and its concentration decreases as I suggested ...
Saturday, August 16, 2008 at 7:59am by GK

Chemistry
Kc is uses concns. Kp uses atmospheres pressure. .......BrCl3(g) + Cl2(l) ==> BrCl5(g) I...0.215 atm......725g.......0.115 atm C......+x............+x..........-x E....0.215+x.................0.115-x Kp = pBrCl5/pBrCl3 Note that Cl2 is not included in Kp since it is not a gas.
Tuesday, October 2, 2012 at 11:17pm by DrBob222

Chemistry (Equilibrium)
Given the reaction below 2NOBr(g) <==> 2NO(g) + Br2(g) and the value of Kc = 1.98, at a temperature of 480 K what is the value of Kp ? (Hint: Use the value of R in the appropriate units.) I used the equation Kp=Kc(RT)^Delta N Then plugged in to get Kp=1.98(.0821x480k)^-1...
Friday, December 9, 2011 at 7:46pm by Summer

Chemistry - Kp
Kp = Kc(RT)^delta n. n = mols products - mols reactants = -2
Sunday, April 29, 2012 at 8:29pm by DrBob222

Chemistry
Yikes. Send me to the bottom of the class. The b part IS for Kp and Qp so that answer should stand. Convert Kp to Kc in #1. I don't agree with your answer.
Tuesday, February 5, 2013 at 10:57pm by DrBob222

Chemistry - help please
........NH4Cl(s) ==> NH3(g) + HCl(g) I......solid.........0.........0 C......solid.........p.........p E......solid.........p.........p Kp = pNH3*pHCl The problems tell you that pNH3 + pHCl = 4.4 atm and since pNH3 = pHCl that makes 2p = 4.4 and p = 2.2 atm Substitute into ...
Monday, October 14, 2013 at 4:35pm by DrBob222

Chemistry
Yes, delta n may be negative and in this instance you are right that it is -3. However, you have parentheses in the wrong place. The formula is Kp = Kc (RT)^delta n. Kp = 0.0628(0.08206*398)^-3
Monday, March 5, 2012 at 8:35pm by DrBob222

chemistry
My calculator is broken so I can't check your calculation; however, no the temperature is not being used EXCEPT that the value for Kp calculated is at 300 K and no other temperature. Kp and Kc change with T.
Wednesday, April 10, 2013 at 9:31am by DrBob222

Chemistry
I think it's your math. I obtained the same equation as you and it looks ok to me. I went through the math and obtained two values for x of 0.0631 (which can't be right since 0.110-2x gives a negative number) and 0.0471. That value plugged back into Kp expression gives Kp = 5....
Sunday, March 16, 2014 at 3:42pm by DrBob222

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

chm152
You still didn't say "of what" but I assume it is Kp after you filled in th remainder of the missing information. First you turned the reaction around. Let's designate the original Kp as Kp1. That makes the new Kp (which we will call Kp2) = 1/Kp1. THEN you divided all of the ...
Saturday, March 27, 2010 at 11:25am by DrBob222

chemistry
I can't tell what the value of Kp is. I will assume you meant it to be 2.91E-3. BTW, you need to learn where the arrow key is too. The arrow tells us where the reactants stop and the products begin. ......NH4OCONH2(s) ==> 2NH3 + CO2 I.......solid...........0.......0 C...
Monday, February 18, 2013 at 11:19pm by DrBob222

College Chemistry
The answer is just the reciprocal of the first Kp. So in your calculator type in 1/1.80e-2 and that will be your answer for the Kp of the second equation at the same temperature. The answer will be (in scientific notation): 5.56e1
Sunday, March 21, 2010 at 6:27pm by Katherine

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

Chemistry
I think you started out wrong. The problem gives as Kp and you are calculating, by mols/L, the concn. You put pressures in Kp and concns in Kc. ........2NF3 ==> N2+ 3F2 I......2.06mols...0....0 C.,.....-2x.... .x....3x E.....2.06-x......x....3x The problem tells you that x(...
Sunday, February 10, 2013 at 12:25pm by DrBob222

Chemistry
So basically for the first 3 answers (Part (A)(B)(C)): (A)and(B) - the concentrations would be equal since the mole ratio is equal and Q = K at equilibrium. (C) - the rate of both reactions would be equal also, as Q = k, right? (D)(1) - If the volume is increased at constant ...
Monday, April 25, 2011 at 11:04am by Molly

College Chemistry Help Asap!
Kp = Kc*R*Tdelta n where delta n = n(products)-n(reactants). Kp = 1.2E3*0.08206*(1-2) = ?? The others follow the same pattern.
Monday, November 15, 2010 at 9:53am by DrBob222

Chemistry - Kp
What is the Kp for the following reaction: 2NH3(g) --> N2(g) + 3H2(g) This reaction is contained in 1.0 L container at 1,000 K and has reached equilibrium. (Kc = 4.0 x 10^-2). You have initially added 1,220 moles of NH3(g) in the flask.
Sunday, April 29, 2012 at 8:00pm by Addyson

Chemistry - Kp
What is the Kp for the following reaction: 2NH3(g) --> N2(g) + 3H2(g) This reaction is contained in 1.0 L container at 1,000 K and has reached equilibrium. (Kc = 4.0 x 10^-2). You have initially added 1,220 moles of NH3(g) in the flask.
Sunday, April 29, 2012 at 8:29pm by Addyson

Chemistry
Kp=1.6 Kp=1.0*10^-4 A<->2B Find the equilibrium partial pressures of A and B B=1.0 atm A=0.0 atm This is what I have so far A 2B 0 1.0 +p -p p 1-p [B]^2/A (1-p)^2/p = 1.6 then got a quadratic equation of p^2+1.6p-1 to get x=.48
Monday, March 12, 2012 at 11:19pm by maura

Chemistry
Kp=1.6 Kp=1.0*10^-4 A<->2B Find the equilibrium partial pressures of A and B B=1.0 atm A=0.0 atm This is what I have so far A 2B 0 1.0 +p -p p 1-p [B]^2/A (1-p)^2/p = 1.6 then got a quadratic equation of p^2+1.6p-1 to get x=.48
Monday, March 12, 2012 at 11:20pm by maura

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
C(g) + CO2(g) ==> CO(g) Kp = 1.72 = pCO/pCO2 I would set up an ICE chart where p = pressure of CO and 4.70 = pressure CO2 at equilibrium. Substitute into Kp expression and solve for p.
Monday, October 3, 2011 at 9:08pm by DrBob222

chemistry
Calculate Kp at 298 K and 490 K for the reaction NO(g) + 1/2 O2(g) = NO2(g) assuming that Delta H(g) is constant over the interval 298 K - 600 K. Do you expect Kp to increase or decrease as the temperature is increased to 600 K?
Sunday, April 7, 2013 at 5:49pm by hayley

chemistry
Calculate Kp at 298 K and 490 K for the reaction NO(g) + 1/2 O2(g) = NO2(g) assuming that Delta H(g) is constant over the interval 298 K - 600 K. Do you expect Kp to increase or decrease as the temperature is increased to 600 K?
Sunday, April 7, 2013 at 5:49pm by ahsang

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 the ...
Sunday, March 18, 2012 at 10:16pm by Raskin

Chemsitry
..........A ==> 2B + 3C I.........10.....0.....0 C.........-x.....2x...3x E........10-x....2x...3x Ptotal = 12.13 = 10-x+3x+2x Solve for x and find pressures of A, B, C; substitute into Kp expression below and solve for Kp. Kp = p^3C*p^2B/pA Then dG = -RT*ln*Kp T is 25C (...
Friday, January 31, 2014 at 2:56pm by DrBob222

chemistry -drbob222 (correction)
work for 2: (typo, correction below) Kp = [(1.0-x)/ 10]/[x/ (100)] =2.7 Kp = [(1/28-x)/ 10]/[x/ (100)] =2.7 Kp = [([1/28]^2-x)/ 10]/[x/ (100)] =2.7 x=(1/28)^3 g
Friday, October 9, 2009 at 5:48am by Anonymous

CHEMISTRY HELP!
Consider the following reactions and their equilibrium constants. (NO(g) + 0.5Br2(g) <===> NOBr(g) Kp = 5.3 2NO(g) <===> N2(g) + O2(g) Kp = 2.1 x 1030 Use these equations and their equilibrium constants to determine the equilibrium constant for the following ...
Wednesday, April 27, 2011 at 11:51pm by jon

chemistry
Tricky, tricky. You will notice that the two Kc values given are for different reactions. What you must do is to multiply equation 2 by 4, reverse it, and add it to equation 1. The result is the equation they want for Kp; i.e., P4(s) + 6Cl2 ==> PCl3(l) So if you do that, ...
Wednesday, July 20, 2011 at 3:25pm by DrBob222

Chemistry
I had to calculate delta G which came out to be 10.30 then i had to solve for Kp so I used the equation DeltaG=-RT(ln Kp) then I got .01565, now im trying to calculate the equilibrium pressure of O2 and that has me stumped.
Friday, July 12, 2013 at 1:03pm by Catherine

Physics
Find the gradient and intercept of this equation q=kp^n and qm=kp^n
Tuesday, December 6, 2011 at 8:18pm by Emmzy

Chemistry
This may sound wordy but it is the definition of Kp. Almost word for word what my chemistry prof said long long ago. "The product of the partial pressures of the products of the reaction divided by the product of the partial pressures of the reactants, each raised to a power ...
Sunday, March 9, 2008 at 11:07pm by DrBob222

CHEMISTRY
Kp = pA*pB = 4. I would let pA = p which means pB = p and solve for p. Kp = Kc(RT)delta n
Sunday, March 18, 2012 at 5:05pm 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
I assume that K listed is Kp and not Kc. Note that your equation is not balanced. ........2NO2 --> 2NO + O2 I.......0.25......0.....0 C........-2x......2x.....x E.......0.25-2x....2x......x Kp = pNO^2*pO2/pNO2^2 Substitute and solve for x and 2x
Thursday, November 29, 2012 at 5:09am by DrBob222

college chemistry
The second equation is just the reverse of the first equation; therefore, the Kp for the second equation is the reciprocal of Kp for the first one given; i.e., Kp2 = (1/4.57 x 10^-2) = ??
Sunday, October 3, 2010 at 11:01pm by DrBob222

Chemistry
Right digits; wrong sign. dGrxn = (n*dG products) - (dG reactants) = (0) - (-770) = +770. dG = -RT*lnK Substitute and solve for Kp. Kp = pO23/2
Friday, April 6, 2012 at 11:15pm by DrBob222

Chemistry
I would approach it this way. ........CO2 + C ==> 2CO2 I.......0.5..solid....0 C.......-x...........2x E......0.5-x.........2x You know that0.5-x + 2x = 0.8 Solve for x, then pCO2 and pCO2 and plug those into the Kp expression and solve for Kp.
Wednesday, July 24, 2013 at 9:01am by DrBob222

chemistry
Determine Kc at 298 K for the reaction 2 CH4(g) reverse reaction arrow C2H2(g) + 3 H2(g), given the following data at 298 K. (Hint: How are Kc and Kp for the reaction related?) CH4(g) + H2O(g) reverse reaction arrow CO(g) + 3 H2(g) Kp = 1.2 multiplied by 10-25 2 C2H2(g) + 3 O2...
Wednesday, March 24, 2010 at 6:21pm by Jenny

College Chemistry
Determine Kc at 298 K for the reaction 1/2 N2(g0 + 1/2 O2(g) + 1/2 Cl2(g)--> NOCl(g), given the following data at 298 K 1/2 N2(g) + O2(g)--> NO2(g) Kp= 1.0 x 10^-9 NOCl(g) + 1/2 O2(g)-->NO2Cl(g) Kp= 1.1 x 10^2 NO2(g) + 1/2 Cl2(g)--> NO2Cl(g) Kp= 0.3
Wednesday, October 27, 2010 at 3:37pm by Jalisa

Chemistry
I think I would do the following: NH4Cl(s) ==> NH3(g) + HCl(g) Ptotal = PNH3 + PHCl 2.2 atm = PNH3 + PHCl From the equation, PNH3 = PHCl; therefore, 2.2 = 2PNH3 and you can go from there. Then substitute partial pressures into Kp = PNH3*PHCl to find Kp.
Monday, March 2, 2009 at 11:52pm by DrBob222

Chemistry
You can do this either Kc and convert to Kp or you can do it Kp all the way. initial: COCl2 = use 0.03 = n and solve PV=nRT for partial pressure COCl2. I get 1.31 atm or something like that. You need to do it more accurately. CO = 0 Cl2 = 0 equilibrium: CO: partial pressure = ...
Sunday, April 25, 2010 at 1:53pm by DrBob222

Chemistry
I believe that, if you are calculating M, you must be dealing with Kc but the problem gives you Kp. I think what you need to do is to solve for mole fraction of each gas. mole fraction NO = moles NO/total moles. mole fraction O2 = moles O2/total moles. mole fraction NO2 = mole...
Saturday, October 16, 2010 at 8:23pm by DrBob222

Chemistry 2
Calculate Kp for the reaction C(s)+CO2(g)<-->2CO(g) kp=? C(s)+2H2O(g)<--->CO2(g)+2H2 kp1=3.47 H2(g)+CO2(g)<--->H2O(g)+CO(g) kp2=0.735
Friday, February 21, 2014 at 1:30pm by Sharon

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) I'm sorry.. English is a second language for me. After solving for K'c and ...
Thursday, March 15, 2012 at 9:55pm by David

Chemistry
Jerry? Sarah? We prefer that you not change screen names. ............H2S ==> H2 + S initial....0.121 atm.0...0 change.....-2p.....p....+p equil.....0.121-2p..p....p Kp = pH2*pS/pH2S Substitute into the Kp expression from the ICE chart above and solve for p, then 0.121-2p.
Friday, March 9, 2012 at 9:17pm by DrBob222

Chemistry
Calculate the value of Kp for the equation C(s)+CO2(g)<->2CO(g) Kp=? given that at a certain temperature C(s)+2H2O(g)<->CO2(g)+2H2(g) Kp1=3.33 H2(g)+CO2(g)<->H2O(g)+CO(g) Kp2=.733 Please show detailed steps.
Thursday, February 7, 2013 at 8:27pm by Julia

Chemistry
Nitrogen Dioxide , a pollutant in the atmosphere, can combine with water to form nitric acid. One of the possible reactions is shown here. Calculate delta ∆G° and Kp for this reaction at 25°C and comment on the spontaneity of the reaction. 3NO2(g)+H2O(l)--> 2 HNO3(aq...
Thursday, March 29, 2012 at 4:40pm by SANDY

chemistry
N2 + O2 ==> 2NO Kp = pNO^2/pN2*pO2 = 0.05 Set up an ICE chart. initial: NO = 0 N2 = 0.8 O2 = 0.2 change: NO = 2x N2 = -x O2 = -x equilibrium: NO = 2x N2 = 0.8-x O2 = 0.2-x Substitute into Kp and solve. Post your work if you get stuck.
Tuesday, March 16, 2010 at 12:50am by DrBob222

chemistry
2. Methanol, CH3OH, is used as fuel in race cars. This liquid fuel can be synthesized using the following process C(s)+ ½ O2(g) + 2H2(g)  CH3OH(l) Calculate delta G using the deta Gf of the reaction. Calculate Kp. What is the relation between the magnitude of delta G ...
Thursday, April 15, 2010 at 7:32am by Kristen

Chemistry
Is that Kp in bar? ........C3H8 ==> C3H6 + H2 Total P = 2 = pC3H6 + pH2 + pC3H8 Solve for pC3H8 = 2-p-p = 2-2p Kp = p*p/(2-2p) Solve for p = H2 = C3H6
Friday, February 14, 2014 at 3:25pm by DrBob222

For the system CaO(s) + CO2(g) = CaCO3(s), I added 1.00 mol of CaO(s) to 1.00L of 0.500M CO2(g) at 200 oC. At equilibrium the [CO2] = 0.150M. What is the value of Kp for this reaction? Kp would = CaCO3/(CaO)(CO2) I do not know what to do with the 0.500M and 1.00mol.
Wednesday, March 14, 2012 at 9:51pm by Hannah

Chemistry
For 1/2 the reaction, new k is sqrt Kp. For 2 x reaction, new k is K^2p For the reverse and 1/2 new k is 1/sqrt Kp.
Monday, February 20, 2012 at 9:10pm by DrBob222

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

Chemistry
Kp = pNH3*pHCl = some number. Let's just make up a number, say pNH3 = 5 atm; pHCl = 5 atm, Kp = 5*5 = 25. Now, if we double the volume, we will half the pressure so if we half NH3 pressure and half pressure HCl, that makes Qp = 2.5*2.5 = 6.25 which means the reaction will ...
Sunday, February 10, 2013 at 4:32pm 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

college chemistry
The value of the equilibrium constant (Kp) as represented by the first chemical equation is 4.57 x 10-2 at 395 °C. Calculate the value of the equilibrium constant (Kp) for the second equation at the same temperature. Express answer in scientific notation. Cl2CO(g) = CO(g)+Cl2(...
Sunday, October 3, 2010 at 11:01pm by sparkle

Chemistry
0.100 mol of SO2 and 0.100 mol of O2 are introduced in a flask of 1.52 L. When in equilibrium, 203 is found to be 0.0916 mol. Determine kp. 2S03(g) <-> 2SO(g) + O2(g) In order to solve this question 1st I made an ICE table and I got the values 2SO3 <-> 2SO + 02 I ....
Saturday, May 28, 2011 at 8:48pm by K

Chemistry
The equilibrium constant Kp for the following reaction is 4 atm^2 at 300 K. 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? How would i solve this when they don't even give me any partial pressures?! All of the ...
Saturday, March 17, 2012 at 7:10pm by David

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
Try this. PCO + PCl2 + PCOCl2 = 1.24 1 mole CO reacts with 1 mole Cl2 to produce 1 mole COCl2 so 3x = 1.24 solve for x to find partial pressure of COCl2. Then PCO = 0.93-x; PCl2 = 1.01-x, substitute those into the Kp expression and solve for Kp.
Wednesday, November 17, 2010 at 11:07pm by DrBob222

physical chemistry
I would do this. Let x = fraction of gas that is NO2 The 1-x = fraction that is N2O4 molar mass NO2 = 46 molar mass N2O4 = 92 46(x) + (92(1-x) = 69 Solve for x and I get 0.5 which is the mole fraction of these gases. Then pNO2 = XNO2*Ptotal and pN2O4 = XN2O4*Ptotal Finally, Kp...
Sunday, May 12, 2013 at 11:41am by DrBob222

Chemistry
In the gas phase reaction CH4 + H2O → CO + 3 H2 At T = 1500 K , Kp = 11000 Calculate Kp, T = 1500 K , for the following reaction 3 CO + 9 H2 → 3 CH4 + 3 H2O .
Thursday, September 24, 2009 at 1:35pm by Ava

chemistry
..........PCl5 --> PCl3 + Cl2 E.........217.......13.2 13.2 Kp = pPCl3*pCl2/pPCl5. Substitute the E line into Kp expression and solve for Kp. Cl2 added. Total P = 217 + 13.2 + 13.2 = 243.4 New total P = 263 Cl2 added = 263-243.4= 19.6 torr New Cl2 = 19.6 + 13.2 = 32.8 torr...
Tuesday, February 25, 2014 at 6:42am by DrBob222

College Chemistry
The value of the equilibrium constant (Kp) as represented by the first chemical equation is 1.80 x 10-2 at 500 K. Calculate the value of the equilibrium constant (Kp) for the second equation at the same temperature. Express answer in scientific notation. 2NOCl(g) = 2NO(g)+Cl2(...
Sunday, March 21, 2010 at 6:27pm by Anonymous

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
Ammonium iodide dissociates reversibly to ammonia and hydrogen iodide. NH4I(s) <==> NH3(g) + HI(g) At 400°C, Kp = 0.215. Calculate the partial pressure of ammonia at equilibrium when a sufficient quantity of ammonium iodide is heated to 400°C. Please help! would it just ...
Thursday, March 8, 2012 at 7:42pm by Sarah

Chemistry
No, and I gave you the wrong information because I didn't see an arrow sign and I though the CO2 was a product. It isn't, it's a reactant. Therefore, Kp = 1/pCO2. You need to find the partial pressure of the CO2 which you can do from PV = nRT. You know V= 1L, you know R, T is ...
Wednesday, February 29, 2012 at 9:23am 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

Chemistry
Kp = pCO2
Wednesday, February 29, 2012 at 9:23am by DrBob222

Chemistry
Is there a Kp? Kc?
Thursday, May 3, 2012 at 11:53am by DrBob222

Chemistry
there isnt a kp or a kc
Thursday, May 3, 2012 at 11:53am by Jake

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