Number of results: 11,053
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
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
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
At a certain temperature, the equilibrium constant, Kc, for this reaction is 53.3. H2(g)+I2(g) <--> 2HI(g) Kc= 53.3 At this temperature, 0.300 mol of H2 and 0.300 mol of I2 were placed in a 1.00-L container to react. What concentration of HI is present at ...
Friday, March 8, 2013 at 10:38pm by Lisa
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
The following reaction is a step in the commercial production of sulfuric acid. 2SO2(g) + O2(g) 2SO3(g) The equilibrium constant is very high at room temperature, but the reaction is very slow. It must be run at high temperatures to achieve a reasonable rate of reaction. ...
Tuesday, October 5, 2010 at 6:35pm by Anonymous
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
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
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 ...
Sunday, March 18, 2012 at 10:16pm by Raskin
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 ...
Sunday, March 18, 2012 at 5:07pm 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? This is what I have so far: I did Kc=0.25(1100(0.0821))^-1 and got Kc=0.00276. That is incorrect. Why? What did I do wrong? I believe I gave ...
Tuesday, July 31, 2007 at 2:00pm by Taasha
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 ...
Monday, March 22, 2010 at 10:24pm 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
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(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
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? ...
Friday, February 9, 2007 at 9:13am by Marisol
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
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
Assume that Kc = 0.0360 at 520°C for the first reaction above. What is the Kc for the second reaction at the same temperature? 2 HI(g)-> H2(g) + I2(g) H2(g) + I2(g) -> 2 HI(g) I thought the answer woudl just be negative because all you have to do is switch ...
Saturday, February 16, 2013 at 6:58pm 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
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
At a certain temperature, 0.900 mol of SO3 is placed in a 2.00-L container. 2SO3(g)<--> 2SO2(g)+O2(g) At equilibrium, 0.130 mol of O2 is present. Calculate Kc. Kc= ? Please post the answer if possible or the steps in detail; I have attempted this problem many ...
Friday, March 8, 2013 at 10:35pm by Laura
chemistry
then like teh same for thsi one Assume that Kc = 0.0130 at 520°C for the first reaction above. What is the Kc for the second reaction at the same temperature? 2 HI(g)->H2(g) + I2(g) HI(g)->½ H2(g) + ½ I2(g) why cant you just divide the k by 2?
Saturday, February 16, 2013 at 6:58pm by Hannah
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'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
chemistry
What's the temperature for the Kc listed?
Sunday, February 26, 2012 at 8:15pm by DrBob222
Science(chemistry)
What is Kc at its temperature?
Saturday, February 5, 2011 at 10:31am by Rozer
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(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) + ½ O2(g) Kc = 3.93 calculate a value for Kc for the reaction, NOCl (g) + ½ O2 (g) == NO2 (g) + ½ Cl2 (g) I do not understnad how I am suppose to use the Kc values given if ...
Wednesday, March 14, 2012 at 9:04pm by Hannah
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(....
Friday, December 9, 2011 at 7:46pm by Summer
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 >>&...
Wednesday, March 10, 2010 at 3:48am by abe
AP CHEM!
IM SO CONFUSED PLEASE HELP! H2 +CO2-->H2O + CO When H2 is mixed with CO2 at 2,000K, equilibrium is achieved according to the equation above. In one experiment, the following equilibrium concentrations were measured. [H2]= 0.20mol/L [CO2]= 0.30mol/L [H2O]=[CO]= 0.55mol/L...
Tuesday, April 3, 2007 at 10:07pm by linds
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
The value of the equilibrium constant (Kc) as represented by the first chemical equation is 2.70 x 10-3 at 1200 K. Calculate the value of the equilibrium constant (Kc) for the second equation at the same temperature. Express answer in scientific notation. F2(g) = 2F(g) 2F(g...
Tuesday, April 13, 2010 at 11:38pm by andy
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
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
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
P. Chemistry
The equilibrium 2 SO2(g) + O2(g) 2 SO3(g) has the value K = 2.5 1010 at 500. K. Find the value of K for each of the following reactions at the same temperature. (a) SO2(g) + 1/2 O2(g) SO3(g) K = (b) SO3(g) SO2(g) + 1/2 O2(g) K = (c) 3 SO2(g) + 3/2 O2(g) 3 SO3(g) I attempted to...
Monday, February 15, 2010 at 10:00pm by Tommy
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
Chemistry
At a certain temperature, the equilibrium constant, Kc, for this reaction is 53.3. At this temperature, 0.300 mol of H2 and 0.300 mol of I2 were placed in a 1.00-L container to react. What concentration of HI is present at equilibrium?
Saturday, January 19, 2013 at 4:49pm by Paul
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 ...
Monday, November 15, 2010 at 9:53am by shanice
chemistry
At high temperature, 2.00 mol of CH2O was placed in a 4.00 L container where it decomposed via the equilibrium CH2O(g)<=>CO(g)+H2(g) . At equilibrium, the concentration of CO was measured to be 0.0317 M. What is Kc for this reaction at this temperature?
Saturday, April 20, 2013 at 9:56am by alex
Chemistry
At elevated temperatures, SbCl5 gas decomposes into SbCl3 gas and Cl2 gas as shown by the following equation: SbCl5(g)<=> SbCl3(g) + Cl2(g) 1. What is the concentration in moles per liter of SbCl5 in the container before any decomposition occurs? 2. What is the ...
Saturday, January 15, 2011 at 10:52am by Fred
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 : ½ N2(g) + ½ O2(g) ⇌ NO (g) Kc = 4.8 x 10-10 2 NO2(g) ⇌ 2 NO (g) + O2...
Thursday, February 9, 2012 at 6:18pm by Daniel
Chemistry-w/addition
1. What is the concentration in moles per liter of SbCl5 in the container before any decomposition occurs? moles = grams/molar mass. Solve for moles. M = moles/L. Solve for M. 2. What is the pressure in atmospheres of SbCl5 in the container before any decomposition occurs? Use...
Saturday, January 15, 2011 at 2:13pm by DrBob222
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) <----&...
Sunday, February 8, 2009 at 3:29pm by Saira
college
Kp for the reaction CO2(g) + C(s) 2CO(g) is 1.47 at 727°C. Calculate Kc at this temperature
Sunday, July 22, 2012 at 11:20pm by gggg
chemistry
Kp for the reaction is 1.47 at 727°S CO2(g) + C(s) 2CO(g) Calculate Kc at this temperature
Saturday, July 21, 2012 at 11:12pm by ken
Chemistry
Consider the following equilibrium process at 686 C C02(g)+H2(g)=CO(g)+H20(g) The equilibrium concentration of the reacting species are [CO]=0.050M, [H2]=0.045M, [CO2]=0.086M, and [H20]=0.040M. (a)Calculate the Kc for the reaction at 686 C. (b) If we add CO2 to increase its ...
Sunday, April 25, 2010 at 1:04pm by Amphee
chemistry
At 25C, Kc= 3.7x10^9 for the reaction CO(g) + Cl2(g) equilibrium with COCl2(g) Calculate the Kp at this temperature.
Tuesday, October 9, 2007 at 7:52pm by Wolf
Chemistry
A 100 L reaction container is charged with 0.724 mol of NOBr, which decomposes at a certain temperature** (say between 100 and 150 oC) according to the following reaction: NOBr(g) ↔ NO(g) + 0.5Br2(g) At equilibrium the bromine concentration is 1.82x10-3 M. Calculate ...
Wednesday, February 20, 2013 at 8:59pm by Anonymous
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
Chem
I have a question on this question would I forgo the sqaure root on this on because there is no sqaure except on the products side which is 2HI? I am lost because I set up ICE then got to: 54=(4X-0.09)^2/x*x Kc=[HI]^2/[x][x] At a particular temperature, Kc = 54 for the ...
Tuesday, March 23, 2010 at 5:39pm by CC
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) + ½ O2(g) Kc = 3.93 calculate a value for Kc for the reaction, NOCl (g) + ½ O2 (g) == NO2 (g) + ½ Cl2 (g) So I understand that 2NO + Cl2 + 1/2O2 = NO2 + 1/2 Cl2 but I do not ...
Thursday, March 15, 2012 at 1:54pm by Hannah
chemistry
At 1100 K, Kp = 0.25 for the reaction 2SO2(g) + O2(g) equilibrium with 2SO3(g) What is the value of Kc at this temperature?
Tuesday, October 9, 2007 at 8:39pm by Wolf
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 &...
Wednesday, June 25, 2008 at 1:43pm 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
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
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 (please help me!)
H2(g) + CO2(g)<-> H20(g) + CO(g) When H2(g) is mixed with CO2(g) at 2,000K, equilibrium is achieved according to the equation above. In one experiment, the following equilibrium concentrations were measured: [H2]=0.20 M [CO2]=0.30 M [H2O]=[CO]=0.55M a) What is ...
Sunday, February 25, 2007 at 6:07pm by sara
Chemistry
Write the Kc expression, substitute the numbers given and solve for Kc.
Wednesday, March 21, 2012 at 9:46pm by DrBob222
Chemistry-w/addition
At elevated temperatures, SbCl5 gas decomposes into SbCl3 gas and Cl2 gas as shown by the following equation: SbCl5(g)<=> SbCl3(g) + Cl2(g) (a) An 59.8 gram sample of SbCl5 (molecular weight 299.0) is placed in an evacuated 15.0 liter container at 182°C. 1. ...
Saturday, January 15, 2011 at 2:13pm by Fred
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
At a certain temperature, the Equilibrium constant, Kc, for this reaction is 53.3. At this temperature, 0.500 mol of H2 and 0.500 mol of I2 were placed in a 1.00-L container to react. What concentration of HI is present at Equilibrium? equation: H2 + I2 = 2HI
Tuesday, December 11, 2012 at 1:40am by cody
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
At a certain temperature, the equilibrium constant, Kc, for this reaction is 53.3. H2(g)+I2(g) <-> 2HI(g) At this temperature, 0.300 mol of H2 and 0.300 mol of I2 were placed in a 1.00-L container to react. What concentration of HI is present at equilibrium?
Monday, March 25, 2013 at 9:36am by Anonymous
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...
Sunday, March 1, 2009 at 8:41pm by DrBob222
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
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
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
At a certain temperature, 0.660 mol of SO3 is placed in a 3.00 L container. 2SO3=>2SO2+O2 Kc=
Saturday, July 23, 2011 at 1:48am by Josh
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 ...
Friday, September 10, 2010 at 3:12am by Riley
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...
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 ...
Monday, March 5, 2012 at 10:52pm 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
............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 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
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 ...
Saturday, October 15, 2011 at 9:18pm 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=...
Monday, March 2, 2009 at 1:26am by Anonymous
chemistry
The reaction SO2 + 1/2O2 -->SO3 has kp equal to 6.55 at 627C. what is the value of kc at this temperature? how do you set this up?
Wednesday, April 14, 2010 at 11:18pm by Anna
Calculus
For a given take-off weight, the take-off distance increases if the air temperature increases. For a specific example, if a KC-135 weighs 200,000 lbs, the take-off distance is modeled by f(t)=1/3(t+145)^2 - 67. If D = f(t) , where D is the take-off distance as a function of t...
Sunday, August 17, 2008 at 5:36pm by Hamilton
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
ap chemistry
At a certain temperature, the equilibrium constant Kc is 0.154 for the reaction 2 SO2(g) + O2(g) *) 2 SO3(g) What concentration of SO3 would be in equilibrium with 0.250moles of SO2 and 0.853 moles of O2 in a 1.00 liter container at this temperature? Note: These latter moles ...
Monday, January 28, 2013 at 8:37pm by cheri
ap chem
At a certain temperature, the equilibrium constant Kc is 0.154 for the reaction 2 SO2(g) + O2(g) *) 2 SO3(g) What concentration of SO3 would be in equilibrium with 0.250moles of SO2 and 0.578 moles of O2 in a 1.00 liter container at this temperature? Note: These latter moles ...
Sunday, February 13, 2011 at 6:39pm by Anonymous
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
When 0.59 mol I2(g) and 0.59 mol H2(g) are placed into a 1.0-L container at a given temperature, 0.30 mol H2(g) is found to be present after the reaction below reaches equilibrium. Calculate Kc at the given temperature. I2(g) + H2(g) 2HI(g)
Friday, November 19, 2010 at 10:00pm by Shayne
Chemistry --really need help!
I am really struggling with these problems!! A reaction mixture that consisted of 0.20 mol N2 and 0.20 mol H2 was introduced into a 25.0 L reactor and heated. At equilibrium, 5.0% of the nitrogen gas has reacted. What is the value of the equilibrium constant Kc for the ...
Friday, February 19, 2010 at 7:05pm by Angelica
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
Chem
At a particular temperature, Kc = 54 for the reaction H2(g) + I2 (g) <=> 2 HI(g). One mole of HI is placed in a 3.0-L container. What would be the equilibrium concentration of HI?
Monday, March 22, 2010 at 10:23pm by CC
chemistry
When N2O5 (g) is heated it dissociates into N2O3 (g) and O2 (g) according to the following reaction: N2O5 (g) <--> N2O3 (g) + O2 (g) Kc=7.75 at a given temperature. The N2O3 (g) dissociates to give N2O (g) and O2 (g) according the following reaction: N2O3 (g) &...
Saturday, February 12, 2011 at 10:55pm by Anonymous
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-...
Tuesday, May 24, 2011 at 2:33pm by DrBob222
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(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 help please!
Suppose K= 4.5x10^-3 at a certain temperature for the reaction : PCl5 <--> PCl3+ Cl3, what must be the concentration of Cl2 under these conditions? Is this Kc or Kp? I assume Kc. The easiest way to solve this is to set up an ICE chart, substitute the unknowns ...
Thursday, May 20, 2010 at 9:06pm by DrBob222
chemistry
a. what is the effect on the Kc when the temperature of an exothermic reaction is lowered? b. according to Le Chatelier's principle, how is equilibrium in part a established.
Friday, November 30, 2012 at 10:03am by Boo Boo
Chem
At a particular temperature, Kc = 54 for the reaction If 1.0 mole of H2 and 1.0 mole of I2 are placed in a 5.0 L container, what would be the equilibrium concentration of HI?
Monday, March 22, 2010 at 10:22pm by CC
Pages: 1 | 2 | 3 | 4 | 5 | 6 | 7 | 8 | 9 | 10 | 11 | 12 | 13 | 14 | 15 | Next>>
For Further Reading
