Wednesday
May 4, 2016

# Search: H2 + I2 2HI

Number of results: 106

chem12
for the equilibrium 2HI(g)--- H2(g) + I2 k eq = 8.0 2.0 mol of HI are placed in a 4.0 L container, and the system is allowed to reach equilibrium. Calculate the equilibrium concentration of all three gases. Inital 2HI 0.5mol/l H2 =0 I2=0 change 2HI= -2x H2=+x I2=+x equilibrium...
March 8, 2016 by George

chem12
2HI(g)--H2(g) + I2(g) k eq= 8.0 2.0 mol of HI are placed in a 4.0L container, and the system is allowed to reach equilibrium. Calculate the equilibrium concentration of all three gases Initial 2HI=0.5 mol/L H2= 0 I2=0 change 2HI= -2x H2= x I2=x equilibrium 2HI= 0.5-2x H2= x I2...
March 13, 2016 by George

chem12
2HI(g)--H2(g) + I2(g) k eq= 8.0 2.0 mol of HI are placed in a 4.0L container, and the system is allowed to reach equilibrium. Calculate the equilibrium concentration of all three gases Initial 2HI=0.5 mol/L H2= 0 I2=0 change 2HI= -2x H2= x I2=x equilibrium 2HI= 0.5-2x H2= x I2...
March 14, 2016 by George

chem 12
for the equilibrium 2HI(g)--- H2(g) + I2 k eq = 8.0 2.0 mol of HI are placed in a 4.0 L container, and the system is allowed to reach equilibrium. Calculate the equilibrium concentration of all three gases. Inital 2HI 0.5mol/l H2 =0 I2=0 change 2HI= -2x H2=+x I2=+x equilibrium...
March 10, 2016 by George

Chemistry
2HI(g)--> H2(g) + I2(g) The rate law for the decomposition of HI is r=k[HI]^2. The rate of the rxn was found experimentally to b 2.5 x 10^4 mol/L x s where the HI concentration was 0.0558 M. Are these values ready to plug in to the equation, or because there is 2HI, do I ...
May 16, 2010 by Jamie

Hi! is my answer correct? Consider the following chemical reaction: H2 (g) + I2 (g) <> 2HI (g) At equilibrium in a particular experiment, the concentrations of H2, I2, and HI were 0.15 M, 0.033 M, and 0.55 M, respectively. The value ofKeq for this reaction is I solved by...
October 25, 2010 by Richard

Idontgetit
The value of the equilibrium constant (Kp) as represented by the first chemical equation is 2.00 x 10-2 at 730 K. Calculate the value of the equilibrium constant (Kp) for the second equation at the same temperature. Express answer in scientific notation. 2HI(g) = H2(g)+I2(g) ...
October 2, 2013 by Chemistry

Chemistry
H2S+Is >2HI+S
April 16, 2016 by Science

Chemistry
Even when a mechanism is consistent with the rate law , later experimentation may it to be incorrect or only one of several alternative. As an example, the reaction between hydrogen and iodine has the following rate law: rate=k[H]^3[I]2. The long accepted mechanism proposed a ...
February 28, 2015 by Munavvar

chemistry
in a reversable reaction H2+I2=2HI,what will happen to the equilibrium if the volume is decrease?
September 7, 2014 by Starsha

chemistry
Considering the reaction i2 h2=2hi energy change =( tive) and give reasons how "HI" will be produced
February 10, 2015 by idiani

chemistry
H2(g) + I2(g) *) 2HI(g) + heat Which response includes all the following that will shift the equilibrium to the left, and no others?
March 10, 2013 by Anonymous

chemistry
H2(g) + I2(g) *) 2HI(g) + heat Which response includes all the following that will shift the equilibrium to the left, and no others?
March 10, 2013 by Anonymous

Chemistry
At some temperature, Keq = 33 for the reaction H2 + I2 „³ 2HI. If initially, [H2] = .0600 M and [I2] = .0300 M, what are all three equilibrium concentrations?
May 28, 2013 by Jim

chemistry
at some temperature, Keq=33 for the reaction H2 + I2 -> 2HI. If initially, [H2]= .0600 M and [I2]= .0300 M, what are all three equilibrium concentrations?
March 7, 2016 by seth

chemistry
H2+I2->2HI If 3 moles of H2, I2, and HI are in a 3L flask, what will be the equilibrium amount of each. Kc=5 The answer is H2= I2= .71M, HI= 1.584M(given by teacher) Just need to know how to do the work.
October 17, 2007 by corey

chemisty
when 2.75 mol HI(g) placed in 1L container and allowed to dissociate into 2HI(g) <==> H2(g)+I2(g) Final H2 concin .275M. What is Ka for rxn The answer is .0156. But I don't know why Thanks
June 6, 2012 by chemistt

Chemistry
Assuming all gases are at the same temperature and pressure, how many milliliters of hydrogen iodide are produced from 160mL of H2? H2(g)+I2(g)→2HI(g)
November 25, 2014 by blank

Chemistry II
At a certain temperature, Kc = 33 for the reaction: H2(g) + I2(g) 2HI(g) Assume that the initial concentrations of both H2 and I2 are 6.00 x 10-3 mol/L. Find the concentration of each reactant and product at equilibrium.
February 22, 2011 by Tiffany

CHEMISTRY
DETERMINE THE NUMERICAL VALUE OF KEQ. A) 2HI(g)--------H2(g) +I2(g) Where [HI]=0.27m,[H2]=0.86M and [I2]=0.86M at 200c
December 1, 2011 by DIAMONDPRM

chemistry
Calculate Delta G for each reaction using Delta Gf values: answer kJ ...thank you a) H2(g)+I2(s)--->2HI(g) b) MnO2(s)+2CO(g)--->Mn(s)+2CO2(g) c) NH4Cl(s)--->NH3(g)+HCl(g) is this correct? a) H2(g)+I2(s)--->2HI(g) From tables: G HI = +1.3 kJ/mol G H2 = 0 G I2 = 0 dG...
October 28, 2015 by Patrick

Chemistry
The decomposition of HI(g) is represented by the equation: 2HI(g) <-> H2(g) + I2(g) Kc= 64 at 25°C. If the equilibrium concentrations of H2 and I2 at 400°C are found to be [H2] = 5.4x10-4 M and [I2] = 8.8x10-3 M, what is the equilibrium concentration of HI?

chemistry
equilibrium constant = 55.3 @ certain temperature H2 (g) + I2 (g) <=> 2HI (g) (reversible) If you start with 0.195 M hydrogen iodide, what will the concentrations of H2, I2, and HI be at equilibrium?
March 31, 2014 by Anonymous

chemistry
What happens to the concentration of HI(g) when the total pressure on the equilibrium reaction 2HCl(g) + I2(s) <--> 2HI(g) + Cl2(g) is increased (by compression)? 1. increases 2. Unable to determine 3. decreases 4. remains the same

Chemistry 12
given the reacting system: H2 (G) + I2(G) ---> 2HI(g) Keq= 64 Equal moles of H2, I2, and HI are placed in a 1.0 L container. Use calculations to determine the direction the reaction will proceed in order to reach equilibirum
December 6, 2012 by Patrick

Chemistry 12
given the reacting system: H2 (G) + I2(G) ---> 2HI(g) Keq= 64 Equal moles of H2, I2, and HI are placed in a 1.0 L container. Use calculations to determine the direction the reaction will proceed in order to reach equilibirum
December 6, 2012 by Patrick

chemistry
the equilibrium system shown below was analyzed and the concentrations of HI(g, and I2(g) were found, in mol/L, to be 4.4, 3.2, 1.5 respectively. the equilibrium constant must be which f the following? H2(g) + I2(g)<> 2HI(g) + 65KJ
May 5, 2012 by nicole

chem
Keq for the reaction 2HI <----> H2 +I2 has a value of 1.85x 10^-2 at 425 degrees celsius. If 0.18 mol of HI is placed in a 2.0 L flask and allowed to come to equilibrium at this temperature. What will the equilibrium of [I2} be?
October 13, 2015 by a

Chemistry
The equilibrium constant for the reaction H2 + I2 --> 2HI, is 54 at 425 degrees C. If the equilibrium mixture contains 0.030 M HI and 0.015 M I2, calculate the equilibrium concentration of H2.
November 24, 2014 by Hannah

Chem
How can i determine that the volume is decreasing? Of the following equilibria, only ??? will shift to the left in response to a decrease in volume. A) 2HI <->(g) H2 (g) + I2 (g) B) N2 (g) + 3 H2 (g)<-> 2 NH3 (g) C) 4 Fe (s) + 3 O2 (g)<-> 2 Fe2O3 (s) D) 2 SO3...
October 25, 2010 by Ben

Chemistry
The following reaction has an equilibrium constant of 0.020 at a given temperature. 2HI(g) I2(g) + H2(g) If you have 1.00 mol HI(g) in a 0.750-L container initially, how many moles of HI(g) will be present when the system reaches equilibrium?

CHEM
1.) At what temperature will the rate constant for the reaction H2 + I2 to 2HI have the value 5.2×10−3 M^{-1}s^{-1}? (Assume k=5.4 *10^{-4}M}{-1)s}^{-1} at 599 K and k=2.8 * 10^{-2}M}^{-1}s}^{-1} at 683 K.) 2.)For the first-order reaction N2O5 to 2NO2 + 1/2O2 t_{1/2}=22....
March 3, 2010 by anonymous

chemistry
1.) At what temperature will the rate constant for the reaction H2 + I2 to 2HI have the value 5.2×10−3 M^{-1}s^{-1}? (Assume k=5.4 *10^{-4}M}{-1)s}^{-1} at 599 K and k=2.8 * 10^{-2}M}^{-1}s}^{-1} at 683 K.) 2.)For the first-order reaction N2O5 to 2NO2 + 1/2O2 t_{1/2}=22....
March 3, 2010 by anonymous

chemistry
equilibrium pressure at 731 K for the reaction H2+I2-2HI initially the mixture contains 0.08592 each of H2 and I2 and 1.0atm.what is the pressure of HI at equilibrium?
July 10, 2012 by christine

Chemistry
how do u complete these questions? 2HCI(aq)+Pb(NO3)2(aq)---> 2HI(aq)+K2SO3(s)---> Pb(NO3)2(aq)+2KCI(aq)---> Ba(NO3)2(aq)+Na2SO4(aq)---> K2CO3(aq)+Ba(NO3)2(aq)---> HCI(aq)+AgNO3(aq)--->
February 28, 2012 by Kim

Gr 12 chemistry
Based on this reaction: H2(g) + I2(g)= 2HI(g) How many moles of iodine are necessary for form 0.530 moles of hydrogen iodine
September 22, 2015 by Avery

chemistry
A 1L flask is filled with 1.000atm of H2 and 2.000atm of I2 at 448*C. The following equilibrium is established: H2(g)+I2(g)= 2HI(g). The value of K for this equilibri- um is 50.5. What are equilibrium partial pressures of H2,I2,and HI?
February 10, 2011 by Victor

Chemistry
Kc for the reaction of hydrogen and iodine to produce hydrogen iodide, H2(g)+I2(g)f 2HI(g) is 54.3 at 430C. What will the concentrations be at equilibrium if we start with 0.240M concentrations of both H2 and I2?
November 29, 2011 by mary

chemistry
I need to derive a net ionic equation after balancing: NA2PO4 (2-) +HI =? what I have so far is NA2Po4 +2HI = 2NAI +H3PO4 I can't get any farther but the answer is HPO4 (2-) +H =H2PO4 can someone help me with the steps?
July 1, 2012 by Nancy

chem
Hydrogen iodide can decompose into hydrogen and iodine gases. 2HI(g) mc026-1.jpg H2(g) + I2(g) K for the reaction is 0.016. If 0.148 atm of HI(g) is sealed in a flask, what is the pressure of each gas when equilibrium is established?
March 5, 2014 by jason

Chemistry***
A mixture containing 19.8 moles of H2 and 7.2 mole of I2 was allowed to reach equilibrium in a 5 L closed vessel at ToC according to the equation: H2 (g) + I2 (g) 2HI (g) At equilibrium, 14 moles of H2 was present. The equilibrium constant for this reaction is denoted as Kc(1...
December 30, 2014 by plasma membrane

chem
Reaction H2 +I2 yields 2HI All three gases are initially at 0.1atm/ upon reaching equilibrium it is found that H2 pressure droped by 55% what is the equilibrium constant for this reaction.
December 26, 2010 by Anonymous

Physical science
9 mol HI(g)is sealed with H2(g)in an empty 2 dm container when equilibriup is reached by the reaction..H2(g)+I2(g)=2HI(g) at 130 C it found that there are 5 mol HI(g)in the equilibrium mixture.calculate the equilibriup constant
January 31, 2013 by Lillian nhlapo

General Chemistry
H2 (g) + I2 (g) -> 2HI (g) What would happen to the amount of iodide present if hydrogen iodide is added? Removed? The volumeof the system is decreased? I got increase, decrease & same as my answer, but I don't completely understand it. Please help.
July 13, 2013 by <3

Chemistry
the initial concentration of each component was: 0.100 M H2(g), 0.100M I2(g), and 0.050 M HI(g) . The Keq = 50.2. Calculate the concentration of each component when equilibrium has been reached. The balanced chemical equation for this reactions is: H2(g) + I2(g)  2HI(g)
April 14, 2012 by Steve

CHEMISTRY
Hydrogen gas and iodine gas react via the equation, H2 + I2 <--> 2HI, and K=76 at 600K. If 0.05 mole of HI is placed in a flask at 600K, what are the equilibrium concentrations of HI, I2, H2? I am very lost at where to even start with this problem
March 18, 2012 by Kristen

Chemistry
Consider the following equilibrium: 2HI(g) *are in equilibrium with* H2(g) = I2(g) Keq = 81.0 A 2.00L container is initially filled with 4.00 mol HI. Calculate the [HI] at equilibrium. *I don't know how to put the equilibrium sign on the computer* Can someone please explain to...
November 12, 2014 by katie

Chemistry
Consider the following reaction: H2(g) + I2(s) ---> 2HI(g) TriangleH = 51.9 kj (enthalpy) Calculate the standard enthalpies of reaction for the following reaction: 6HI(g) ---> 3H2(g) + 3I2(s) Thanks!
April 28, 2012 by Sandy

chemistry
Hydrogen iodide decomposes according to the reaction 2HI(g)H2(g) + I2(g) A sealed 1.50 L container initially holds .00623 moles of H2, .00414 moles of I2, and .0244 moles of HI at 703K. When equilibrium constant is reached, the concentration of H2(g) is .00467 M. What are the ...
September 29, 2015 by jude

chemistry
Calculate the value of the equilibrium constant (Kp) for the reaction displayed if the following equilibrium pressure data were measured at 25.00 °C: P(H2(g)) = 0.2282 atm, P(I2(g)) = 0.1646 atm, P(HI(g)) = 5.462 atm. H2(g)+I2(g) = 2HI(g)
April 2, 2010 by bme1

CHEMISTRY
Which conditions ( reactant concentration , pressure , and temperature ) elevate high concentration of the underlines in these following equilibrium systems : 1) 2CO + O2 <==> 2CO2 + 167 kJ 2) Cu^+2 + 4NH3 <==> [ Cu(NH3)4 ]^+2 + 24 kJ 3) 2HI + 12.6 kJ <==> H2...

college chemistry
When a sample of HI(g) (5.825 mol) is placed in 320.0 L reaction vessel at 702.0 K and allowed to come to equilibrium the mixture contains 1.052 mol of H2(g). What is the equilibrium concentration (mol/L) of HI(g)? 2HI(g) = H2(g)+I2(g)
October 12, 2010 by sparkle

chemistry
for the reaction H2+I2--2HI at a given temperature it was found that an equilibrium mixture in a 10mL container consisted of 8.0 mol of HI, 1.0 mol of H2 nd 1.0 mole of I2. what is the equilibrium constant at that temperature?
September 14, 2015 by kedi

Chemistry
2HI <==> H2 + I2 Keq = 81.0 A 2.00L container is initially filled with 400 mol HI. Calculate the [HI] at equilibrium. This is what I did so far... HI = 4.00/2 = 2M ___2HI___<==>___H2___I2_ I 2.0M_________----__---- C -2X___________X_____X__ E 2-...
November 13, 2014 by Anonymous

chem
hydgogen and iodine form HI(g)per the reaction H2(g)+I2=2HI(g). If 2 L of iodine gas at .5 atm and 295 K react with excess oxygen, how many liters of HI at 295K and 1 atm will form?
March 31, 2008 by bob

Chemistry
Which of the following reactions will result in a reduced total pressure? a. CH4(g) + 2O2(g) → CO2(g) + 2H2O(g) c. 2HI(g) → H2(g) + I2(g) b. 2N2O(g) → 2N2(g) + O2(g) d. 2H2(g) + O2(g) → 2H2O()
November 6, 2012 by Brittany

chemistry
At a certain temperature, the equilibrium constant, K, for this reaction is 53.3. H2(g)+I2(g)->2HI(g) At this temperature, the reactants were placed in a container to react. If the partial pressures of H2 and I2 were each 0.300 bar initially, what is the partial pressure of...
March 12, 2015 by kelsey

chemistry
Determine the concentration at equilibrium if you start with 2.3 grams of Hydrogen and 200grams of Iodine in a 2.3 liter container. If you now add an extra .25M of HI after equilibrium, calculate Qc. Recalculate now what the concentrations should be at equilibrium. H2(g)+I2(g...
March 8, 2011 by regina

CHEMISTRY
To what temperature would the reaction below need to be heated to have a rate constant of 8.474e-4 M-1s-1 if the rate constant was 2.7000e-4 M-1s-1 at 327.00°C and the activation energy was 166.000 kJ/mol? H2(g) + I2(g) ↔ 2HI(g) a. 609.24°C b. 336.09°C c. 348.37°C d. 377...
April 6, 2014 by Chemistry

Chemistry
H2 (g)+I2 (g)↔2HI(g) Calculate ΔG for the system at 700 K when the concentrations are [H2] = 0.12M, [I2] = 0.27M, and [HI] = 0.118M. What would be my first step? If I make an ICE chart, what would I do from there? I just need the first step to help me out :( THANKS!
May 2, 2015 by Robby

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)
November 19, 2010 by Shayne

chemistry
dG for the formation of Hi(g) from its gaseous elements is -20.2 kj/mol at 500k. when the partial pressure of HI is 10 atm, and I2 0.001 atm, what must the partial pressure of hydrogen be at this temperature to reduce the magnitude of dG for the reaction to 0. H2(g)+I2(g)----&...
May 9, 2015 by thomas

thermodynamics
dG for the formation of Hi(g) from its gaseous elements is -20.2 kj/mol at 500k. when the partial pressure of HI is 10 atm, and I2 0.001 atm, what must the partial pressure of hydrogen be at this temperature to reduce the magnitude of dG for the reaction to 0. H2(g)+I2(g)----&...
May 10, 2015 by Anonymous

CHEMISTRY> HELP QUICK! pls
Calculate the reaction free energy of: H2(g) + I2(g) 2HI(g) when the concentrations are 0.026 mol L-1 (H2), 0.33 mol L-1 (I2), and 1.84 mol L-1 (HI), and the temperature is 700K. For this reaction Kc= 54 at 700 K. +11.6 kJ mol-1 0 kJ mol-1 -11.6 kJ mol-1 +2273 kJ mol-
September 5, 2010 by Lucinda

chemistry
There is 0.150 moles of H2 and I2, and are brought to equilibrium in a 3.30 L flask. The equation is H2 + I2 = 2HI. Find the equilibrium amounts of H2, I2, and HI. I'm not getting the correct answer. I set up the formula as x^2/(.04545-x) (.04545-x). To get moles I multiplied ...
March 14, 2010 by anonymous

Chemistry Kinetics
If I had the equation H2 + I2 --> 2HI could I write the rate of reaction as d[H2 + I2]/dt = k[H2]^x[I2]^y were x is the order of reaction with respect to x and y is just the order of reaction with respect to y thanks
December 1, 2010 by Kate

chemistry dont know how to do it
dG for the formation of Hi(g) from its gaseous elements is -20.2 kj/mol at 500k. when the partial pressure of HI is 10 atm, and I2 0.001 atm, what must the partial pressure of hydrogen be at this temperature to reduce the magnitude of dG for the reaction to 0. H2(g)+I2(g)----&...
May 10, 2015 by Anonymous

Chemistry
Air in the vicinity of a local power station contains 8.8x10^-4 gm^-3 SO2. What volume of 0.001moldm^-3 Iodine solution would be required to react with a solution obtained from 200dm^3 of contaminated air? The equation given is SO2 + I2 + 2H2O ==> H2SO4 + 2HI Thanks! :)
January 26, 2013 by Matt

Chemistry 2
The equilibrium constant, Kc, for the following reaction is 1.54E-2 at 643 K. 2HI(g) H2(g) + I2(g) When a sufficiently large sample of HI(g) is introduced into an evacuated vessel at 643 K, the equilibrium concentration of I2(g) is found to be 0.351 M. Calculate the ...
March 21, 2015 by Mariah

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
December 11, 2012 by cody

Chemistry
A 5.00L reaction vessel is filled with 1.00mol of H2, 1.00mol of I2, and 2.50mol of HI. If equilibrium constant for the reaction is 129 at 500k, what are the equilibrium concentrations of all species? H2(g) + I2(g) <-> 2HI(g) Kc = 129
March 16, 2013 by Presh

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?
March 25, 2013 by Anonymous

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 equilibrium? HI...
March 8, 2013 by Lisa

Chemistry 2
The equilibrium constant, Kc, for the following reaction is 1.54E-2 at 643 K. 2HI(g) H2(g) + I2(g) When a sufficiently large sample of HI(g) is introduced into an evacuated vessel at 643 K, the equilibrium concentration of I2(g) is found to be 0.351 M. Calculate the ...
March 21, 2015 by Mariah

Chemistry
Determine the concentration at equilibrium if you start with 4.65 grams of Hydrogen and 200 grams of Iodine in a 4.55 liter container. If you now add an extra 1.25M of I2 after equilibrium, calculate Qc. Recalculate now what the concentrations should be at equilibrium. H2(g...
July 28, 2015 by Jessica

Chemistry
How do I determine the value of the reaction 2HI(g) + 2.4 kcal --> H2(g) + i2(g) delta H = a) 2.4 kcal b) -2.4 kcal c) 0.00024 kcal d) -0.00024 kcal
February 16, 2016 by Susan

Chemistry
How do I determine the value of the reaction 2HI(g) + 2.4 kcal --> H2(g) + i2(g) delta H = a) 2.4 kcal b) -2.4 kcal c) 0.00024 kcal d) -0.00024 kcal
February 16, 2016 by Susan

Chemistry
Given the reaction 2HI (aq) + CaCO3(s) = CaI2(aq)+CO2(g)+H2O(l) What volume of of CO2 can be produced from 255mL of 3.0M HI and 75.2g of CaCO3 at STP? 75.2g CaCO3/100.09g/mol CaCO3 =.751mol CaCO3 (3M)(.255L)=.765 mol HI
March 28, 2016 by Kevin

Chemistry
At 400°C the reaction H2+I2<->2HI has an equilibrium constant Kp value of 55.5. A mixture of 1 mole of H2 and 1 mole of I2 is placed in a flask and heated to 400°C. Calculate the mole fraction of HI in the mixture of gases when equilibrium reached.
February 1, 2013 by Kelly

Chem II - Equilibrium
For the reaction at 430 degree C, H2 + I2 <=> 2HI Kc = 54.3. Initially 0.714 moles of H2 and 0.984 miles of I2 and 0.886 moles of HI are placed in a 2.40 L vessel. The equilibrium concentration of H2 and I2 are _____. Ok, I tried this by changing the moles to M by ...
June 16, 2008 by Ken

AP Chem
the activation energy for the reaction H2+I2 >>2HI is 167kJ/mol, and deltaE for the reaction is +28kJ/mol. What is the activation energy for the decompistion of HI?
October 27, 2011 by Grace Henry

chemistry(check my work)
Calculate the value of the equilibrium constant (Kp) for the reaction displayed if the following equilibrium pressure data were measured at 25.00 °C: P(H2(g)) = 0.2282 atm, P(I2(g)) = 0.1646 atm, P(HI(g)) = 5.462 atm. H2(g)+I2(g) = 2HI(g) is it like this, (5.462)^2/(0.2282x0....
April 4, 2010 by bme1

Chem
I stuck on this problem. Can you help me to solve it? A reaction mixture in a 3.67L flask at a certain temp. initially contains 0.763g H2 and 96.9g I2. At equilibrium, the flask contains 90.4g HI. Calculate the equilibrium constant(Kc) for the reaction at this temp. H2(g) + I2...
October 17, 2010 by Kim

Chemistry
The equilibrium constant for HI decomposition at 500 °C is 5.8×10-3. 2HI(g) > H2(g) + I2(g) At that temperature reactants and products are gaseous. (There is no change in the total number of moles, so Kc = Kp.) A sample of 0.49 mol of HI is placed in a 1.00 L vessel which ...
October 5, 2010 by Anonymous

Chemistry
The equilibrium constant for HI decomposition at 500 °C is 5.8×10-3. 2HI(g) > H2(g) + I2(g) At that temperature reactants and products are gaseous. (There is no change in the total number of moles, so Kc = Kp.) A sample of 0.49 mol of HI is placed in a 1.00 L vessel which ...
October 5, 2010 by Anonymous

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 ...
March 23, 2010 by CC

chemistry
Which of the following reactions will be spontaneous at standard state? Not all the reactions are balanced, so make sure they are balanced first. The ΔG of formation data can be found in an appendix in your text book. You may select multiple answers. Any reaction with ...
February 7, 2015 by danny

Chemistry
8. For the reaction H2(g)+I2(g)„\2HI(g); [H2] = 0.95 M; [I2] = 0.78 M; [HI] = 0.27 M. Calculate the equilibrium constant K and describe the direction (forward or reverse) of the reaction. Will adding a catalyst to the reaction alter the direction of the reaction? Why? Describe...
March 29, 2010 by Kathleen

chemistry
1)At room temperature (20 degree C), milk turns sour in about 64 hours. In a refrigerator at 3 degree C, milk can be stored three times as long before it sours. How long should it take milk to sour at 40 degree C (activation energy =44kj/mol)? 2)At what temperature will the ...
February 3, 2009 by sue

Chemistry
For the reaction: H2(g) + I2(g) 2HI(g) , Kc = 12.3 at some temperature T. If [H2] = [I2] = [HI] = 3.21 x 10-3 M at this temperature, which one of the following statements is true? 1. ) Not enough information is given to answer the question. 2. ) The concentration of HI will ...
October 25, 2009 by Jerry

Chemistry
Based on the following chemical equation answer the question below show all your calculation The balanced chemical reaction of iodine with hydrogen sulfide h2s(g)+i2(s)-----2HI(g) + S(s) (a) Based on the above chemically balanced equation, how many grams of HI should be ...
October 20, 2012 by Tasha

Chem II
For the reaction at 430 degree C, H2 + I2 <----->2HI. Kc = 54.3. Initially 0.714 moles of H2 and 0.984 moles of I2 and 0.886 molrd of HI are placed in a 2.40 L vessel. The equilibriuim concentration of H2 and I2 is _____. This is what I did. I changed all the moles ot M...
June 25, 2008 by Ken

chemistry
Based on the following chemical equation, answer the questions below. Show all your calculation The balanced chemical reaction of iodine with hydrogen sulfide is as follows: H2S(g)+I2(s)-----2HI(g) + S(s) (a) Based on the above chemically balanced equation, how many grams of ...
October 19, 2012 by Tasha

Help --->Chemistry
1) Complete and balance the following chemical reactins: 2HCI(aq)+Pb(NO3)2(aq)---> 2HI(aq)+K2SO3(s)---> Pb(NO3)2(aq)+2KCI(aq)---> Ba(NO3)2(aq)+Na2SO4(aq)---> K2CO3(aq)+Ba(NO3)2(aq)---> HCI(aq)+AgNO3(aq)---> 2) How could you separate gold from a mixture of ...
February 26, 2012 by melek

Chemistry
Consider the following reaction: H2+I2<->2HI A reaction mixture at equilibrium at 175 K contains P(H2)=0.958 atm, P(I2)=0.877 atm, and P(HI)=0.020 atm. A second reaction mixture, also at 175 K, contains P(H2)=P(I2)=0.616 atm, and P(HI)=0.106 atm. What will the partial ...
April 4, 2011 by Brooke

chemistry
Can someone explain this to me? In the reaction: --> AgCl(s)<_______ Ag+(aq) + Cl-(aq) the shorter arrow pointing to the right shows that the qe. mixture consists mostly of ______. ---> In the reaction HC2h302 + H20<_______ H30+ + C2h302-, when the concentration of...
July 20, 2008 by Xi

chemistry
In which one of the following processes is ΔH = ΔE? a. 2HI(g) → H2(g) + I2(g) at atmospheric pressure. b. Two moles of ammonia gas are cooled from 325°C to 300°C at 1.2 atm. c. H2O(l) → H2O(g) at 100°C at atmospheric pressure. d. CaCO3(s) → CaO(s...
August 15, 2009 by seth

Chemistry
for the reaction of hydrogen with iodine H2(g) + I2(g) --> 2HI(g) relate the rate of disappearance of hydrogen gas to the rate of formation of hydrogen iodide. and my answer is: rate formation of HI= delta [HI]/delta t and the rate of reaction of I2 = delta [I2]/ delta t to...
February 17, 2008 by Lauren

Chemistry
What is the percent yield of the reaction below if 2.23g of hydrogen gas react with 55.3 g of iodine to produce 43.1g of HI. use the equation below: H2+I2=2HI the answers: a) 21.8 b) 77.3 c) 33.7 d) 87.1 I started by trying to find the limiting reagent. I multiplied the 2.23 g...
March 22, 2016 by John

Chemistry
Hydrogen iodine is a strong acid that is used in chemical synthesis to produce some common drugs as well as a source for iodine, I2. Data for the formation of hydrogen iodine was obtained as shown. The reaction was found to be first order with respect to hydrogen gas and ...
May 19, 2007 by Christian

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