H2 + I2 2HI

120 results

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...

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...

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...

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...

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 ...

Chemistry check my answer?

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...

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) ...

Chemistry

H2S+Is >2HI+S

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 ...

chemistry

in a reversable reaction H2+I2=2HI,what will happen to the equilibrium if the volume is decrease?

chemistry

Considering the reaction i2 h2=2hi energy change =( tive) and give reasons how "HI" will be produced

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?

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?

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?

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?

chemistry

Assuming all gases are at the same temperature and pressure, how many milliliters of hydrogen iodide are produced from 165 mL of H2? H2(g)+I2(g)→2HI(g)

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.

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

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)

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.

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

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...

Chemistry

The delta G^o for a reaction : h2 (g) + i2 (g) = 2HI(g) Is 2.6 kj/moles. In one experiment the initial pressures are P h2 = 4.26 atm, P i2 = 0.024 atm,

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?

Help Chemistry!!!!!!!

For the reaction 2HI(g) <----> H2(g) + I2(g), Kc = 0.0198 at 721K. What is the HI concentration at 721K if [H2] = 0.120 M and [I2] = 0.0150 M? I'm getting .303 M but that's not one of the options.

Chemistry Help

For the reaction 2HI(g) <----> H2(g) + I2(g), Kc = 0.0198 at 721K. What is the HI concentration at 721K if [H2] = 0.120 M and [I2] = 0.0150 M? I'm getting .303 M but that's not one of the options.

Chemistry Help

For the reaction 2HI(g) <----> H2(g) + I2(g), Kc = 0.0198 at 721K. What is the HI concentration at 721K if [H2] = 0.120 M and [I2] = 0.0150 M? I'm getting .303 M but that's not one of the options.

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

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

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

Chemistry

For the following reactions, determine the equilibrium constant equation. 1) CO2(g) + H2(g) CO(g) + H2O(g) 2) 2NO(g) + 2H2(g) N2(g) + 2H2O(g) 3) Cu(s) + 2Ag+(g) Cu2+(g) + 2Ag(s) 4) H2(g) + I2(g) 2HI(g)

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?

chemistry

For the equilibrium: H2 + I2 <=> 2HI The equilibrium konstant Kc is equal to 50.5 at 448ºC. If [H2]o=[I2] o= 1 mol/l. What will the concentration of H2, I2 and HI be at equilibrium

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.

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...

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...

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...

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?

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)--->

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

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?

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?

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?

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?

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...

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.

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

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.

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)

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

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...

Chemistry

The delta G^o for a reaction : h2 (g) + i2 (g) = 2HI(g) Is 2.6 kj/moles. In one experiment the initial pressures are P h2 = 4.26 atm, P i2 = 0.024 atm, P hi = 0.23 atm. Calculate delta G

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!

chemistry

The decomposition of hydrogen iodide if the equation: 2HI (g)--> H2 (g) + I2 (g) The reaction is second order and has a constant rate equal to 1, 6X10^-3 L/mol * s at 700 degrees. If the initial HI concentration in a vessel is 3.4X10 ^-2m. How many minutes will it take for ...

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 ...

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)

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)

chemistry

In equation He +Br2------>2HI why chemical rate of Br2 is taken as 1/2 . It's a reversible reaction. Please explain in detail. While H2 rate is taken as 1 why?

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?

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-...

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?

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()

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...

Chemistry

A 2.00L flask was filled with 4.00 mol of HI at a certain temperature and given sufficient time to react. At equilibrium the concentration of H2 was 0.400 M. Find the equilibrium concentrations of I2 and HI and then find the Keq at this temperature 2HI(g) <-> H2(g) + I2(g)

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...

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...

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!

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)

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)----&...

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)----&...

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-

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 ...

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

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)----&...

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! :)

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 ...

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

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

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?

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...

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 ...

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...

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

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

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

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.

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 ...

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?

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....

Chemistry!!! PLZ PLZ HELP!!

Calculate the equilibrium amounts of each susbtance in the reaction below if an initial amount of 0.1 moles of H2 are brought together with an initial amount of 0.2 moles of I2 and then equilibrium is established at 900K. Kc at this temperature=70. H2 + I2 <-> 2HI

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...

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...

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...

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 ...

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 ...

Chemistry

Hello, I really don't understand how to find the grams of moles in some of these reactions. If someone could help I would appreciate it. 1) Balance the following chemical reaction and determine the number of moles of HI produced when 2.33 moles of H2(g) are consumed in the ...

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