# The equilibrium constant (Keq) is the ratio of ____ concentrations to ____ concentrations at equilibrium, with each concentration raised to a power equal to the number of ____ of that substance in the balanced chemical equation

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1. ## Chemistry

The equilibrium constant (Keq) is the ratio of ____ concentrations to ____ concentrations at equilibrium, with each concentration raised to a power equal to the number of ____ of that substance in the balanced chemical equation.
2. ## Chemistry

Consider the equilibrium 2NOCl (g) <---> 2NO (g) + Cl2 (g). In a 1 L container @ equilibrium there are 1.0 mol NOCL, 0.70 mol NO, and 0.40 mol Cl2. @ constant temperature and volume, 0.10 mol NaCl is added. What are the concentrations in the "new"
3. ## Chemistry

The equilibrium constant, Keq, is defined as the ratio of the concentrations of products to reactants. What is the equilibrium constant for the following reaction: ClNO2 (g) + NO (g) ↔ NO2 (g) + ClNO (g)
4. ## Chemistry

X2 + Y2 <=> 2XY 0.50 mole each of X2 and Y2 are placed in a 1.0 litre vessel and allowed to reach equilibrium at a given temperature. The equilibrium concentrations of XY is found to be 0.025 mol/L. What is the equilibrium cosntant for this reaction?
5. ## chem

What is constant about the equilibrium constant? A. The reversibility of the reaction at equilibrium is constant. B. The ratio of products to reactants at equilibrium is constant. C. The concentrations of products present at equilibrium are constant. D.
6. ## chem

For the equilibrium reaction: CO(g)+H2O(g)<=>CO2(g)+H2(g) the Keq value at 690°C is 10.0. A mixture of 0.300 mol of CO, 0.300 mol of H2O, 0.500 mol of CO2 and 0.500 mol of H2 is placed in a 1.0 L flask. a)Write the Keq expression for this reaction
7. ## CHEM

For the equilibrium reaction Co(g)+H2O(g)<=>CO2(g)+H2(g) the Keq value at 690°C is 10.0. A mixture of 0.300 mol of CO, 0.300 mol of H2O, 0.500 mol of CO2 and 0.500 mol of H2 is placed in a 1.0 L flask. a) Write the Keq expression for this reaction
8. ## chemistry

For the reaction H2(g) + I2(g) ↔ 2 HI(g), you have the initial concentrations [H2] = 0.15 and [I2] = 0.05. Keq for the reaction at this temperature is 4.5 x 10-6. Make a reaction table. Include rows for initial concentration, change in concentration,
9. ## chemistry

For the reaction H2(g) + I2(g) ↔ 2 HI(g), you have the initial concentrations [H2] = 0.15 and [I2] = 0.05. Keq for the reaction at this temperature is 4.5 x 10-6. Make a reaction table. Include rows for initial concentration, change in concentration,
10. ## chemistry

For the reaction H2(g) + I2(g) ¡ê 2 HI(g), you have the initial concentrations [H2] = 0.15 and [I2] = 0.05. Keq for the reaction at this temperature is 4.5 x 10-6. Make a reaction table. Include rows for initial concentration, change in concentration,
11. ## chm

The equilibrium constant for the equation 2 H2(g) + CO(g) CH3OH(g) Is 19 at a certain temperature. If there are 3.11 x 10-2 moles of H2 and 5.79 x 10-3 moles of CH3OH at equilibrium in a 6.75 L flask. What is the concentration of CO? At 1280 °C the
12. ## chem

Given the concentrations, calculate the equilibrium constant for this reaction: I2(g) + Cl2(g)---> 2ICl(g) At equilibrium, the molar concentrations for reactants and products are found to be I2 = 0.50M, Cl2 = 0.60M, and ICl = 5.0M. What is the
13. ## chemistry

A reaction is represented by this equation: 2W( aq ) ⇌ X( aq ) + 2Y( aq ) K c = 5 × 10 −4 (a) Write the mathematical expression for the equilibrium constant. (b) Using concentrations of ≤1 M , make up two sets of concentrations that
14. ## chemistry

A reaction is represented by this equation: 2W( aq ) ⇌ X( aq ) + 2Y( aq ) K c = 5 × 10 −4 (a) Write the mathematical expression for the equilibrium constant. (b) Using concentrations of ≤1 M , make up two sets of concentrations that
15. ## CHEMISTRY

A chemist studying the equilibrium N2O4(g)<----->2NO2(g) controls the temperature so that keq ( equilibrium constant)= 0.028. At one equilibrium position, the concentration of N2O4 is 1.5 times greater than the concentration of NO2. Find the
16. ## "le Chat. principle".

Hey, can you check this, this is regarding "le Chat. principle". Thanks! #1) The value of the equilibrium constant for the reaction H2CO3(aq) + energy >>> H2O(l) + CO2(g) can be changed by introducing a change to which component of the equation?
17. ## Chemistry

For the following reaction at a certain temperature: 2( ) 2( ) ( ) 2 H F HF g g g +  it is found that the equilibrium concentrations in a 5.00 L rigid container are [H2]=0.0500 M, [F2]=0.0100 M, and [HF]=0.400 M. If 0.200 mol F2 is added to this
18. ## Chemistry

For the reaction below at a certain temperature, it is found that the equilibrium concentrations in a 5.00 L rigid container are [H2] = 0.0500 M, [F2] = 0.0100 M, and [HF] = 0.400 M. If 0.340 mol of F2 is added to this equilibrium mixture, calculate the
19. ## chemistry

For the reaction below at a certain temperature, it is found that the equilibrium concentrations in a 4.87-L rigid container are [H2] = 0.0496 M [F2] = 0.0116 M [HF] = 0.429 M. H2(g) + F2(g) <==> 2 HF(g) If 0.185 mol of F2 is added to this
20. ## chemistry

For the following reaction at a certain temperature, it is found that the equilibrium concentrations in a 5.00 L rigid container are [H2] = 0.0500 M, [F2] = 0.0100 M, and [HF] = 0.400 M. If 0.261 mol of F2 is added to this equilibrium mixture, calculate
21. ## Chemistry

Consider the equilibrium 2NO (g) <---> 2NO (g) + Cl2 (g). In a 1 L container @ equilibrium there are 1.0 mol NOCL, 0.70 mol NO, and 0.40 mol Cl2. @ constant temperature and volume, 0.10 mol NaCl is added. What are the concentrations in the "new"
22. ## chemistry

200g of HOCl is placed inside a 3L container and allowed to reach equilibrium. Find the equilibrium concentrations for all species. Given: 2HOCL (g) <--> H20 (g) + Cl20 (g) when Delta H = +56 kJ and Keq = 11.11 at 25 C
23. ## chemistry

please help and explain. At a certain temperature, Keq = 10.5 for the equilibrium below. CO(g) + 2 H2(g) equilibrium reaction arrow CH3OH(g) Calculate the following concentrations. (b) [H2] in an equilibrium mixture containing 1.01 mol/L CO and 0.335 mol/L
24. ## chemistry

At a certain temperature, Keq is 4.13 x 10^-5 for the equilibrium: 2IBr(g) ↔ I2(g) + Br2(g) Assume that the equilibrium is established at the above temperature by adding only the reactant to the reaction flask. What are the concentrations of I2 and
25. ## Science

A chemist is studying the following equilibrium: 2Pb(NO3)2 (s) ! 2PbO (s) + 4NO2 (g) + O2 (g) He starts out with 10 g of Pb(NO3)2 and, at equilibrium, has 2.02 g of PbO. The concentrations of NO2 and O2 at equilibrium are 0.25 M and 0.019 M, respectively.
26. ## Equilibrium

An aqueous solution of carbonic acid reacts to reach equilibrium as described below. H2CO3(aq) + H2O(l) <---> HCO3^-(aq) + H3O^+(aq) The solution contains the following solute concentrations: Carbonic Acid: 3.3*10^-2 mol/L HCO3^-: 1.19*10^-4 mol/L
27. ## Chemistry, equilibrium molarity

At a particular temperature, K=3.75 for the following reaction. SO2(g) + NO2(g) (reversible arrows) SO3(g) + NO(g) If all four gases had initial concentrations of 0.500 M, calculate the equilibrium concentrations of the gases. This is what I've done so
28. ## chemistry

Consider the equilibrium, A + B <--> C, with K=32.217 and initial concentrations of A,B, and C, of 3.665M, 0.883M, and 3.925M, respectively. What is the equilibrium concentration of B 3.665 0.883 3.925 A + B = C Keq=(C)/(A)*(B)= 32.217 Q =
29. ## Chemistry

Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of SO2(g). 2SO2(g)+O2(g)=2SO3(g) Kc=1.7*10^8 [SO3]aq=0.0034 M [O2]aq=0.0018 M
30. ## Chemistry

At a particular temperature, K=3.75 for the following reaction. SO2(g) + NO2(g) (reversible arrows) SO3(g) + NO(g) If all four gases had initial concentrations of 0.500 M, calculate the equilibrium concentrations of the gases. K=(.5+x)^2/(.5-x^2) solve for
31. ## College Chemistry

Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of SO2(g). 2SO2(g)+O2(g)=2SO3(g) Kc=1.7*10^8 [SO3]aq=0.0034 M [O2]aq=0.0018 M
32. ## chemistry

For the reaction 2A(g) + B(aq) + 3C(l)<------> D(s) + 3E(g), the concentrations at equilibrium are found to be: A: 2.3x10^3 Pa B: 1.8x10^-2 M C: 15.8M D: 12.5M E: 5.6x10^4 Torr Find the numerical value of the equilibrium constant that would appear in

Just made it a new post didn't what it to get overcrowning.I hope this will help us figure out now For questions #1 through #10, refer to the following equilibrium system, with a Kc of 1.23E-03: C3H6O (aq) + 2C2H6O(aq)----> C7H16O2 (aq) + 2H2O (l) 1.
34. ## Chemsitry

For the following equilibrium process: CO2 + H2 = CO + H2O The equilibrium concentrations of reacting species are: [CO]= .050 M; [H2]= .045 M; [CO2]= .086 M; [H2O]= .040 M. (a) Calculate Kc for the reaction (b) If we add CO2 to increase its concentration
35. ## equilibrium question

For the reaction N2(g)+o2(g)<-->2NO(g), you have the initial concentration [N2]=0.03 and [O2]=0.08 Keq for the reaction at this temperature is 5.7*10^-5. What are the equilibrium concentrations for N2, O2, and NO? Please help me with this!
36. ## 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
37. ## chem

a.) At equilibrium, the molar concentrations for reactants and products are found to be [I2] = 0.50 M,[Cl2] = 0.60 M, and [ICl] = 5.0 M. What is the equilibrium constant (Kc) for this reaction? b.) The concentration of I2 is increased to 1.5 M, disrupting
38. ## Chemistry

Consider the following reaction. CaSO4(s) reverse reaction arrow Ca2+(aq) + SO42-(aq) At 25°C the equilibrium constant is Kc = 2.4x10^-5 for this reaction. (a) If excess CaSO4(s) is mixed with water at 25°C to produce a saturated solution of CaSO4, what
39. ## Chemistry

The equilibrium constant is equal to 5.00 at 1300K for the reaction 2SO2(g) + O2(g) <--> 2SO3(g) if initial concentrations are [SO2] = 6.00M, [O2] = 0.45M, [SO3]= 9.00M, the system is a/. At equilibrium b/. Not at equilibrium and will remain in an un
40. ## 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)
41. ## Chemistry

At 1285°C, the equilibrium constant for the reaction Br2 (gas) <---> 2Br (gas) is Keq= 1.04 X 10^ -3 A 0.200-L vessel containing an equilibrium mixture of gases has 0.245 g. Br2 (gas) in it. What is the mass of Br (gas) in the vessel? What are the
42. ## Chemistry

At room temperature, 80.0 ml of 0.125 M AgNO3(aq) and 20.0 ml of 0.500 M Fe(NO3)2(aq) are mixed together, generating the following equilibrium system Ag+ (aq) + Fe2+(aq) Ag(s) + Fe3+(aq). At equilibrium, the concentration of Fe3+ is 0.00505 M. (a) (4 pts)
43. ## Science

The following reaction: 2SO3 (g) ! 2SO2 (g) + O2 (g) has an equilibrium constant equal to 0.23 M. If the following concentrations are present: [SO2] =0.480 M, [O2] = 0.561 M, [SO3] = 0.220 M, is the reaction at equilibrium? If not, which way must it shift
44. ## Chemistry

An equilibrium mixture of SO2, O2, and SO3 at 1000 K contains the gases at the following concentrations: [SO2] = 3.77 10-3 mol/L, [O2] = 4.30 10-3 mol/L, and [SO3] = 4.13 10-3 mol/L. Calculate the equilibrium constant, K, for the following reaction. 2
45. ## chemistry

Chloroacetic acid has a relatively large equilibrium constant, so at low acid concentrations it is necessary to use the quadratic equation in order to calculate the concentrations of the aqueous species. Ka for ClCH2COOH is 1.4 ´ 10-3. For the problems
46. ## Chemistry

Consider this equilibrium process at 686°C. CO2(g) + H2(g) CO(g) + H2O(g) The equilibrium concentrations of the reacting species are [CO] = 0.050 M, [H2] = 0.045 M, [CO2] = 0.086 M, and [H2O] = 0.040 M. (a) Calculate Kc for the reaction at 686°C. (b) If
47. ## math

Write the first six terms of each of the sequences whose nth term is a)(-3)n { ____, ____, ____, ____ , ____, ____ } b)3 – 4n { ____, ____, ____, ____ , ____, ____ }
48. ## Chemistry

SO this is my first time doing this... lol i need help on an AP chemistry question for equilibrium. A 0.500 L tank contains 3.00 g of NO(g) at 750. K. The equilibrium constant for the reaction below at this temperature is 3.4 x 10 -3 2NO(g) ⇌ N2(g) +
49. ## chemistry

I have gotten the equilibrium concentrations of N202 to be 2M and N02 to be 2M also. After equilibirum is reached, a pistons is used to decrease the flask volume to 3L. Once equilibrium is established find the concentration and moles of each gas. K = 2 How
50. ## college chem

When the following reaction reaches equilibrium, the concentrations are 2.26 M A, 0.50 M B, and 2.00 M C. Calculate the equilibrium constant. A+2B<=====>3C
51. ## 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?
52. ## 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?
53. ## Chem 101

At 600degrees Celcius, gaseous CO and Cl2 are mixed together in a 1.00 L closed container. At the instant they are mixed, their concentrations are CO=.25 mol/L and Cl2= .69 mol/L. After equilibrium is established, their concentrations are CO= .25 mol/L and
54. ## CHEMISTRY

Find the equilibrium constant. 1. The equilibrium constant for the reaction,! Fe3+ + SCN- ⇋ FeSCN2+ (at a specific temperature), can be determined by first preparing a standard solution of FeSCN2+ and comparing its absorbance of light to an
55. ## Chemistry

C(g) + 2A(g) ⇌ 3E(s) + 2F(g) The concentrations of C, A, and F are measured as 0.2 M, 0.2 M, and 0.4 M at equilibrium and at 100 K. What is the value of the equilibrium constant?
56. ## Chemistry

C(g) + 2A(g) ⇌ 3E(s) + 2F(g) The concentrations of C, A, and F are measured as 0.2 M, 0.2 M, and 0.4 M at equilibrium and at 100 K. What is the value of the equilibrium constant? a. 25 b. 20 c.10 d. 15
57. ## 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
58. ## 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?
59. ## chemistry

for the reaction S2F6 (g) 2SF2(g), the equilibrium concentrations are as follows: [S26]=0.000430M, [SF2]=2.08 M, [F2]=1.32M. the equilibrium constant is
60. ## Chemistry

Find the equilibrium constant. 1. The equilibrium constant for the reaction,! Fe3+ + SCN- ⇋ FeSCN2+ (at a specific temperature), can be determined by first preparing a standard solution of FeSCN2+ and comparing its absorbance of light to an
61. ## Science (Chemistry)

4. A Beer’s Law plot was prepared for the reaction A(aq) + B(aq) AB(aq), plotting absorption over AB(aq) concentration. The linear equation for this plot was y = 78.3x. A solution was prepared by mixing 10.0mL of 0.100M A with 5.00mL of 0.100M B
62. ## Chemistry

C(s) + H20(g)↔ CO(s) + H2(s) the equilibrium constant for this reaction is 4.251 x 10^-2 at 800 K. if the equilibrium concentration of H2O(g)is 0.1990 M, what are the concentrations of CO, H2, and C?
63. ## Chemistry

C(s) + H20(g)↔ CO(s) + H2(s) the equilibrium constant for this reaction is 4.251 x 10^-2 at 800 K. if the equilibrium concentration of H2O(g)is 0.1990 M, what are the concentrations of CO, H2, and C?
64. ## chemistry

Some hydrogen and iodine are mixed up at 229 degrees celsiusin a 1-L container. When equilibrium is established, the following concentrations are present: [HI]= 0.490M, [H2]=0.080M, and [I2]= 0.060M. If an additional 0.300 mol of HI is then added, what
65. ## Chem

The apparent equilibrium constant for the reaction A + B <==> 2C is Kc= 4.11 at 298.2 K. Given that the initial concentrations of A, B, and C are .10M, .10M, and zero, respectively, find the equilibrium concentrations of A, B, and C. I had this long,
66. ## CHEMISTRY HELP DESPERATELY NEEDDED!!!

Given: N2O4 (g) « 2NO2 (g) @ 25 degrees celcius, Kc is 5.84 x 10^-3. (A) Calculate the equilibrium concentrations of both gases when 4.00 grams of N2O4 is placed in a 2.00 L flask at 25 degrees celcius. (B) What will be the new equilibrium concentrations
67. ## CHEMISTRY HELP STILL NEEDED PLEASE!!!

Given: N2O4 (g) « 2NO2 (g) @ 25 degrees celcius, Kc is 5.84 x 10^-3. (A) Calculate the equilibrium concentrations of both gases when 4.00 grams of N2O4 is placed in a 2.00 L flask at 25 degrees celcius. (B) What will be the new equilibrium concentrations
68. ## CHEMISTRY HELP NEEDED A.S.A.P

Given: N2O4 (g) « 2NO2 (g) @ 25 degrees celcius, Kc is 5.84 x 10^-3. (A) Calculate the equilibrium concentrations of both gases when 4.00 grams of N2O4 is placed in a 2.00 L flask at 25 degrees celcius. (B) What will be the new equilibrium concentrations
69. ## chemistry calculations

At 25 deg C, Kc is 5.84x10-3 for the dissociation of dinitrogen tetraoxide to nitrogen dioxide. N2O4(g) ==== 2NO2(g) a) Calculate the equilibrium concentration of both gases when 4.00 grams of N2O4 is placed at 2.00-liter flask at 25 deg C. b) What will be
70. ## chemistry

Given the equilibrium concentrations in the table, what is the equilibrium constant for the synthesis of ammonia at this temperature? 3H2(g) + N2 2NH3(g) A. 0.0035 B. 0.014 C. 0.066 D. 0.017
71. ## AP Chemistry

For the system 2SO2(g) + O2(g) <--> 2SO3 (g), change in enthalpy is negative for the production of SO3. At a particular temperature, 8.00 moles of sulfur dioxide and 10.00 moles of sulfur trioxide are introduced into a 2.00 L container. The system is
72. ## Chemistry

At 2000°C the equilibrium constant for the reaction is Kc = 2.4 ✕ 103. 2 NO(g) equilibrium reaction arrow N2(g) + O2(g) If the initial concentration of NO is 0.160 M, what are the equilibrium concentrations of NO, N2, and O2? I do not
73. ## AP CHEMISTRY

write the equilibrium-constant expression and calculate the value of the equilibrium constant for each of the following reactions at 298 K. (a) NaHCO3(s)<--> NaOH(s) + CO2(g) Answer: Keq = PCO2 (b)Value of the Equilibrium Constant: Please help me
74. ## Chemistry

Consider the reaction A+B->C+3D. A solution was prepared by mixing 50 ml of .001 M of A, 100 ml of .002 M of B, 10 ml of 1 M of C, and 75 ml of .0015 M of D. At equilibrium, the concentration of D was measured and found to be .0006 M. Calculate the
75. ## Chemistry

Consider the following reaction: CO(g)+2H2(g)⇌CH3OH(g) This reaction is carried out at a specific temperature with initial concentrations of [CO] = 0.27 M and [H2] = 0.49 M. At equilibrium, the concentration of CH3OH is 0.11 M. Find the equilibrium
76. ## Chemistry

The following system is at equilibrium,at 699K in a 5L container. H2(g)+I2(g)--->2HI(g) Kc = 54.9 Initially,the system had 2.50 moles of HI.What is the moles of H2 at equilibrium? Can Dr.Bob check if my steps are correct? My solution: Initially,the
77. ## Equilibrium

An equilibrium mixture at 852 K is found to contain 3.61*10^-3 mol/L of SO2, 6.11*10^-4 mol/L of O2, and 1.01*10^-2 mol/L of SO3. Calculate the equilibrium constant Keq, for the reaction where SO2 and O2 are reactants and SO3 is the product. Equation would
78. ## Calculus

Match the rule with the title: ____ 3. d/dx [f(x)/g(x) ]=(g(x) f^' (x)-f(x) g^' (x))/[g(x)]^2 ____ 4. d/dx [f(g(x))]=f^' (g(x))∙g'(x) ____ 5. d/dx [f(x)∙g(x)]= f(x) g^' (x)+g(x) f^' (x) ____ 6.d/dx [x]=1 ____ 7. d/dx [f(x)+g(x)]= f^' (x)+g^'
79. ## Chemistry

Question from text: "The reaction between phosphorus and chlorine is described by the equation, P4(s) + 6 Cl2(g) ↔ 4 PCl3(l). At equilibrium, the concentration of Cl2 is found to be 0.87 M. Calculate Keq." Keq = [PCl3]^4 / [P4] [Cl2]^6 I am not
80. ## chemistry

H2 + I2 <====> 2 HI. Looking for Keq: Complete the equation. Assume all concentrations are equilibrium constants in mol/L , M Temp in Celcius = 25 [H2] = .355 [I] = .388 [HI] = .0922 K eq = ??
81. ## chemistry

Which of the following is true of the solubility product constant? A. It is the product of the initial concentrations of the ions in a solution. B. It is an equilibrium constant. C. It is an equilibrium position. D. Its value changes in the presence of a
82. ## chemistry help

Which of the following is true of the solubility product constant? A. It is the product of the initial concentrations of the ions in a solution. B. It is an equilibrium constant. C. It is an equilibrium position. D. Its value changes in the presence of a
83. ## Chemistry12

For the reaction NO2 + NO = N2O3 If at a particular temperature, K was 575 and the equilibrium concentration of N2O3 was 2.5M, calculate the equilibrium concentrations of NO2 and NO if they both had the same initial concentrations. I have this information
84. ## chem, find concentrations

A 2 liter container holds 2.2 mol of NH3 gas, which starts to decompose according to the following reaction. At equilibrium there are .6 mol of H2. Determine the concentrations of NH3, H2, and N2 at equilibrium. 2NH3-> 3H2+N2 ^ all gas
85. ## Chemistry

For the reaction NO2(g) + NO(g) = N2O3(g) If at particular temperature, K was 575 and equilibrium concentration of N2O3(g) was 2.5 M, calculate the equilibrium concentrations of NO2(g) and NO(g) if they both had the same initial concentrations. i have my
86. ## Chemistry

Which of the following statements is a false statement concerning characteristics of chemical equilibrium? a. Equilibrium is dynamic. b. For a specific reaction at a specific temperature, the equilibrium state will be dependent of the direction of approach
87. ## chemistry

Which of the following statements is not true? 1.Chemical equilibria are examples of reversible processes. 2.When multiple reaction steps are in equilibrium, then the equilibrium constant for the net reaction is the product of the individual reactions.

I completed a lab to find the determination of Kc. I have to find the concentrations of reactants at equilibrium using an ICE table. The equation that were are using is Fe^3+(aq) + SCN^-(aq) -> Fe(SCN)^2+(aq) I have to create 5 ICE tables because we
89. ## Math - Magic Square???

My daughter is in 2nd grade and has a worksheet called Magic 26. It wants her to use the numbers 1 -12. Each row, column, and diagonal must equal 26. The four corners and four center numbers must equal 26 too. (example of puzzle below) Please help solve.
90. ## Chemistry(Please check, thank you!)

I completed a lab to find the determination of Kc. I have to find the concentrations of reactants at equilibrium using an ICE table. The equation that were are using is Fe^3+(aq) + SCN^-(aq) -> Fe(SCN)^2+(aq) I have to create 5 ICE tables because we
91. ## chemistry

How is the reaction quotient used to determine whether a system is at equilibrium? The reaction is at equilibrium when Q > Keq. At equilibrium, the reaction quotient is undefined. The reaction quotient must be satisfied for equilibrium to be achieved.
92. ## Chemistry

A l.00L flask contains 4.40mol of HI at a certain temperature. The Keq at this temperature is 5.0 * 10^-4. What are the concentrations of H2 and I2 at equilibrium?
93. ## chemistry

At 674.5 K the equilibrium concentrations of N2, H2, and NH3 were 0.1614 M, 0.1128 M, and 0.005892 M, respectively. What is the equilibrium constant for the reaction below? 2 NH3(g) → N2(g) + 3 H2(g)
94. ## 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
95. ## chemistry

following equilibrium system with a Kc of 1.23E-03: C3H6O (aq) + 2C2H6O (aq)--> C7H16O2 (aq) + 2H2O (l) 1.What is the equilibrium expression for this system? 2.If the molar concentrations of C3H6O2 and C2H6O are both 0.255 at equilibrium, what is the
96. ## Chemistry

The equilibrium constant, K, for the following reaction is 1.54×10-2 at 506 K: PCl5(g) PCl3(g) + Cl2(g) An equilibrium mixture of the three gases in a 15.7 L container at 506 K contains 0.207 M PCl5, 5.64×10-2 M PCl3 and 5.64×10-2 M Cl2. What will be
97. ## Chemistry

Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of H2O(g). C2H4(g) + H2O(g) C2H5OH(g) Kc = 9.0 × 103 [C2H4]eq = 0.015 M [C2H5OH]eq = 1.69 M
98. ## Chemistry 2!

consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of H2O(g) C2H4(g) + H2O(g) <--> C2H5OH(g) kc= 7.0* 10^3 [C2H4]= 0.010M [C2H5OH]= 1.99M
99. ## Chemistry

At 1473K the equilibrium constant for the reaction H2(g) + Cl2(g) <--------> 2HCl(g) Kc = 2.5*10^4. What would be the equilibrium concentration of HCL if the initial concentrations of H2 and Cl2 were 0.1840M and 0.1918M. I got 29.7 but was told it
100. ## chemistry

For the following reaction Co(g)+H2o(g)=Co2(g)+H2(g) If the initial concentrations of Co and H2o are 1.00 mol in a 50 L vessel, what is the number of mole of each species at equilibrium, if the equilibrium constant Kc= 0.85 at 1000 C? please can any one