# Consider the equation A(aq) + 2B(aq) 3C(aq) + 2D(aq). In one experiment, 45.0 mL of 0.050 M A is mixed with 25.0 mL 0.100 M B. At equilibrium the concentration of C is 0.0410 M. Calculate K. a) 7.3 b)

81,609 results
1. ## Chemistry

Consider the equation A(aq) + 2B(aq) 3C(aq) + 2D(aq). In one experiment, 45.0 mL of 0.050 M A is mixed with 25.0 mL 0.100 M B. At equilibrium the concentration of C is 0.0410 M. Calculate K.
2. ## chemistry

Consider the equation A(aq) + 2B(aq) 3C(aq) + 2D(aq). In one experiment, 45.0 mL of 0.050 M A is mixed with 25.0 mL 0.100 M B. At equilibrium the concentration of C is 0.0410 M. Calculate K. a) 7.3 b) 0.34 c) 0.040 d) 0.14 e) none of these the answer for

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
4. ## 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) +
5. ## 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
6. ## chemistry... HELPP

Chemistry Equilibrium Constant PLEASE Help!? In an experiment, equal volumes of 0.00150 M FeCl3 and 0.00150 M NaSCN were mixed together and reacted according to the equation: Fe3+ (aq) + SCN– (aq) <--> Fe(SCN)2+ (aq) The equilibrium concentration
7. ## AP CHEMISTRY

An experiment was carried out to determine the value of the equilibrium constant Kc for the reaction. Total moles of Ag+ present = 3.6 x 10-3 moles Total moles of NH3 present = 6.9 x 10-3 moles Measured concentration of Ag(NH3)2+ at equilibrium= 3.4* 10-2

Consider the following reaction: 2 HI (g) → H2 (g) + I2 (g) Assume that an experiment is carried out in which the starting concentration of HI (g) is 0.100 mol/L. No products are present at the beginning of the reaction. When equilibrium is established,
9. ## Chemistry``

A substance (CD) decomposes into C and D. CD(g)  C(g) + D(g) At the temperature of the experiment, 15.0 percent of CD is decomposed when equilibrium is established. a) If the initial concentration of CD is 0.200 mol/L, what are the
10. ## chemistry

When 10.0 mL of 0.012 M Pb(No3)2 is mixed with 10.0 mL of 0.030M KI, a yellow precipitate of PbI2(s) forms. a. Calculate the molarity of [Pb2+] b. calculate the initial molarity of [I-] c. On measuring the equilibrium concentration of [I-] it cam out to be
11. ## chemistry

a) The OH- concentration of 0.050 M ammonia, NH3, is 9.5x10^-4. Write the equilibrium equation for its ionization and the equilibrium constant expression; solve for the value of K.
12. ## chemistry

The OH- concentration of 0.050 M ammonia, NH3, is 9.5x10^-4. Write the equilibrium equation for its ionization and the equilibrium constant expression; solve for the value of K.
13. ## Chemistry

In the reaction, PCl3 + Cl2 ------> PCl5 the concentration of the reactants at equilibrium were each determined to be 7.2 mol/L, and the product at 0.050 mol/L. Calculate the equilibrium constant (rounding to 2 significant figures and using scientific
14. ## Chemistry

PLEASE fully explain these...I've already tried to figure them out and failed terribly... thanks so much 4. 5.6 x 10-6 mol of A and 5 x 10-5 mol of B are mixed in a 200 mL flask. The system is represented by the equation: At equilibrium, there is 4.8 x
15. ## Chemistry

1) Frank and Oswalt report a molar absorptivity of 4700 L mol^-1 cm^-1 for thiocyanatoiron(lll) ion. What absorbance would you expect for a soloution that it 1.0e-4 M in thiocyanatorion(lll) ion, if the path length is 1.00 cm? 2) At a given temperature,
16. ## chemistry

A mixture consisting of 0.150 M N2(g) and 0.612 M H2(g) reacts and then reaches equilibrium according to the equation: N2(g) + 3H2(g) ⇋ 2NH3(g) At equilibrium, the concentration of ammonia is 0.213 M. Calculate the concentration (molarity) of H2(g)
17. ## Physical Chemistry

A 100 amino acid folded protein (F) is in equilibrium with it’s unfolded (U) (or denatured) form. Let ΔrH(std) =+347 kJ mol-1 and ΔrS(std) =-1010 J K-1 mol-1 for the equilibrium (F U) at 25℃. (a) Calculate the concentration of protein in
18. ## Osciallations

A partridge of mass 5.01kg is suspended from a pear tree by an ideal spring of negligible mass. When the partridge is pulled down 0.100 m below its equilibrium position and released, it vibrates with a period of 4.20s . What is its speed as it passes
19. ## Chemistry

The pH of a weak monoprotic acid, HA, is 4.55. It took 39.22 ml of 0.2334 M NaOH to titrate 25.00 ml of the acid. a. Write an equation for the above reaction. b. Calculate the molarity of the weak acid c. Write the equilibrium equation. Construct a table
20. ## Chemistry

I'm supposed to calculate the rate equation, including k, for the reaction whose data is given in the table: Experiment: 1 2 3 Initial Concentration X: 0.10, 0.10, 0.60 Initial Concentration Y: 0.20, 0.10, 0.10 Measured Initial Rate: 2.57, 1.25, 1.27 (I
21. ## Chemistry

A(g) + B(g) <=> AB(g) At a given temperature 1.0 mole of A and 1.0 mole of B are placed in the 1.0 litre vessel and allowed to reach equilibrium. Analysis revealed that the equilibrium concenration of AB was 0.40 molar. What percent of A had been
22. ## Chemistry

At equilibrium, the concentrations in this system were found to be [N2]=[O2]=0.100 M and [NO]=0.500 M. The balanced chemical equation is N2+O2<--->2NO. If more NO is added, bringing its concentration to 0.800 M, what will the final concentration of
23. ## Chemistry

1. In an equilibrium, A + B ---> C + D; "A" & "B" are mixed in a vessel at temperature "T". The initial concentration of "A" was twice the initial concentration of "B", & after the equilibrium has reached, concentration of "C" was twice the equilibrium
24. ## Chemistry

3.0 moles each of carbon monoxide, hydrogen, and carbon are placed in a 2.0 liter vessel and allowed to come to equilibrium according to the equation: CO(g)+H2(g)-->C(s)+H20(g) if the equilibrium constant at the temperature of the experiment is 4.0,
25. ## 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
26. ## 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
27. ## chemistry

A mixture of 0.100 mol NO, 0.200 mol H2 and 0.0800 mol N2 were placed in a 2.00L reaction vessel, heated, and allowed to come to equilibrium conditions. At equilibrium, the molar concentration of N2 was 0.0500 mol/L. Calculate Kc for this reaction. 2NO +
28. ## chemistry 30 concentration of a product

calculate the concentration of the products of the following equilibrium when the equilibrium constant is 12.3 and the equilibrium concentration of nobr2 is 2.17 mol/l
29. ## AP Chem

NO2 + H2 <-> NO + H2O [H2] = .30 mol/L [NO2] = .20 mol/L [NO] = [H20] = .70 mol/L @ 1000K A. What is the mole fraction of NO in the equilibrium mixture? B. Calculate Kc C. Determine Kp in terms of Kc D. If system is cooled to a lower temperature, 35%
30. ## chemistry

Bromine gas is allowed to reach equilibrium according to the equation. Br2=2Br Kc=0.0011 at 1280°C Initial concentration of br2 is 0.063M and Br is 0.012M. How to calculate the concentration of these species at equilibrium. Please help me .
31. ## 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
32. ## Biochem

Assuming that the value of the equilibrium constant for the aldolase reaction Keq=6.43*10^-5 at pH=7 a.) What will be the equilibrium concentration of dihydroxyacetone phosphate (DHAP) if 1 mM of fructose-1,6-biphosphate is added to a buffered solution
33. ## chem 12

This is my question Into a 500mL container a chemist introduces 2.0 x 10^-2 mol of N2(g) and 2.0 x10^-2 mol of O2(g). The container is heated to 900degrees celcius and the following equilibrium is achieved. N2(g) + 2O2----N2O4(g) calculate the intial
34. ## chemistry

On this problem I keep getting the wrong answer. I am subtracting the initial concentration of Cl2 by the equilibrium concentration then using the difference to subtract for the rest using the mole ratios. Then i used the keq constant equation of
35. ## science

Acetic acid (CH_3COOH) is a weak acid. a) Write the symbolic equation showing the ionisation of acetic acid. b)Given that an acetic acid solution of pH 4.8 has a hydrogen ion concentration of 1.58 * 10^-5 mol L^-1, what is the concentration of the acetate
36. ## Chemistry

At 2000 ∘C the equilibrium constant for the reaction 2NO(g)←−→N2(g)+O2(g) is Kc=2.4×103. The initial concentration of NO is 0.220M . What is the equilibrium concentration of NO? What is the equilibrium concentration of N2? What is
37. ## Chemistry (reposts#6)

!A 100.0 mL aliquot of 0.200 M aqueous calcium hydroxide is mixed with ! 100.0 mL of 0.200 M aqueous aluminum nitrate. a.)! Write a complete molecular equation for this reaction, including phases b.)! Write a net ionic equation for this reaction, including
38. ## Chemistry

In one experiment, 50.0ml of 0.10M CH3NH2, is mixed with 20.00ml of 0.10 M CH3NH3Cl. The kb of CH3NH2 is 3.70*10^-4. a) write the chemical reaction for the equilibrium which becomes established, using H2O as a reactant. b)Write the net-ionic equation that
39. ## SI Chemistry

hydrogen chloride gas reacts with oxygen gas to yield chlorine gas and water vapor in an equilibrium reaction. an experiment was performed in a closed vessel starting with a mixture of 0.50 M HCl and 0.050 M O2. the amount of chlorine was monitored until
40. ## Chem

Estimate the equilibrium constant for the weak base (CH3)2NH, if a 1.59×10-2 M aqueous solution of (CH3)2NH has a pOH 2.58 (make an exact calculation assuming that initial concentration is not equal to the equilibrium concentration). (CH3)2NH + H2O =
41. ## pH

im trying to calculate the pH of a 1.0L soln containing 53.8 g of completely dissociated Mg(CN)2. is this the diss. equation? Mg(CN)2 + water --> MgOH + 2CN^- i don't think i did the problem rite b/c i got 15.7 for the pH. i got 53.8M Mg(CN)2 for the
42. ## Chem

A mixture of 2.5 moles of H2O and 100 g of C are placed in a 50.0 L container and allowed to come to equilibrium in the following reaction: C(s) + H2O(g)  CO(g) + H2(g) The equilibrium concentration of hydrogen gas is found to be 0.040 M.
43. ## Chemistry 30

A mixture of 2.5 moles of H2O and 100 g of C are placed in a 50.0 L container and allowed to come to equilibrium in the following reaction: C(s) + H2O(g)  CO(g) + H2(g) The equilibrium concentration of hydrogen gas is found to be 0.040 M.
44. ## Chemistry

i need help with a rate law question: The reaction is 2ClO2(aq) + 2OH -(aq)---> ClO3-(aq)+ ClO2-(aq) + H2O(l) Experiment 1: [ClO2]0= 0.0500 [OH-]0= 0.100 INITIAL RATE= 5.75*10^-2 Experiment 2: [ClO2]0= 0.100 [OH-]0= 0.100 INITIAL RATE= 2.30*10^-1
45. ## 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
46. ## Chemisty

For the reaction: 2NO(g) + H2(g) <=> N2O(g) + H2O(g) + energy Write the equilibrium constant expression for the reaction. This reaction takes place at 25°C. At this temperature the concentration of NO is found to be 1.75 mol/L, the concentration of
47. ## Science

For the reaction: 2NO(g) + H2(g) <=> N2O(g) + H2O(g) + energy Write the equilibrium constant expression for the reaction. This reaction takes place at 25°C. At this temperature the concentration of NO is found to be 1.75 mol/L, the concentration of
48. ## Chemisty

For the reaction: 2NO(g) + H2(g) <=> N2O(g) + H2O(g) + energy Write the equilibrium constant expression for the reaction. This reaction takes place at 25°C. At this temperature the concentration of NO is found to be 1.75 mol/L, the concentration of
49. ## chemistry

Equal volumes of 0.00150M FeCl3 and 0.00200M NaSCN were mixed together and reacted according to the equation: Fe3+ + SCN- <--> FeSCN2+ The equilibrium concentration of FeSCN 2+ was 1.40 x 10^-4 M Calclulate the equilibrium constant for the reaction.
50. ## 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)
51. ## SCIENCE

when 10.0 ml of .012 M PbNO32 is mixed with 10.0 ml of .030 M KI, a yellow precipitate of PbI2 forms. calculate the initial molarity of Pb+2 calculate the initial molarity of I- On measuring the equilibrium concentration of I-, it came out to be 8.0 x
52. ## Chemistry

Need help in AP chemistry on Equilibrium When heated, hydrogen sulfide gas decomposes according to the equation 2 H2S(g) ⇄ 2 H2(g) + S2(g) A 3.40 g sample of H2S(g) is introduced into an evacuated rigid 1.25 L container. The sealed container is
53. ## 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.
54. ## Chemistry

At equilibrium, the concentrations in this system were found to be [N2]=[O2]=0.100 M and [NO]=0.400 M. N2 (g) + O2 (g) --> 2NO (g) If more NO is added, bringing its concentration to 0.700 M, what will the final concentration of NO be after equilibrium
55. ## Chemistry

Calculate the thiocyanate concentration at equilibrium if the irone (III) ion concentration is 0.23 M and the complex ion concentration is 0.625 M t equilibrium. Keq= 138M^-1
56. ## chemistry

Calculate the thiocyanate concentration at equilibrium if the irone (III) ion concentration is 0.23 M and the complex ion concentration is 0.625 M t equilibrium. Keq= 138M^-1
57. ## Chemistry

Calculate the thiocyanate concentration at equilibrium if the irone (III) ion concentration is 0.23 M and the complex ion concentration is 0.625 M t equilibrium. Keq= 138M^-1
58. ## Chemistry

This question was posted: At 22 °C an excess amount of a generic metal hydroxide M(OH)2, is mixed with pure water. The resulting equilibrium solution has a pH of 10.56. What is the Ksp of the compound at 22 °C? I have found my [OH-] concentration
59. ## chemistry

A classic experiment in equilibrium studies dating from 1862 involved the reaction in solution of ethanol and acetic acid to produce ethyl acetate and water. The reaction can be followed by analyzing the equilibrium mixture for its acetic acid content. In
60. ## 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.
61. ## chemistry

How can i calculate the concentration of each ions remaining in the solution after precipitation is complete? ok heres the full question:: 2KOH + Mg(NO3)2 -------------> 2KNO3 + Mg(OH)2 a 100.0 mL aliquot of 0.200 M aqueous potassium hydroxide is mixed
62. ## Chemistry

How can i calculate the concentration of each ions remaining in the solution after precipitation is complete? ok heres the full question:: 2KOH + Mg(NO3)2 -------------> 2KNO3 + Mg(OH)2 a 100.0 mL aliquot of 0.200 M aqueous potassium hydroxide is mixed
63. ## Chemistry

How can i calculate the concentration of each ions remaining in the solution after precipitation is complete? ok heres the full question:: 2KOH + Mg(NO3)2 -------------> 2KNO3 + Mg(OH)2 a 100.0 mL aliquot of 0.200 M aqueous potassium hydroxide is mixed
64. ## chemistry

How can i calculate the concentration of each ions remaining in the solution after precipitation is complete? ok heres the full question:: 2KOH + Mg(NO3)2 -------------> 2KNO3 + Mg(OH)2 a 100.0 mL aliquot of 0.200 M aqueous potassium hydroxide is mixed
65. ## Chemistry

For the reaction: 2NO(g) + H2(g) <=> N2O(g) + H2O(g) + energy Write the equilibrium constant expression for the reaction. I wrote: [N2O][H2O] / [NO]2 [H2] This reaction takes place at 25°C. At this temperature the concentration of NO is found to be
66. ## Chemistry

5.6 x 10-6 mol of A and 5 x 10-5 mol of B are mixed in a 200 mL flask. The system is represented by the equation: 2A(g) + B(g) --> 3C(g) At equilibrium, there is 4.8 x 10-5 mol of B. Calculate the value of the equilibrium constant.

5.6 x 10-6 mol of A and 5 x 10-5 mol of B are mixed in a 200 mL flask. The system is represented by the equation: 2A(G) + B(G) <--> 3C(G) At equilibrium, there is 4.8 x 10-5 mol of B. Calculate the value of the equilibrium constant.
68. ## chemistry

2 HI(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 0.248 M. Calculate the concentration of HI in the equilibrium mixture. M.
69. ## Chemistry (solubility product question)

"When 3.00 ml of a 0.00600 M K2CrO4 solution and 3.000 ml of a 0.0100 M Cu(NO3)2 solution are mixed, some solid forms. The mixture is centrifuged and the supernatant is removed. The absorbance of the supernatant, measured at 400 nm in a 1.00 cm cuvette, is
70. ## AP Chemistry- Equilibrium

If 10.0 mL of 0.18 M MgCl2 are mixed with 20.1 mL of 0.56 M NaOH, what will be the final concentration of Mg2+ in solution when equilibrium is established? Assume the volumes are additive. Ksp = 1.2 ✕ 10-11 for Mg(OH)2.
71. ## AP Chemistry- Equilibrium

If 10.0 mL of 0.18 M MgCl2 are mixed with 20.1 mL of 0.56 M NaOH, what will be the final concentration of Mg2+ in solution when equilibrium is established? Assume the volumes are additive. Ksp = 1.2 ✕ 10-11 for Mg(OH)2.
72. ## chemistry

sulfur trioxide gas dissociates into sulfer dioxide gas and oxygen gas at 1250 degrees C. In an experiment, 3.6 moles of sulfur trioxide were placed into an evacuated 3.0-L flask. THe concentration of sulfur dioxide gas measured at equilibrium was found to
73. ## Chemistry

I have 3 Questions: We actually did the lab experiment for this, but I have no idea whether my reasons are correct. 1) For the equilibrium system Fe+3 + SCN- <--> FeSCN+2, what would happen if you add 2 drops of Fe No3?. Which way will the
74. ## Equilibrium Consentration

At a certain temperature, the reaction H2(g)+ Cl(g)=2HCl(g)has Kc = 5 x 10^8. If a reaction mixture at equilibrium contains 0.48 M of H2 and 0.23 M of Cl2, what is the concentration of HCl? I was wondering if I had to rearrange the equilibrium constant
75. ## AP Chemistry

CH3NH2(aq)+H2O(l)=>CH3NH3+(aq)+OH-(aq) Kb=4.4 x 10^-4 Methylamine, CH3NH2, is a weak base that reacts with water according to the equation above. A student obtains a 50.0 mL sample of a methylamine solution and determines the pH of the solution to be
76. ## chemistry

CH3NH2(aq)+H2O(l)=>CH3NH3+(aq)+OH-(aq) Kb=4.4 x 10^-4 Methylamine, CH3NH2, is a weak base that reacts with water according to the equation above. A student obtains a 50.0 mL sample of a methylamine solution and determines the pH of the solution to be
77. ## Chemistry``

I answered this question but I did not get the right answer. CO2 + H2 <=> H2O + CO CO2 = 0.5 mole and H2 he 0.5 mole both sollutions were forced into a 1 Litre container. K = 2 what is the equlibrium concentration of each reactant and product. as I
78. ## Chemistry

The reaction for the formation of gaseous hydrogen fluoride from hydrogen and fluorine has an equilibrium constant of 1.15x10^2 at a given temperature. In a particular experiment, 3.0 mol of each component was added to a 1.5 L flask. What is the
79. ## Chem

If you have an equation for a line, y = 0.15x + 0.010, where y is absorbance and x is concentration in molarity of Fe (2+), calculate the concentration of a test sample with an absorbance of 0.065. What is the absorbance value for the blank in this
80. ## Chemistry

0.25mol of CO are mixed with 0.90mol of H2 and heated to 950 degrees celcius in a 15L flask at equilibrium 0.190mol of H2O were present, what is the concentration of the other reactants and products at equilibrium and what is Kc
81. ## 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
82. ## chemistry

A system initially contains 0.100 mol each of the three species sealed in a 10.0 L container. The temp was raised to a temp where the equilibrium constant Kc, is 12.6 for PCl3(g) + Cl2(g)--> <-- PCl5(g) Calculate the equilibrium concentration of all
83. ## chemistry

A system initially contains 0.100 mol each of the three species sealed in a 10.0 L container. The temp was raised to a temp where the equilibrium constant Kc, is 12.6 for PCl3(g) + Cl2(g)--> <-- PCl5(g) Calculate the equilibrium concentration of all
84. ## chemistry

A chemical is placed in a beaker containing 20 g of soil and 500 mL of water. At equilibrium, the chemical is found in the soil at a concentration of 100 mg/kg of soil. The equilibrium concentration of this same chemical in the water is 250 µg/L.
85. ## chemistry

HCOOH(aq) <-----> H^+ (aq)+ HCOO^-(aq) The equilibrium constant (Ka) for Reaction 3 at 25 °C is 1.80 × 10−4 mol dm−3. Calculate the equilibrium concentration of hydrogen ions if the concentration of formic acid at equilibrium is 0.00500
86. ## Chemistry

Trying to figure out this equation I did the first part but I am really having trouble getting this one and my professor told me to re do it. Trying to calculate ke for the following equation (equilibrium concentration below problem) NO^2(g) + O^2(g) +
87. ## Chemistry

Trying to figure out this equation I did the first part but I am really having trouble getting this one and my professor told me to re do it. Trying to calculate ke for the following equation (equilibrium concentration below problem) NO^2(g) + O^2(g) +
88. ## chemistry

Trying to figure out this equation I did the first part but I am really having trouble getting this one and my professor told me to re do it. Trying to calculate ke for the following equation (equilibrium concentration below problem) NO^2(g) + O^2(g) +
89. ## 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
90. ## science

The equilibrium constant (Ka) for Reaction 3 at 25 °C is 1.80 × 10−4 mol dm−3. Calculate the equilibrium concentration of hydrogen ions if the concentration of formic acid at equilibrium is 0.00500 mol dm−3. (Show all of your working
91. ## chemistry

In an esterification experiment, 2.0 mol of ethanol were mixed with 1.0 mol of ethanoic acid in a container of volume 30cm3 and the chemicals were allowed to come to equilibrium at 25°, CH3CO2H + C2HOH <-> CH3COOC2H5 + H20 If the equilibrium mixture
92. ## Chemistry

My question is ..can anyone explain how to do problem #2? I feel lost. :( And could you also explain why? Problem#1, is that a regular dG = dH - TdS problem? Then using Go = -RTlnK to find K? Im just afraid if there are other seps to it.. 1. The combustion
93. ## 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
94. ## 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
95. ## 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.
96. ## Chemistry

What are the equilibrium concentrations of all the solute species in a 0.95 M solution of hydrogen cyanide, HCN? The Ka value = 6.2 x 10^-10. (a) [H3O+], M; (b) [OH-], M; (c) [HCN], M; (d) What is the pH of the solution? For HCN So far i have calculated
97. ## chemistry

For the equilibrium H2(g)+CO2(g)<-->H2O(g)+CO(g) Kc=3.18 at 1106 K.If each of the four species was initially present at a concentration of 3.000M,Calculate the equilibrium concentration of the CO (g) at this temperature. Choices 0.844 3.268 3.844
98. ## Chemistry

A student does a standard addition experiment by pipetting 25 mL of unknown, adding ferrous ion spikes and reagents, into a 100 mL volumetric flask and making up to the mark. The equation of the line has a slope of 0.103 and an intercept of 0.135 when the
99. ## Chemistry

0.80 mol/L of A and B are mixed. They react very slowly to produce C and D as follows: A(aq) + B(aq) ⇔ C(aq) + 2D(aq) When equilibrium is attained, the concentration of C is 0.60 mol/L and the concentration of A is: a) 0.20 M b) 0.40 M c) 0.60 M d)
100. ## Chemistry

0.80 mol/L of A and B are mixed. They react very slowly to produce C and D as follows: A(aq) + B(aq) ⇔ C(aq) + 2D(aq) When equilibrium is attained, the concentration of C is 0.60 mol/L and the concentration of A is: a) 0.20 M b) 0.40 M c) 0.60 M d)