
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.

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.

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 106. Make a reaction table. Include rows for initial concentration, change in concentration,

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 106. Make a reaction table. Include rows for initial concentration, change in concentration,

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 106. Make a reaction table. Include rows for initial concentration, change in concentration,


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

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?

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^'

Words to use: Accelerate  Sliding  Brake  Friction  Slipping  Inertia Velocity  Wheel  Strength  Static  Terminal velocity Questions 1. An object will ____?____ when the net force is not zero. 2. ____?____ will never speed up an object. 3. The

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

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"

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 102 moles of H2 and 5.79 x 103 moles of CH3OH at equilibrium in a 6.75 L flask. What is the concentration of CO? At 1280 °C the

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)

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

I am writing things that I do on the ship. Choose the correct verb (based on its meaning) to complete each sentence. A. Taco B. Nado C. Almuerzo D. Juego E. Escucho F. Miro. G. Abro H. Hablo I. Voy J. Como 1. ____ la musica. 2. ____ en la comedor. 3. ____


Fill in the sentences with adverbs. Do not repeat. 1.______ my friend and I _____ went _____. 2.We had _______ wanted to go ____, so we went _____ ______ and ____. 3. When we arrived _____, it was ____ dark, so we ____ went _____. 4. ____, we were ____ and

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.

Answer these questions: 1. What is s third of £18? 2. What is two thirds of £33? 3. What is three quarters of £42? 4 What is a quarter of £42? 5. What is a third of £42? Complete these statements: 6. ____ is a third of ____ 7. ____ is two thirds of

The value of the equilibrium constant (Kp) as represented by the first chemical equation is 2.00 x 102 at 730 K. Calculate the value of the equilibrium constant (Kp) for the second equation at the same temperature. Express answer in scientific notation.

7. ____ is two thirds of ____ 8. ____ is three quarters of ____ 9. ____ is a quarter of ____ 10. ____ is a third of ____

Put this in order ____ Constitutional Convention ____ Northwest Ordinance ____ Shays' Rebellion ____ Articles of Confederation ____ American Revolution end Please help

1) ____ of 50% = 45.5 2) ____ of 3 = 1.8 3) 56% of ____ = 3.92 4)69% of 30 = ____ 5)29% of ____ = 26.1 6) ____ of 20 = 6.2 7)82% of 10 = ____

23 _____ XXIII 44 ____ XLIV 52 ____ LII 17 ____ XVII 68 ____ LXVIII 99 XCIX 1,111 MCXI 575 DLXXV 946 ____ CMXLVI

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

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


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

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

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

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

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

Which of the following is a true statement about chemical equilibria in general A.there is only one set of equilibrium concentrations that equal the Kc value B.eqauilibrium is the result of cessation of all chemical change C.at equilibrium the rate of the

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 =

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?

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

____ kg = 440 g ((Help Please)) ____ kg 1,006,000 ((Help Please)) 8.6 kg = ____ g ((8600/0.0086??)) 800 g = ____ mg ((800.000??)) 1.7 kg = ____ ((1700/0.0017??)) ____ mg = 6.2 kg ((Help please)) (((((I understand it it's just I can't get a correct answer


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

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

Usa la forma presente de ESTAR con el participio pasado del verbo entre paréntesis para completar cada oración. Are these answers correct? 1. La maleta ya _____1.)____ ______2.)_______. (abrir) 1.) está 2.) 2.) abierto 2. ¿ ___(1)___ ___(2)___ todos

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)

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

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

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 ´ 103. For the problems

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

A researcher used an analysis of variance to compare three treatment conditions with a separate sample of n = 8 participants in each treatment. The results of the analysis are shown in the following summary. Fill in all missing values in the table. (Hint:

(Which indefinites correspond with the following words?) Please rewrite the following nouns preceded by the correct indefenido. 6. ____ primos 7. ____ apartamentos 8. ____ idioma 9. ____ naciones


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

Arrange the digits 5, 6, 7, 8, and 9 in the blanks to maximize the product. ___ ____ ____ x ____ ____

Complete the table of values for the function y = 4(1^x/2)^x: x 3 2 1 0 1 2 3 y ___ ____ _____ ____ ____ ____ __

Arrange the digits 5, 6, 7, 8, and 9 in the blanks to maximize the product. ___ ____ ____ x ____ ____

f(x) = (x^3+5x^228x32)/(x^318x^2+105x196) which can be written as f(x) = [(x+1)(x4)(x+8)]/[(x7)^2(x4) The domain of the function f(x), in interval notation from left to right, is ____ U ____ U ______. The root(s) of f(x), in increasing order,

. 3 gal = ____ qt. 22. 5 cups = ____ tsp 23. 15 lb = ____ kg 24. 150 ml = ____ Tbsp 25. 3 qt = ____ oz = _____ tsp

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

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!

Find the missing numbers to complete the patterns. Some are arithmetic and some are geometric. State the commom differences or common ratio. 1) 1,2,___,___,___,32 2)800,80,8,0,8,0.08,___,____ Some tricky ones that don't follow the "rules."

8. ____ is three quarters of ____ 9. ____ is a quarter of ____ 10. ____ is a third of ____


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

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

Answer the following questions to determine why Euler’s formula continues to hold for the polyhedron formed by cutting corners off of an octahedron, as in Figure 11.35(b): a. For an octahedron V = , ____,F = ____, and E = _____. b. When you slice off one

Find the formula for piecewise function f(x) = ____ if x < or equal to 1 ____ if 1 < x < or equal to 2 ____ if x > 2 Thanks! I got 1, x, and 2. Am I right?

Answer the following questions to determine why Euler’s formula continues to hold for the polyhedron formed by cutting corners off of an octahedron, : a. For an octahedron V = , ____,F = ____, and E = _____. b. When you slice off one corner of the

write the missing fraction or mixed number for each number line 0,1/3,2/3,1,____,____,____,______,2 1/3 3

For the reaction: H2(g) + I2(g) 2HI(g) , Kc = 12.3 at some temperature T. If [H2] = [I2] = [HI] = 3.21 x 103 M at this temperature, which one of the following statements is true? 1. ) Not enough information is given to answer the question. 2. ) The

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

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

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


For the reaction below at a certain temperature, it is found that the equilibrium concentrations in a 4.87L 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

name the states that the Chargers will fly over in route to their game in Jacksonville, ____,_____,_____,_____,____,_____,____, ____,____.

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)

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

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

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 1.23E03: C3H6O (aq) + 2C2H6O(aq)> C7H16O2 (aq) + 2H2O (l) 1.

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?

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?

A substance (CD) decomposes into C and D At the temperature of the experiment, 15.0% of CD is decomposed when equilibrium is established. a) if the initial concentration of CD is 0.200mol/L, what are the equilibrium concentrations of CD, C and D? I got

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


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

A spanish exchange student is trying to figure out what his friends like to eat. Provide the correct pronoun forms to complete his sentences below.: ____ gusta la comida china. A Patricia y a Juan ____ gusta la comida mexicana. ¿A vosotros ____ gusta la

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

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"

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

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/(.5x^2) solve for

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

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

Draw an arrow in the box that shows the direction of the force. Please help. I want to be sure. W > 0 W = 0 W < 0 ___ ____ ____ ___ ____ ____ d> d> d>

I am having trouble in calculating equilibrium concentrations. Where I get stuck will be at the end where I have to square root both sides and get the value of x to plug in the equation to get the individual concentration of every substance.


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] = 5.4x104 M and [I2] = 8.8x103 M, what is the equilibrium

11. The freezing point of a substance is ____ the melting point of the same substance. (1 point)greater than less than equal to unrelated to 12. For most substances, the distance between particles is smallest when the substance ____. (1 point)exists as a

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,

Are the pronouns I put down right? My answers are the ones in parentheses 1. The trip led to an argument between Helen and _____. (I) 2. It was ____ who demanded an apology from the newspaper. (us) 3. We appreciated ____ writing a personal letter to

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

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) +

¿Cuales artículos corresponden con las siguientes palabras? (Which articles correspond with the following words? Watch out for gender exceptions. Please rewrite the following nouns preceded by the correct article. 1. ____ perro 2. ____ ventanas 3. ____

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

I don't get it. I need to find out these conversions. 15,000 g= ____ kg 5,000 mL= ____ L 75 mL= ____ L 390 mL= ____ L 0.03 m= ____ mm 6 m= _____ mm 2.48 L= ______ mL 43.2 L= ______ mL 807 mL= _____ L 3,751 m= _____ km

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


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

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

At 1650 °C the value of Kc for the equilibrium represented by the balanced equation is 2.38 x 101. Calculate the value of Kp at the same temperature. Express answer in scientific notation. CO(g)+H2O(g) = CO2(g)+H2(g) ___ x 10 ____

At 25 deg C, Kc is 5.84x103 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 2.00liter flask at 25 deg C. b) What will be

I am not good at equations I need to complete this chart for this problem... y=1/2x4 X y (x,Y) __ 1 ____ 2 __ ____ __ 4 ____ 2 ___ ____ 8 ___ ____ I tried the first problem but I do not think it is correct.. y=1/2x4 x=1 y=1/2(1)4 = 3 1/2 that