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)

118,902 results

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.

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 this is suppose to be ...

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)

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 [H2O]=[CO]= 0.55mol/L a/ ...

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 of FeSCN 2+(aq) was 2....

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.

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.

Chemistry (please help me!)

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 a) What is the mole ...

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, the equilibrium ...

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 concentration of "B...

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 the concentration of ...

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 NO be after ...

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 equilibrium concentrations of...

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 occurs when Ba(OH)2 ...

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, what is the equilibrium ...

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 M Total solution ...

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 equilibrium ...

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 through the equilibrium ...

Chemistry

Consider the reaction CaSO4(s)rightleftharpoons Ca^2+(aq)+ SO_4^2-(aq) At 25 C the equilibrium constant is Kc = 2.4 \times 10^-5 for this reaction. If excess CaSO4(s) is mixed with water at 25C to produce a saturated solution of CaSO4, what are the equilibrium concentration of...

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 (pH=7) of aldolase? b.) ...

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 the equilibrium ...

Chemistry

consider the equation for the following reaction at equilibrium. X+Y<-->2Z+heat the concentration of the product could be increased by 1.adding a catalyst 2.adding more heat to the system 3.increasing the concentration of Y 4.decreasing the concentration of X

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 notation), and state ...

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 Experiment 3: [ClO2]0= 0....

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 no change was observed...

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 converted to products? I...

chemistry

Consider the following equation: N2O4(g)+ 2NO2(g) Kc= 5.8 x 10^-3 If the initial concentration of N2O4(g)= 0.040 M and the initial concentration of NO2(g) is 0 M, what is the equilibrium of concentration of N2O4(g)?

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. What is the ...

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. What is the ...

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) at equilibrium to 3 ...

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 is re-established?

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 one experiment, a ...

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

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

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 to 0.50 mol/L, what ...

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.

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.

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. I got 55.3...is that ...

chemistry

Consider the equation: 2NO2(g) N2O4(g). Using ONLY the information given by the equation which of the following changes would increase the molar concentration at equilibrium of the product N2O4(g)?

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 10-5 mol of B. Calculate...

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 equation to work out the...

Chemistry

1. Molarity is to moles of solute over liters of solution as molality is to A. molar concentration over molal concentration. B. moles of solute over kilograms of solvent. C. molal concentration over molar concentration. D. moles of solute over moles of solvent. 2. In ...

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% of NO is converted ...

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 that follow, consider ...

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

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 + 2H2 <---> N2 + ...

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

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 hope the formatting ...

Chemistry

Consider the reversible reaction: A(g)-2B(g)At equilibrium, the concentration of A is 0.381 M and that of B is 0.154 M. What is the value of the equilibrium constant, Keq?

chemistry

consider the following equilibrium. 4NH3(g) +3O2(g)<-> 2N2(g) + 6H2O(g) suppose 0.30mol of NH3 and 0.40mol of oxygen are added to a 5.0L container. If x mol of water is present at equilibrium, what is the equilibrium concentration of oxygen?

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 each form if the ...

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 equilibrium shift towards? I ...

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 equilibrium concentration of ...

Chemistry

Consider the gas-phase equilibrium A ⇌ B. In a series of experiments, different initial amounts of A and B are mixed together, and the mixture in each case is allowed to come to equilibrium. Which one of these experiments would yield values for the amounts of A and B ...

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 ion at equilibrium? c...

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) 0.80 M

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) 0.80 M

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 unit of concentration...

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 (3.63x10^-4) but I am ...

chemistry

n one experiment, a mixture of 1.000 mol acetic acid and 0.5000 mol ethanol is brought to equilibrium. A sample containing exactly one-hundredth of the equilibrium mixture requires 28.80mL 0.1040M Ba(OH)2 for its titration. Calculate the equilibrium constant, , for the ethanol...

Chemistry

At equilibrium, the concentrations in this system were found to be [N2] = [O2] = 0.100 M and [NO] = 0.500 M. N2(g) + O2(g) <-> 2NO(g) If more NO is added, bringing its concentration to 0.800 M, what will the final concentration of NO be after equilibrium is re-...

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 .

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 = (3.025)/(3.665)*(0.883)=1.21 Q...

Chemistry

N2 +O2 = 2NO has an equilibrium constant Keq of 0.10 mol/L @ 2000 degrees celcius. If the equilibrium concentration for NO is 0.40 mol/L and the equilibrium concentration for N2 is 0.80 mol/L, what is the equilibrium concentration of O2?

CHM 152

Consider the following equilibrium: PCl3 + Cl2 = PCl5 Kc=26 @ 250 degree Celcius 1.0 mol of PCl3 , 1.0 mol of Cl2 , and 5.0 mol of PCl5 are placed in a 10.0L flask at 250 C and allowed to come to equilibrium. What is the concentration, in M, of at equilibrium? Choose one ...

Chemistry

The following table contains data for the equilibrium reaction CH3COOH(g)+ C2H5OH(g)↔ CH3COOC2H5(g)+ H2O(g) T = 100oC. Each row in the table represents a different experiment (diffferent intial concentrations). Initial concentration Equilibrium concentration...

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 concentrations of H2 & I2...

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 concentration of products over...

Chemistry

Consider the following equilibrium process at 686 C C02(g)+H2(g)=CO(g)+H20(g) The equilibrium concentration of the reacting species are [CO]=0.050M, [H2]=0.045M, [CO2]=0.086M, and [H20]=0.040M. (a)Calculate the Kc for the reaction at 686 C. (b) If we add CO2 to increase its ...

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 8.0 x 10^-3 M. ...

Chem

find pH of 0.050 M HCLO4 plus 0.050 M HBr> You must consider activities>

Chemistry

A sample of ammonia gas was allowed to come to equilibrium at 400 K. 2NH3(g) --> N2(g) + 3H2(g) At equilibrium, it was found that the concentration of H2 was 0.0584 M, the concentration of N2 was 0.0195 M, and the concentration of NH3 was 0.430 M. What was the initial ...

Science

If 1 mole of acetic acid and 1 mole of ethyl alcohol are mixed and reaction proceeds to equilibrium, the concentration of acetic acid and water are found 1/3 and 2/3 mole respectively. If 1 mole of ethyl acetate and 3 mole of water are mixed,how much ester is present when ...

Chemistry

Consider the gas-phase equilibrium A ⇌ B. In a series of experiments, different initial amounts of A and B are mixed together, and the mixture in each case is allowed to come to equilibrium. Which one of these experiments would yield values for the amounts of A and B ...

Chemistry

EQUILIBRIUM: To prepare the standard solution, a very large concentration of ferric ion is added to a small initial concentration of thiocyanate ion. True or False It would help if we knew what you were doing. We are determining Chemical Equilibrium: Finding a Constant Kc... ...

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 concentrations of the two ...

chemistry

Wrtie the equilibrium constant expression for the reaction of NH3 with water. the OH- concentration of .050 M ammonia, NH3, is 9.5 x 10^-4 M

Chemistry

Which of the following solution should be mixed with 50.0 mL of 0.050 M HF solution to make an effective buffer? A) 50.0 mL of 0.10 M NaOH B) 25.0 mL of 0.10 M NaOH C) 50.0 mL of 0.050 M NaOH D) 25.0 mL of 0.050 M NaOH

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 H2 is 3.00 mol/L, the...

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 H2 is 3.00 mol/L, the...

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 H2 is 3.00 mol/L, the...

chemistry

during an experiment, 20 ml of 4 M hydrochloric acid is mixed with 30 ml of water. what is the concentration of your new solution

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

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

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, and equilibrium ...

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, and equilibrium ...

Ciollege algebra

Suppose that X liters of 38% acid solution are mixed with y liters of a 42% solution to obtain 100L of a 39% solution. One equation in a system for solving this problem is x+y=100. Which one of the following is the other equation? A. 42x+38y=0.39*100 B 0.38x+0.42y=0.39*100 C. ...

chemistry

At 2010K, the equilibrium constant Kc is 4*10^-4 for the following: N2+O2-->2NO If the equilibrium concentration of N2 is .28M and O2 is .38M, what is the equilibrium concentration of NO? a)1.8*10^-9 b)2.1*10^-5 c)4.3*10^-5 d)6.5*10^-3

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, and equilibrium ...

Chemistry

At a high temperature, the equilibrium constant for the decomposition of hydrogen iodide is 65.0. If the initial concentration of HI is 1.60 M, what is the concentration of hydrogen at equilibrium? 2Hl(g) H2(g) + I2(g) A. 1.42 M B. 0.753 M C. 0.240 M D. 0.802 M I think that ...

Chemistry

If there were two solutions- one with areagent(100% pure) mixed in water and the other solution containing the same reagent (99.9% pure) mixed in equal volume of water. How significant would the difference in concentration be between these two solutions?

chemical equilibrium

At a certain temperature, Kc = 0.914 for the reaction NO2 (g) + NO (g) <----> N2O (g) + O2 (g) Equal amounts of NO and NO2 are to be placed in a 5.00 L container until the N2O concentration at equilibrium is 0.050 M. How many moles of NO and NO2 must be placed in the ...

English

I would like to know if this grammatically correct. When there is change in reactant, product, and temperature the equilibrium position will shift in a direction that tends to decrease that change in situations. When the concentration of one of the products of an equilibrium ...

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 concentrations in mol/L ...

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 and adding enough ...

Chemistry - Ksp

i did an experiment where we titrated HCl on calcium hydroxide, and now i am confused with the calculations, i do not know if i am correct, so please help me out... Trial One volume of HCl used - 11.20mL concentration of HCl - 0.04mol/L so to get moles of HCl i used M= CV is ...

Chemistry

1. Write the balanced equation. Use ONLY this equation to reference how the reactions below will shift. Consider whether there is an addition, a removal, or no effect to the reaction. Co(H2O)6^2+ + 4Cl^- <--> CoCl4^2- + 6H2O 2. Write the equilibrium expression for the ...

Chemistry

when Fe(NO3)3 and KNCS were mixed they reacted together to establish an equilibrium with FE(NCS)+2. what are the changes in terms of quotient Q when the solutions were just mixed (no reaction), to the point where equilibrium is reached.

Math

(.050-2ƒÎ/(ã6.18))/(2ƒÎ/(ã6.18))*100 I think the answer is 5 because everything cancels out except the .050*100 is this right?

Chemistry

Consider the following buffer equilibrium: HF (high concentration) + H2O <--> H3O+ (low concentration) + F- ( high concentration) Using Le Chatelier's Principle, explain what happens to the pH of the buffer solution when a small amount of NaOH is added. Wouldn't OH- ...

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