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July 3, 2015

Search: h2 concentrations at equilibrium

Number of results: 4,974

CHEMISTRY
The equilibrium constant for the reaction, SO2(g)+ NO2(g) <----> NO(g)+ SO3(g) has been experimentally determined as a function of temperature. The results are presented in the table below. T (F) KC 285 662 752 156 842 93.4 932 59.6 1022 40.2 If 0.0791 ft3 SO2, 0.158 ...
March 24, 2011 by Josh

Chemistry
1. For the reaction 2N2O(g) ⇋ O2(g) + 2N2(g), what happens to the equilibrium position if the pressure decreases? A. Shift to the right B. Shift to the left C. Doubles D. Does nothing E. Halves 2. if an equilibrium reaction shifts to the right when the system is cooled, ...
October 16, 2012 by josh

Chem
Hi! I need help with this question: Sulfur dioxide reacts with chlorine at 227 oC: SO2(g) +Cl2(g) ↔ SO2Cl2(g) Kp for this reaction is 5.1 x 10-2 atm-1. Initially, 1.00 g each of SO2 and Cl2 are placed in a 1.00 L reaction vessel. After 15 minutes, the concentration of ...
February 20, 2013 by Anonymous

Chemistry
Ranking equilibrium constants from largest to smallest according to an image?Ethene (C2H4) can be halogenated by the following reaction: C2H4 (g) + X2 (g) -><- C2H4X2 (g) where X2 can be Cl2 (green), Br2 (brown), or I2 (purple). Examine the three figures below ...
February 8, 2012 by L.Bianchessi

Chemistry
At 25C, K = 0.090 for the following reaction. H2O(g) + Cl2O(g) equilibrium reaction arrow 2 HOCl(g) Calculate the concentrations of all species at equilibrium for the following case. 1.3 mol pure HOCl is placed in a 1.6 L flask [HOCl]________ [Cl2O]________ [H2O]________ ...
February 27, 2012 by Ann

Chemistry
Calculate the value of the equilibrium constant for the following reaction based on the given concentrations of reactants and products. N2 = 1.5 M, H2 = 0.5 M, NH3 = 2 M N2 (g) + H2 (g) ↔ NH3 (g)
November 11, 2014 by Tamera

Chem
4NH3(g) + 3O2(g) -> 2N2 + 6H20, K=10^80 @ certain temp initially, all the reactants and products have concentrations equal to 12M. At equilibrium, what is the approximate concentration of ammonia?
September 28, 2010 by Daniel

Chem
4NH3(g) + 3O2(g) -> 2N2 + 6H20, K=10^80 @ certain temp initially, all the reactants and products have concentrations equal to 12M. At equilibrium, what is the approximate concentration of ammonia?
September 28, 2010 by Daniel

Chem
4NH3(g) + 3O2(g) -> 2N2 + 6H20, K=10^80 @ certain temp initially, all the reactants and products have concentrations equal to 12M. At equilibrium, what is the approximate concentration of ammonia?
September 28, 2010 by Daniel

chemistry
For the reaction 4NH3(g) + 3O2(g) -> 2N2(g) + 6H2O(g) , K = 10^80 at a certain temperature. Initially, all reactants and products have concentrations equal to 12 M. What is the approximate concentration of ammonia at equilibrium? a. 3 M b. 12 M c. 18 M d. 6 M e. 0 M
February 9, 2011 by Eddy

Chemistry
How do I calculate the amount of grams of Na2HPO4 and NaH2PO4 to prepare 200 mL of a buffer with an 8.25 pH so the sum of the concentrations of HPO4 and H2PO4 ions is 0.5 M? Does this involve writing a Ka expression and equilibrium? I am confused and Thanks for your help!
March 11, 2012 by Carrie

Chemistry
How do I calculate the amount of grams of Na2HPO4 and NaH2PO4 to prepare 200 mL of a buffer with an 8.25 pH so the sum of the concentrations of HPO4 and H2PO4 ions is 0.5 M? Does this involve writing a Ka expression and equilibrium? I am confused and Thanks for your help!
March 11, 2012 by Carrie

chem
1) If more reactant is added to a gaseous reaction at equilibrium, what will happen to the value of the equilibrium constant? a. it will increase b. it will decrease c. it will remain the same d. it can either increase or decrease 2) Which of the following describes a property...
February 1, 2012 by HEATHER

Chemistry
At a particular temp, K = 1.6 x 10^-5 for the reaction: 2SO3(g) <-> 2SO2(g) + O2 (g) If 4 mol of SO2 and 2 mol of O2 are placed into a 2.0L flask, calculate the equilibrium concentrations of all species. I set up an ICE table with SO3 to start with 0M and SO2 to start ...
May 23, 2010 by Scott L.

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...
November 30, 2011 by Cody

chemistry
Gaseous CO2 decomposes to form the gaes CO and O2. At 20.0 degrees Celsius, =2.0*10^-8. 2.0 mol carbon dioxide is placed in a 5.0 L flask. What are the equilibrium concentrations of each species. My attempt to get the answer: Balanced equation: 2CO2--> 2CO+O2 To get the ...
March 1, 2009 by Anonymous

Chemistry
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.
March 18, 2008 by Rosa

biology,chemistry,physics
the contact process prepares purest form of sulphuric acid 2so2+o2=2so3 calculate its kp if following concentrations are found at equilibrium so2=0.59,o2=0.05 and so3=0.259
December 18, 2014 by Arooj

chemistry
If 1.00 mol of iodine and 0.50 mol of chlorine are initially placed into a 2.00 L reaction vessel at 25 degrees celsius, find the concentrations of all entities at equilibrium
April 7, 2008 by Kelsy

chemistry
A 0.239 mol sample of PCl5(g) is injected into an empty 2.85 L reaction vessel held at 250 C. Calculate the concentrations of PCl5(g) and PCl3(g) at equilibrium.
May 3, 2015 by layla

chemistry
I2(g)+Cl2(g)-><-2ICl(g) molar concentrations are I2=1.5M, Cl2=0.60M and ICl=5.0M calculate the ratio of products to reactants assume that the reaction has not yet regained equilibrium
June 7, 2015 by jennifer

Chemistry
Could someone explain the reasoning for this? 6) Which of the following is a false statement about ALL reactions in equilibrium? a) Increasing temperature shifts the reaction toward the products in an endothermic reaction b) Temperature effects on the equilibrium do not depend...
March 8, 2010 by Val

Chemistry
If the pH of a solution is 6, what are the hydrogen- and hydroxide-ion concentrations? The PH of a 0.1 M MCl (M+ is an unknown cation) was found to be 4.7. Write the net ionic equation for the hydrolysis of M+ and its corresponding equilibrium expression Kb. Calculate the ...
February 19, 2013 by Jefferson

chemistry
A diprotic acid solution H2A has a molarity of .95 M. the concentrations of the species present at equilibrium are as follows: [H+] = .25 M, [HA-]=.25M, [A^2-] =4.6x10^-4 M. what are the first and second ionization constants for this acid?
November 15, 2010 by Sam

chemistry
A 0.411 mol sample of PCl5(g) is injected into an empty 4.65 L reaction vessel held at 250 C. Calculate the concentrations of PCl5(g) and PCl3(g) at equilibrium.kc=1.80 at 250c
November 10, 2013 by muna

chemistry
Calculate each of these equilibrium concentrations based on the reaction below. 2 NO(g) + O2(g) 2 NO2(g) K = 1.71 1012 (a) [NO] = 0.0048 M; [O2] = 0.000057 M; [NO2] = ? (b) [NO] = 0.0026 M; [O2] = 0.000023 M; [NO2] = ?
September 12, 2011 by Anonymous

chemistry
Calculate each of these equilibrium concentrations based on the reaction below. 2 NO(g) + O2(g) 2 NO2(g) K = 1.71 1012 (a) [NO] = 0.0048 M; [O2] = 0.000057 M; [NO2] = ? (b) [NO] = 0.0026 M; [O2] = 0.000023 M; [NO2] = ?
September 12, 2011 by Anonymous

Chemistry
Consider the reaction below: 4NH3(g) + 3O2(g) -> 2N2 + 6H20, K=10^80 @ certain temp initially, all the reactants and products have concentrations equal to 12M. At equilibrium, what is the approximate concentration of oxygen?
May 23, 2010 by Scott L.

Chemistry
Consider the reaction below: 4NH3(g) + 3O2(g) -> 2N2 + 6H20, K=10^80 @ certain temp initially, all the reactants and products have concentrations equal to 12M. At equilibrium, what is the approximate concentration of oxygen?
May 23, 2010 by Scott L.

college chemistry
For the following reaction: PCl5(g)<===> PCl3(g) + Cl2(g) Kc=.058 If the initial concentration of PCl5(g) is .160M, calculate the equilibrium concentrations of all the components. (use quadratic)
March 24, 2010 by Jerrett

ap chem
At 350 K, Kc = 0.142 for the reaction 2BrCl(g) *) Br2(g) + Cl2(g) An equilibrium mixture at this temperature contains equal concentrations of bromine and chlorine, 0.067 mol/L. What is the equilib- rium concentration of BrCl? Answer in units of M.
February 13, 2011 by Anonymous

ap chemistry
At 350 K, Kc = 0.142 for the reaction 2BrCl(g) *) Br2(g) + Cl2(g) An equilibrium mixture at this temperature contains equal concentrations of bromine and chlorine, 0.069 mol/L. What is the equilib- rium concentration of BrCl? Answer in units of M
January 28, 2013 by cheri

science
At 472 deg C the reaction reaches equilibrium with the following composition: [H2]=7.38atm, [N2]=2.46atm, [NH3]=0.166atm. Into the equilibrium mixture 1.5 atm of N2 is introduced: a. Calculating Kp and Q, determine in which direction the reaction will proceed after addition of...
March 26, 2012 by kim

Chem
Determine the concentrations of K2SO4, K , and SO42 in a solution prepared by dissolving 2.84 104 g K2SO4 in 2.25 L of water. Express all three concentrations in molarity. Additionally, express the concentrations of the ionic species in parts per million (ppm). Note: ...
February 19, 2013 by Jhanvi

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! http://www2.ucdsb.on.ca/tiss/...
April 13, 2007 by Chrissy

chemistry
a mixture of 0.500 mol H2 and 0.500 mol I2 was placed in a 2.00-L stainless-steel flask at 430C. Calculate the concentrations of H2, I2, and HI at equilibrium
February 14, 2012 by tammie

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...
May 8, 2007 by Linda

Chemistry
A voltaic cell consists of Ag/Ag+2 electrode E= 0.80 and a Fe+2/Fe+3 electrode E=0.77 with the following initial molar concentrations: [Fe+2}= 0.30 M [Fe+3]= 0.10 M [Ag+]=0.30 M. What is the equilibrium concentration of Fe+3? (Assume the anode and the cathode solutions are of ...
July 20, 2012 by Jackie

chemistry
At 35C, Kc = 1.6 X 10-5 M for the reaction 2NOCI(g) 2NO(g) + Cl2 (g)' Calculate the concentrations of all species at equilibrium for each of the following systems. Note any simplifying assumptions made in the calculations. 3.0 mol NO(g) and 1.0 mol ofCl2(g) in a 1.0 L flask
December 6, 2014 by airman

AP Chem
At a particular temperature, K = 1.00 102 for the following reaction. H2(g) + I2(g) 2 HI(g) In an experiment, 1.23 mol H2, 1.23 mol I2, and 1.23 mol HI are introduced into a 1.00 L container. Calculate the concentrations of all species when equilibrium is reached.
January 8, 2012 by Bill

Chemistry
H2 (g) + I2 (g) 2 HI (g) If the initial concentrations of H2 and I2 are 1.0 M and the initial concentration of HI is 0.5 M (Kc = 54.3 at 430oC). (a) Is the reaction at equilibrium? (b) If not, which way will the reaction proceed?
May 4, 2014 by Troy

Chemistry
I posted this last night, A 0.500L vessel initially contains 0.0125 mol of H2S2 . Find the equilibrium concentrations of H2 and S2. Kc = 1.67 x 10^-7 2 H2S <--> 2 H2 + S2 I have come up with this equation so far, but I am lost now because I dont even know if this is ...
June 8, 2014 by Veronica

biochemistry
Reaction A B proceeds with H = 240 kJmol-1; S = 40 JK-1mol-1. Substance A was taken at initial concentration 2 mM. Determine the concentrations of A and B after the reaction reaches equilibrium at 298 K.
September 14, 2011 by Anonymous

Chemistry
What are the concentrations of Cu^2+, NH3, and Cu(NO3)4^2+ at equilibrium when 18.8 g of Cu(NO3)2 is added to 1.0 L of a .400 M solution of aqueous ammonia? Assume that the reaction goes to completion and forms Cu(NH3)4^2+.
March 17, 2015 by Jamila

Chemistry
Consider the following equilibrium: 2HI(g) *are in equilibrium with* H2(g) = I2(g) Keq = 81.0 A 2.00L container is initially filled with 4.00 mol HI. Calculate the [HI] at equilibrium. *I don't know how to put the equilibrium sign on the computer* Can someone please explain to...
November 12, 2014 by katie

Chemistry
At a particular temperature, K = 2.0 10-6 mol/L for the following reaction. 2 CO2(g) 2 CO(g) + O2(g) If 1.8 mol CO2 is initially placed into a 5.9-L vessel, calculate the equilibrium concentrations of all species.
February 20, 2012 by Elizabeth

chemistry
Why do the concentrations of Pb 2+ and SO4 2- ions in a saturated solution of PbSO4 in contact with solid PbSO4 remain the same when the solution evaporates to half of its original volume? it has to do with equilibrium.
March 28, 2012 by alex

Chem
Consider 1.40 mol of carbon monoxide and 3.20 mol of chlorine sealed in a 8.00 L container at 476 oC. The equilibrium constant, Kc, is 2.50 (in M-1) for CO(g) + Cl2(g) ↔ COCl2(g) Calculate the equilibrium molar concentration of CO. So I tried this question by finding the...
February 12, 2013 by Anonymous

chemistry
What are the equilibrium concentrations of H+,OH- ,(HSO3)-, (SO3)2- and Na+ in the solution that results from combining 50.0 mL of 0.200 M NaHSO3 with 50.0 mL of 0.600 M Ba(OH)2 ? Ka1 = 1.5 x 10-5 and Ka2 = 1.0 x 10-7 for H2SO3 does it matter that Ba(OH)2 has 2 OH's?When ...
August 3, 2008 by alexis

bioelectricity
Cl equil-v: Only chloride may cross a membrane separating two compartments. At a temperature of 26∘C, the concentrations of chloride ions are: intracellular: 70 extracellular: 485 What is the equilibrium potential? Give a numeric answer within 1%, in mV.
February 19, 2013 by B

College Chemistry
2NO(g)+O2(g)<->2NO2(g) has KP = 2.77 1011 at 25 C. Suppose a mixture of the reactants is prepared at 25 C by transferring 0.943 g of NO and 589 mL of O2 measured at 30.7 C and 829 torr into a 1 L vessel. When the mixture comes to equilibrium, what will be the ...
March 12, 2013 by Peter

CHEMISTRY
Method for getting correct answer? Thank you! Initially there were equilibrium concentrations of 0.1887 M A, 0.1042 M B. Which of the equations below is correct if the pressure decreased by a factor of 2.40? Use the reaction below. 6A(g) ↔ 5 B(g) Qc = 0.42 Kc Qc = 0.45 ...
April 6, 2014 by Chemistry

CHEMISTRY
Method for getting correct answer? Thank you! Initially there were equilibrium concentrations of 0.1887 M A, 0.1042 M B. Which of the equations below is correct if the pressure decreased by a factor of 2.40? Use the reaction below. 6A(g) ↔ 5 B(g) a. Qc = 0.42 Kc b. Qc = ...
April 6, 2014 by Chemistry

Bioelectricity
Na equil-v: Only sodium may cross a membrane separating two compartments. At a temperature of 28∘C, the concentrations of sodium ions are: intracellular: 100 extracellular: 485 What is the equilibrium potential? Give a numeric answer within 1%, in mV.
February 19, 2013 by B

Bioelectricity
K equil-v: Only potassium may cross a membrane separating two compartments. At a temperature of 30∘C, the concentrations of potassium ions are: intracellular: 280 extracellular: 110 What is the equilibrium potential? Give a numeric answer within 1%, in mV.
February 19, 2013 by B

chemistry
Assume that gaseous hydrogen iodide is synthesized from hydrogen gas and iodide vapor at 50 degrees celcius where the equilibrium constant is 1.00 x 10^2. Suppose HI at 5.00 10^-1 M, H2 at 1.00 x 10^-2 M, and I2 at 5.00 x 10^-3 M are mixed in a 5.0 L container. Calculate all ...
August 15, 2010 by Anonymous

CHEMISTRY
Hydrogen gas and iodine gas react via the equation, H2 + I2 <--> 2HI, and K=76 at 600K. If 0.05 mole of HI is placed in a flask at 600K, what are the equilibrium concentrations of HI, I2, H2? I am very lost at where to even start with this problem
March 18, 2012 by Kristen

Chemistry
At the start of the reaction there are 0.714 mole of H2, 0.984 mole of I2, and 0.886 mole of HI in a 2.70 L reaction chamber. Calculate the concentrations of the gases at equilibrium.
February 23, 2013 by Amy

chem help!!
The following equilibrium concentrations were observed for the Haber process at 127 oC: [NH3] = 3.1 x 10-2 mol L-1 [N2] = 8.5 x 10-1 mol [H2] = 3.1 x 10-3 mol Calculate the value of K at 127 oC for this reaction
May 31, 2011 by xx

chemistry
For the diprotic weak acid H2A Ka1=2.1x10^-5 and Ka2=5.5x10^-7. What is the pH of a 0.0800M solution of H2A? What are the equilibrium concentrations of H2A and A^2- in this solution?
October 12, 2012 by ice cream

science
passive transport involves movement of substances...... A) from areas of lower concentration areas of higher concentrations. B)from areas of higher concentrations to areas of lower concentration C) from areas which the concentration has reached a balance D) from areas of ...
January 26, 2015 by KK

chemistry
Calculate the equilibrium concentrations of all three substances. Kc=1.7e-3 Q=3.6e-3 [NO]=0.0015 mol/L [O2]=0.025 mol/L [N2]=0.025 mol/L I cannot figure out the concentration for NO...please help! thank you!
September 10, 2014 by Lauren

Chemistry
For the diprotic weak acid H2A, Ka1 = 2.2 10-5 M and Ka2 = 7.8 10-7 M. What is the pH of a 0.0650 M solution of H2A? What are the equilibrium concentrations of H2A and A2 in this solution? Thank you for the help!!
October 20, 2013 by Homework help

Chemistry
For the diprotic weak acid H2A, Ka1 = 2.2 10-5 M and Ka2 = 7.8 10-7 M. What is the pH of a 0.0650 M solution of H2A? What are the equilibrium concentrations of H2A and A2 in this solution?
October 20, 2013 by D.C.

Chemistry
For the diprotic weak acid H2A, Ka1 = 2.2 10-5 M and Ka2 = 7.8 10-7 M. What is the pH of a 0.0650 M solution of H2A? What are the equilibrium concentrations of H2A and A2 in this solution?
October 20, 2013 by D.C.

Chemistry
For the diprotic weak acid H2A, Ka1 = 2.2 10-5 M and Ka2 = 7.8 10-7 M. What is the pH of a 0.0650 M solution of H2A? What are the equilibrium concentrations of H2A and A2 in this solution?
October 20, 2013 by D.C.

Chemistry
For the diprotic weak acid H2A, Ka1 = 2.2 10-5 M and Ka2 = 7.8 10-7 M. What is the pH of a 0.0650 M solution of H2A? What are the equilibrium concentrations of H2A and A2 in this solution? Thank you for the help!!
October 20, 2013 by Homework help

Chemistry
For the diprotic weak acid H2A, Ka1 = 2.2 10-5 M and Ka2 = 7.8 10-7 M. What is the pH of a 0.0650 M solution of H2A? What are the equilibrium concentrations of H2A and A2 in this solution? Thank you for the help!!
October 20, 2013 by D.C.

chemistry
Concerning the following reaction at equilibrium: 3Fe(s) + 4H2O(g) Fe3O4(s) + 4H2(g), increasing the concentration of the Fe(s) would: Answer A. Shift the equilibrium to the right B. Shift the equilibrium to the left C. No change D. Increase the value of the equilibrium ...
July 21, 2012 by ken

chemistry 2
Calculate the relative concentrations of o-ethylbenzoic acid (pKa 3.79) and potassium o-ethylbenzoate that are needed to prepare a pH 4.0 buffer I know to set up hassle equation but when i get .21=log[a-/ha] i get lost because i was not given concentrations .. please help ...
July 28, 2013 by amber

chemistry
Liquid Nitrogen tetroxide, N2O4(l), was used as a fuel in Apollo missions to the moon. In a closed container the gas N2O4(g) decomposes to nitrogen dioxide, NO2(g). The equilibrium constant,k, for this reaction is 0.87 at 55 degrees Celsius. A vessel filled with N2O4(g) at ...
April 3, 2008 by Claus

equilibrium constant (Kp)
What is the equilibrium constant "Kp" at 200 C for the reaction below: P4(s) + 6 Cl2(g) --><-- 4 PCL3(l) Given the following at 200 C P4(s)+ 10 Cl2(g) --><-- 4 PCl5(s) Kc=8.12 PCl3(l)+ Cl2(g) --><-- PCl5(s) Kc=0.771 Answer: 6.7*[10^(-9)] not sure what to do. ...
July 20, 2011 by k

chemistry
What are the concentrations of [H+] and [OH-] in each of the following. Determine the pH and pOH for each solution. A. 1.25 M HCl B. 0.25 M NaOH C. 0.035 M Ca(OH)2 D. 0.50 M HNO3 I know how to do the pH and pOH I just do not know how to figure out the both concentrations.
April 28, 2010 by Anna

Chemistry
PCl5 --> PCl3 + Cl2 A 0.318 mol sample of PCl5(g) is injected into an empty 4.15 L reaction vessel held at 250 C. Calculate the concentrations of PCl5(g) and PCl3(g) at equilibrium.
April 22, 2014 by Jordyn

Chemistry
What are the concentrations of A and HA after 24 mL of 0.33 M hydrochloric acid solution is added to 86 mL of a solution that has [A ]=0.67 M? Do NOT consider any equilibrium reactions in this problem. A(aq) + HCl(aq) → HA(aq) + Cl(aq) How do I calculate this problem...
March 31, 2013 by John

chemistry
Calculate [Fe^2]+ when the cell reaction reaches equilibrium? A voltaic cell is constructed based on the following reaction and initial concentrations: Fe^2+,( 0.0050 M ) + Ag+,( 2.5 M ) ----> Fe^3+,( 0.0050 M ) + Ag(s)
March 28, 2009 by HELP!!!

Chemistry
A solution is made by mixing exactly 500 mL of 0.178 M NaOH with exactly 500 mL of 0.100 M CH3COOH. Calculate the equilibrium concentrations of H+, CH3COOH, CH3COO-, OH-, and Na+.
May 2, 2011 by Martina

AP Chemistry
A solution is made by mixing exactly 500 mL of 0.167 M NaOH with exactly 500 mL of 0.100 M CH3COOH. Calculate the equilibrium concentrations of H+, CH3COOH, CH3COO-, OH-, and Na+.
February 16, 2014 by Allison

Chemistry
A solution is made by mixing 5.00 102 mL of 0.167 M NaOH with 5.00 102 mL of 0.100 M CH3COOH. Calculate the equilibrium concentrations of H+, CH3COOH, CH3COO−, OH−, and Na+.
March 20, 2015 by Sandhya

Chemistry
The value of KC for the interconversion of butane and isobutane is 2.5 at 25C. If you place 0.067 mol of butane in a 0.250-L flask at 25C and allow equilibrium to be established, what will be the concentrations of the two forms of butane? A)[butane] B)[isobutane]
March 1, 2014 by Chris

Chemistry
in the presence of NH3, Cu+2 forms the complex ion [Cu(NH3)4]+2. If the equilibrium concentrations of Cu+2 and [Cu(NH3)4]+2 are 1.8x10^-17M and 1.0x10^-3M respectively, in a 1.5 M NH3 solution, calculate the value for the overall formation constant of [Cu(NH3)4]+2. Cu+2(aq)+ ...
April 3, 2012 by lena

chemistry
For the reaction at equilibrium: 3Fe(s) + 4H2O(g) Fe3O4(s) + 4H2(g), removing some of the product, Fe3O4(s), would: Answer A. Increase the value of the equilibrium constant, K B. No change C. Decrease the value of the equilibrium constant, K D. Shift the equilibrium to the ...
July 21, 2012 by ken

chemistry
An equilibrium constant ... A. is the same, regardless of the initial concentrations of reactants. B. is small when the products are favored in the reaction. C. is calculated by dividing the concentration of the reactants by the concentration of the products. D. is ...
April 10, 2008 by Wayland

CHEMISTRY 1C
An equilibrium constant ... A. is small when the products are favored in the reaction. B. is calculated by dividing the concentration of the reactants by the concentration of the products. C. is the same, regardless of the initial concentrations of reactants. D. is ...
January 19, 2009 by WENDY

chemistry
A voltaic cell is constructed based on the following reaction and initial concentrations: Fe^2+,( 0.0055 M ) + Ag+,( 2.5 M ) ----> Fe^3+,( 0.0055 M ) + Ag(s) <---- its a forward and reverse arrow Calculate [Fe^2]+ when the cell reaction reaches equilibrium can someone ...
March 28, 2009 by lynn

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. The reaction is at ...
February 25, 2015 by danny

chemistry
When 10.0 mL of 0.012 M pb(NO3)2 is mixed with 10.0 mL of 0.030 M KI, a yellow precipitate of PbI2(s) forms. a)Calculate the molarity of [Pb^2+] b)Calculate the initial molarity of [I^-] c)On measuring the equilibrium concentrations of [I^-] it came out to be 8.0 x 10^-3 M. ...
August 15, 2010 by Anonymous

Chemistry
2 NO(g) + O2 (g) <==> 2 NO2 (g) Given that Kp=7.961012 for the reaction above and the following starting conditions: Initial Concentrations p(NO)=0.775 atm p(NO2)=0.000 atm p(O2)=0.789 atm Determine the equilibrium concentration of NO2.
March 7, 2014 by Haley

chemistry - exam practice help!!
i'm not exactly sure how to do this question :/ i dont even know where to start. "Determine the equilibrium [F-] of the following solution with initial concentrations od [HF]= 1.296 M and [NaF] = 1,045 M (ka for HF is 6.6 * 10 ^ -4) options are a) 1.046 b) 0.251 c) 2.344 d) 8....
December 12, 2012 by Anya

Chemistry
With the initial concentrations of [SCN]= 0.0005 M, [Fe3+]= 0.000698M, and [Fe(SCN)2+]=0.000M, determine the value of k if the [Fe(SCN)2+] at equilibrium is 0.0000866M. Fe3+(aq) + SCN (aq) = Fe(SCN)2+ (aq)
June 8, 2011 by Marcelo

chemistry
An equilibrium constant A. is small when the products are favored in the reaction. B. is the same, regardless of the initial concentrations of reactants. C. is calculated by dividing the concentration of the reactants by the concentration of the products. D. is independent of ...
April 9, 2008 by Jason

chemistry,
the question is, if concentrations do not change why is the equilibrium state considered dynamic? First of all I dont understand what makes a state dynamic? The reaction is not stopped, it is going forward, and reverse, at the same rate. Molecules are constantly reacting in ...
February 21, 2007 by amy

Chemistry
At 2000 ∘C the equilibrium constant for the reaction 2NO(g)←−→N2(g)+O2(g) is Kc=2.4103. 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 ...
June 6, 2015 by Braxten

Chemistry
Fluorine reacts with oxygen to yield oxygen difluoride. 2 F2(g) + O2(g)<--> 2 OF2(g) What is the value of K if the following concentrations are found at equilibrium: [O2]= 0.200 mol/L, [F2]=0.0100 mol/L, and [OF2]=0.0633 mol/L
March 1, 2012 by Sally

Chemistry
Fluorine reacts with oxygen to yield oxygen difluoride. 2 F2(g) + O2(g) 2 OF2(g) What is the value of K if the following concentrations are found at equilibrium: [O2] = 0.200 mol/L, [F2] = 0.0100 mol/L, and [OF2] = 0.0633 mol/L
December 9, 2012 by Marie

chem
What are the equilibrium concentrations of H2SO3, H+, HSO3−, and SO32−in a 0.050 M solution of sulfurous acid H2SO3 at 25 oC? For H2SO3 at 25 oC, Ka1 = 1.510−2 and Ka2 = 1.010−7
February 25, 2013 by ston

chem
What are the equilibrium concentrations of H2SO3, H+, HSO3−, and SO32−in a 0.050 M solution of sulfurous acid H2SO3 at 25 oC? For H2SO3 at 25 oC, Ka1 = 1.510−2 and Ka2 = 1.010−7
February 25, 2013 by ston

chm152
Consider the following equilibrium: 5.0 moles of are placed in a 10.0 L flask at 200 C and allowed to come to equilibrium. Analysis shows that 1.0 mole of is present in the equilibrium mixture. How many moles of Cl2 are present at equilibrium. Choose one answer. a. 0 b. 1.0 c...
March 27, 2010 by ami

Chemistry
Phosphorus pentachloride decomposes according to the chemical equation PCl5(g) ⇌ PCl3(g) + Cl2(g) A 0.304 mol sample of PCl5(g) is injected into an empty 4.75 L reaction vessel held at 250 C. Calculate the concentrations of PCl5(g) and PCl3(g) at equilibrium.
April 2, 2013 by Dee

Chemistry
An equilibrium constant ... A. is independent of temperature. B. is small when the products are favored in the reaction. C. is calculated by dividing the concentration of the reactants by the concentration of the products. D. is the same, regardless of the initial ...
April 9, 2009 by Lisa

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