Tuesday
October 21, 2014

Search: h2 concentrations at equilibrium

Number of results: 4,584

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
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

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
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

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 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
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
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

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

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
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
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
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
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
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
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
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

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

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
you made up a standard solution of calcium sulfate (CaSO4). the temperature is 25C. you then add 5.00*10^-3 odium sulfate (Na2SO4). Calculate the concentrations of calcium and sulfate after equilibrium is reached? The pKs of CaSO4 is 4.58.
January 15, 2011 by Maria

"le Chat. principle".
Hey, can you check this, this is regarding "le Chat. principle". Thanks! #1) The value of the equilibrium constant for the reaction H2CO3(aq) + energy >>> H2O(l) + CO2(g) can be changed by introducing a change to which component of the equation? My answer: It would ...
July 19, 2006 by Dave

physiology (nernst equation)
If cell depolarises at +50mV, what are the concentrations of K+? I am really confused how to use the nernst equation to get the concentrations. If I set up 58 [Kout]/[Kin] = 50, will that be right? I am not sure how to start this problem.
March 6, 2007 by Anna

Chemistry
a) An equilibrium exists between three chemical species in the blood , Hemoglobin, oxygenated hemoglobin and oxygen. Using the symbols Hb for hemoglobin , O2 for oxygen and HbO2 for oxygenated hemoglobin write out the equilibrium reaction. If you have determined if the forward...
November 26, 2011 by AB

Chemistry (conceptual question)
If you have a soln of HNO2 at equilibrium HNO2 (aq) + H20 (l) <-->H3O+ (aq) + NO2- (aq) and water is added, is there a shift in the equilibrium? Can someone explain why to me? I have a hard time understanding the concept of equilibrium and what is part of the equilibrium...
February 19, 2010 by Tommy

CHEMISTRY
The extracellular concentrations of Na+ and K+ are 135mM and 6mM, respectively. The intracellular concentrations of Na+ and K+ are 10mM and 105mM, respectively. The membrane potential is 75mV. For Na+/K+ ATPase, 3Na+ are exported and 2K+ are imported. Calculate the total free ...
September 26, 2013 by Izabella

Chemistry
The extracellular concentrations of Na+ and K+ are 135mM and 6mM, respectively. The intracellular concentrations of Na+ and K+ are 10mM and 105mM, respectively. The membrane potential is 75mV. For Na+/K+ ATPase, 3Na+ are exported and 2K+ are imported. Calculate the total free ...
September 29, 2013 by Kam

Chemistry
The extracellular concentrations of Na+ and K+ are 135mM and 6mM, respectively. The intracellular concentrations of Na+ and K+ are 10mM and 105mM, respectively. The membrane potential is 75mV. For Na+/K+ ATPase, 3Na+ are exported and 2K+ are imported. Calculate the total free ...
September 29, 2013 by Drew

Chemistry check my answer?
Hi! is my answer correct? Consider the following chemical reaction: H2 (g) + I2 (g) <> 2HI (g) At equilibrium in a particular experiment, the concentrations of H2, I2, and HI were 0.15 M, 0.033 M, and 0.55 M, respectively. The value ofKeq for this reaction is I solved by...
October 25, 2010 by Richard

chemistry
Determine the expression for the equilibrium constant for this equilibrium reaction: 2NO(g) + 2CO(g) (arrows)(in equilibrium with) N2(g) + 2CO2(g) PLease help anyone i really apreciate it Beccy
January 8, 2011 by rebecca niles

chemistry
Into a 1.00 liter flask are placed 0.820 moles of NO and 0.223 moles of N2 and O2. What are the concentrations of NO, N2, and O2 at equilibrium? For the molarity for each, I got this: NO= .027 M N2= .0079 M O2= .0069 M balanced equation: 2NO(g) <-> N2(g) + O2 How do I ...
November 27, 2012 by Victoria

Chemistry
Consider this system at equilibrium. A(aq) <-> B(aq) Delta H = +750 kJ/mol .. What can be said about Q and K immediately after an increase in temperature? a] Q > K because Q increased.. b] Q>K because K decreased.. c] Q<K because Q decreased.. d] Q<K because ...
March 5, 2012 by Tracy

Chem
You made up a saturated solution of calcium sulfate (CaSO4). The temp is 25 degrees Celsius. You then add 5.00*10^-3 of sodium sulfate (NaSO4). What are the concentrations of calcium and sulfate after equilibrium is reached? The pKs of CaSO4 is 4.58. I know the Ks of CaSO4 to ...
June 5, 2011 by Mig

Chemistry
Phosphorus pentachloride decomposes according to the chemical equation PCl5(g) -----> PCl3 (g)+ Cl2(g) Kc= 1.80 at 250 degrees C A 0.206 mol sample of PCl5(g) is injected into an empty 3.30 L reaction vessel held at 250 C. Calculate the concentrations of PCl5(g) and PCl3(g...
September 30, 2013 by Katherine

Chemistry
Given: Al^3+ forms a complex ALSO4+ in the presence of sulfate... Al^3+ + SO4^2- = AlSO4+ with Kstab = 10^3.01 Question: How many ppm Al(total) would be in equilibrium with gibbsite at pH 4 and 25 degrees celsius in the presence of 10^3- m SO4^2- (consider only this one ...
February 16, 2007 by Mary

Chemistry
If a solution of formic acid contains 0.2 M HCHO2, 0.006 M CHO2-, and 0.006 M H+, What is the Ka of the acid? What is the ph of the solution at the concentrations given? What would happen to the equilibrium position if more CHO2- were added to the solution?
July 7, 2014 by Anonymous

College Chemistry
What are the concentrations of Pb2+ and Cu2+ when the cell potential falls to 0.370 V? Given: A voltaic cell consists of a Pb/Pb2+ half-cell and a Cu/Cu2+ half-cell at 25degrees C . The initial concentrations of Pb2+ and Cu2+ are 5.3010−2 M and 1.60 M, respectively. The...
June 23, 2012 by Maria

Science
4. Chlorine and bromine react by the equation​​Cl2(g) + Br2(g) D 2BrCl(g) Kc = 1.2 x 102 at 150oC. What are the equilibrium concentrations of each reactant and product if a 2.0 L container initially contained 0.026 mole each of Cl2 and Br2 at 150oC? Show all ...
October 3, 2013 by Abay

science
I posted this before but i realized i posted somethings that were wrong. mosquito larvae can tolerate extremely low dissolved oxygen concentrations, yet cannot survive at temperatures above 25 degrees celcius. how might you account for dissolved oxygen concentrations of such a...
September 13, 2009 by cara

Dr. BOB chemistry help please!
hi At a particular temperature, K = 1.00 102 for the following reaction. H2(g) + I2(g)= 2 HI(g) In an experiment, 1.73 mol H2, 1.73 mol I2, and 1.73 mol HI are introduced into a 1.00 L container. Calculate the concentrations of all species when equilibrium is reached. H2 okay ...
January 18, 2009 by Enrique

CHM 152
Consider the following equilibrium: PCl5 = PCl3+ Cl2 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 are present at equilibrium. Choose one answer. ...
March 26, 2010 by AMI

Chemistry
At 473 K, for the elementary reaction 2NOCl <=> 2NO + Cl_2 k(1) =0.078 L/mol*s k(-1)=470 L^2/mol^2*s A sample of NOCl is placed in a container and heated to 473 K. When the system comes to equilibrium, [NOCl] is found to be 0.49 mol/L. Find Cl_2 and NO concentrations
September 8, 2011 by Anonymous

CHM
Given the initial concentrations of 0.10 atm NO2 and 0.10 atm N2O4 in a 1.0 L flask, what will be the equilibrium partial pressure of NO2? N2O4(g)=2NO2 Kp=0.660at319K Choose one answer. a. 0.10 atm b. 0.31 atm c. 0.045 atm d. 0.72 atm e. 0.19 atm
March 28, 2010 by AMI

Chemistry
Al^3+ forms a complex ALSO4+ in the presence of sulfate... Al^3+ + SO4^2- = AlSO4+ with Kstab = 10^3.01 How many ppm Al(total) would be in equilibrium with gibbsite at pH 4 and 25 degrees celsius in the presence of 10^3- m SO4^2- (consider only this one complex and assume ...
February 11, 2007 by Mary

Chemistry
Al^3+ forms a complex ALSO4+ in the presence of sulfate... Al^3+ + SO4^2- = AlSO4+ with Kstab = 10^3.01 How many ppm Al(total) would be in equilibrium with gibbsite at pH 4 and 25 degrees celsius in the presence of 10^3- m SO4^2- (consider only this one complex and assume ...
February 11, 2007 by Mary

chemistry
An equilibrium mixture contains N2O4, (P= 0.30 ) and NO2 (P= 1.1 ) at 350 K. The volume of the container is doubled at constant temperature. Calculate the equilibrium pressure of when the system reaches a new equilibrium. Calculate the equilibrium pressure of NO2 when the ...
May 20, 2010 by Anonymous

Chemistry
At 25C, K = 0.090 for the following reaction:H2O(g) + Cl2O(g) 2 HOCl(g) Calculate the concentrations of all species at equilibrium for each of the following cases. (a) 1.2 g H2O and 1.6 g Cl2O are mixed in a 1.4 L flask. (b) 1.2 mol pure HOCl is placed in a 1.9 L flask
February 15, 2009 by Lindsey

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