Chemistry

Chemistry, 23.07.2019 06:10, mdkester11

The equilibrium constant you studied in this reaction is dependent upon the [h+]. fe3+(aq)+hscn(aq))⇌[fescn]2+(aq)+h+ (aq) keq=[fescn2+][h+][fe3+][hscn] a. what was the effect upon the magnitude of keq caused by using dilute hno3 rather than 1.0 m hno3?

answer

Answers: 3

Show answers

Similar questions

Предмет

Chemistry, 08.08.2019 04:20, jpruitt10

1. a student mixes 5.0 ml 2.00 x 103 m fe(noh with 5.0 ml 2.00 x 10 m kscn. she finds that in the equilibrium mixture the concentration of fescn" is 1.2 x 10*m. find ke for the reaction fe (aq)+scn(aq)fescn(aq) step 1 find the number of moles fe and scn initially present. (use eq. 3.) sample caleulation moles fe moles scn step 2 how many moles of fescn are in the mixture at equilibrium? what is the volume of the equilibrium mixture? (use eq. 3.) ml moles fescn2 sample calculation how many moles of fe and scn reacted to form fescn moles fe reacted moles scn reacted sample calculation step 3 how many moles of fe and scn remain in the solution at equilibrium? (use eq. 4 and th results of steps 1 and 2.) equilibrium moles fe equilibrium moles scn

Answers: 2

Предмет

Chemistry, 20.09.2019 19:30, GabriellaDul

At equilibrium, the concentrations of reactants and products can be predicted using the equilibrium constant, kc, which is a mathematical expression based on the chemical equation. for example, in the reaction aa+bb⇌cc+dd where a, b, c, and d are the stoichiometric coefficients, the equilibrium constant is kc=[c]c[d]d[a]a[b]b where [a], [b], [c], and [d] are the equilibrium concentrations. if the reaction is not at equilibrium, the quantity can still be calculated, but it is called the reaction quotient, qc, instead of the equilibrium constant, kc. qc=[c]tc[d]td[a]ta[b]tb where each concentration is measured at some arbitrary time t. part a a mixture initially contains a, b, and c in the following concentrations: [a] = 0.300 m , [b] = 1.10 m , and [c] = 0.450 m . the following reaction occurs and equilibrium is established: a+2b⇌c at equilibrium, [a] = 0.110 m and [c] = 0.640 m . calculate the value of the equilibrium constant, kc. express your answer numerically.

Answers: 1

Предмет

Chemistry, 21.09.2019 23:30, kyriejr

At equilibrium, the concentrations of reactants and products can be predicted using the equilibrium constant, kc, which is a mathematical expression based on the chemical equation. for example, in the reaction aa+bb⇌cc+dd where a, b, c, and d are the stoichiometric coefficients, the equilibrium constant is kc=[c]c[d]d[a]a[b]b where [a], [b], [c], and [d] are the equilibrium concentrations. if the reaction is not at equilibrium, the quantity can still be calculated, but it is called the reaction quotient, qc, instead of the equilibrium constant, kc. qc=[c]tc[d]td[a]ta[b]tb where each concentration is measured at some arbitrary time t. part a a mixture initially contains a, b, and c in the following concentrations: [a] = 0.350 m , [b] = 0.750 m , and [c] = 0.350 m . the following reaction occurs and equilibrium is established: a+2b⇌c at equilibrium, [a] = 0.150 m and [c] = 0.550 m . calculate the value of the equilibrium constant, kc. express your answer numerically.

Answers: 3

Предмет

Chemistry, 09.10.2019 22:00, kingk7368

At equilibrium, the concentrations of reactants and products can be predicted using the equilibrium constant, kc, which is a mathematical expression based on the chemical equation. for example, in the reaction aa+bb⇌cc+dd where a, b, c, and d are the stoichiometric coefficients, the equilibrium constant is kc=[c]c[d]d[a]a[b]b where [a], [b], [c], and [d] are the equilibrium concentrations. if the reaction is not at equilibrium, the quantity can still be calculated, but it is called the reaction quotient, qc, instead of the equilibrium constant, kc. qc=[c]tc[d]td[a]ta[b]tb where each concentration is measured at some arbitrary time t. part a a mixture initially contains a, b, and c in the following concentrations: [a] = 0.350 m , [b] = 0.800 m , and [c] = 0.500 m . the following reaction occurs and equilibrium is established: a+2b⇌c at equilibrium, [a] = 0.150 m and [c] = 0.700 m . calculate the value of the equilibrium constant, kc. express your answer numerically.

Answers: 3

Do you know the correct answer?

The equilibrium constant you studied in this reaction is dependent upon the [h+]. fe3+(aq)+hscn(aq))...

Questions in other subjects:

Konu

Geography, 11.04.2020 05:15

What three new viruses have come about in the 21st century?...

Konu

Physics, 11.04.2020 05:15

Did you diagram all the faults and folds correctly? Which fault and/or fold did you find most difficult to diagram? Explain why....

Konu

History, 11.04.2020 05:15

I need help with this I can’t figure out which one is the correct one

Konu

English, 11.04.2020 05:15

communication strategies may include the use of picture books and computer assisted devices that help people with expressive difficulties overcome the frustration of being unable t...

Konu

Chemistry, 11.04.2020 05:15

What is the correct IUPAC name for NH4CL?...

Konu

Arts, 11.04.2020 05:15

Your Personal Essay should address why you selected pharmacy as a career and how the Doctor of Pharmacy degree relates to your immediate and long-term professional goals. Describe...

Konu

Chemistry, 11.04.2020 05:15

The Question is attached :(...

Konu

English, 11.04.2020 05:16

How does author Allison Friedman draw readers into her article...

Konu

History, 11.04.2020 05:16

Who disliked democracy and wanted educated aristocrats to lead the United states

Konu

Mathematics, 11.04.2020 05:16

How do I solve this? Thank youu...

Other tasks in the category: Chemistry More task