How many electrons are transferred in the following reaction? 2clo_4^- + 16H^+ +

Question

How many electrons are transferred in the following reaction? 2clo_4^- + 16H^+ + 14l- right arrow pi_2 + Cl_2 + 8h_2O? 2 20 30 14 5 Determine deltaGdegree for the following reaction: CH_4(g) + 2O_2(g) right arrow CO_2(g) + 2H_2O(1) Substance deltaG degree CH_4(g) -50.7 O_2(g) 0 CO_2(g) -394.4 H_2O(1) -237.4 -207.7 kj -817.9 kj -106.3 kj -130.4 kj At 699 K, delta Gdegree = -23.25 kj for the reaction H_2(g) + l_2(g) = 2HI(g). Calculate delta for this reaction if the reagents are both supplied at 10.0 atm pressure and the product is at 1.00 atm pressure. 50.0 kj -36.6 kj -3.5 kj -50.0 kj The acid dissociation constant for a weak acid HX at 25 degree C is 1.80 * 10^-5. Calculate the free energy of formation for X^-(aq)at 25 degreeC. The standard free energies of HX(aq) and H^*(aq)at 25 degree C are -211.5 kj?mol and O, respectively. -184.4 kj/mol -12.5 kj/mol 223 kj/mol 255 kj/mol THe following reaction occures in basic solution: F_2 + OH^-+ O_2 + F_- + H_2O When the equation is balanced is balanced, the sum of the coefficients is: 11 13 12 10

Explanation / Answer

11)

consider the iodine half reaction

14I- ---> 7I2

balance it with charges

14I- --> 7I2 + 14e-

so

14 electrons are transferred

answer is D) 14

12) given

CH4 + 202 ---> C02 + 2H20

we know that

dGo rxn = dGof products - dGof reactants

so

dGo rxn = dGof C02 + ( 2 x dGof H20) - dGof CH4 - ( 2 x dGfo 02)

using given values

dGo rxn = -394.4 + ( 2 x -237.4) - (-50.7) - ( 2 x0)

dGo rxn = -818.5 kJ

so

answer is B) -817.9 kJ

13) H2 + I2 --> 2 HI

the reaction quotient is given by

Q = (pHI)^2 / (pH2) (pI2)

so

Q = 1 / 10 x 10

Q = 10-2

now

dG = dGo + RT ln Q

so

dG = ( -23.25 x 1000) + ( 8.314 x 699 x ln 10-2)

dG = -50 kJ

so

the answer is D) -50 kJ

14)

we know that

dGO = -RT ln K

dGo = -8.314 x 298 x ln 1.8 x 10-5

dGo = 27068 J/mol

dGo = 27.068 kJ / mol

now

HX --> H+ + X-

dGo rxn = dGof H+ + dGof X- - dGof HX

using given values

27.068 = 0 + dGof X- - (-211.5 )

dGof X- = -184.4 kJ/mol

so

the answer is A) -184.4 kJ/mol

15)

F2 + 2e- ---> 2F-

4OH- ---> 02 + 2H20 + 4e-

the balanced reaction is

4OH- + 2F2 ---> 02 + 2H20 + 4F-

the sum of coefficeints = 4 + 2 + 1 + 2 + 4 = 13

so

the answer is B) 13

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