since deltaG= -RTlnK
and deltaG= deltaH- T*deltaS = -RT lnK
lnK= -deltaH/RT + deltaS/R
where K = ioninc prodict of water and T is inK
when the above equation is written for two different temperatures
lnK1= -deltaH/RT1+ deltaS/ R (1)
lnK2=- deltaH/RT2+ deltaS/R (2)
lnK2- lnK1= deltaH/r*(1/T1-1/T2)
ln(1.45/1)= deltaH/R*(1/298-1/303)
deltaH/R= 6710 and deltaH= 6710*8.314 J/mole. =55787 J/mole= 55.787 Kj/mole
substituting this value in Eq.1
ln(1*10-14)= -6710/298+deltaS/R
deltaS= 80.8 J/mole.K
at body temperature of 37 deg.c= 37+273= 310K
lnK= -6710/310+ 80.8/8.314
K= 6*10-6 mole2/L2
10) The ionic product [HIOH], which is the equilibrium constant for the dissociation of water, is...
calculate equilibrium dissiociation constant of water help! We know that Kw = 1.0 x 10-14 at 25°C. At 37°C, the [H3O+] in pure water is 1.6 x 10"| M. Calculate the equilibrium dissociation constant of water, Kw, at this temperature. A. 2.6 x 10-14 | CNH-TT H+7: 10 x 10-14 DH = -log(11 B. 1.0 x 10-7 C. 1.0 x 10-14 [1-6x10-?][6.16 *10-8] PH= 6.79 D. 1.6 x 10-7 POH=7. 21
1)Consider the following equilibrium at 972 K for the dissociation of molecular iodine into atoms of iodine. I2(g) ----> 2 I(g); Kc = 1.40 ? 10?3 Suppose this reaction is initiated in a 3.4 L container with 0.067 mol I2 at 972 K. Calculate the concentrations of I2 and I at equilibrium. * I got I2= 0.0135M and I= 0.0124 is this right?* 2)Consider the following equilibrium. NH3(aq) + H2O(l) -----> NH4+(aq) + OH ?(aq) What will happen to the...
Write the equilibrium constant for the dissociation of water. Rewrite it in terms of the ionization of water constant Kw. The concentration of hydronium and hydroxide equals what value?
Calculate the equilibrium dissociation constant, pKdn, for a 0.01 M solution of weak acid for which a conductivity measurement shows that it is 1.16% dissociated at equilibrium in water.
(a) HA (aq) is a weak acid with a dissociation constant, Ka, of 1.0 x 10-11. What is the pH of a 0.061 M solution in A- (aq)? The temperature is 25oC. (b) For the reaction A (g) ⇋ B (g) + C (g), the equilibrium constant is 1.80 at 25.0oC and 4.46 at 75.0oC. Making the approximation that ΔH and ΔS do not change with temperature, calculate the value of the equilibrium constant at 50.0oC as well as the...
(a) HA(aq) is a weak acid with a dissociation constant, Ka, of 1.0 x 10-11. What is the pH of a solution 0.066 M in A-(aq)? The temperature is 25oC. (b) For the reaction A(g) ⇋ B(g) + C(g), the equilibrium constant is 1.80 at 25.0oC and 4.36 at 75.0oC. Assuming ΔH and ΔS do not change with the temperature, calculate the value of the equilibrium constant at 50.0oC and the value of ΔSuniverse at 50.0oC.
(a) HA(aq) is a weak acid with a dissociation constant, Ka, of 1.0 x 10-11. What is the pH of a solution 0.065 M in A-(aq)? The temperature is 25oC. (b) For the reaction A(g) ⇋ B(g) + C(g), the equilibrium constant is 1.80 at 25.0oC and 4.00 at 75.0oC. Assuming ΔH and ΔS do not change with the temperature, calculate the value of the equilibrium constant at 50.0oC and the value of ΔSuniverse at 50.0oC
(a) HA(aq) is a weak acid with a dissociation constant, Ka, of 1.0 x 10-11. What is the pH of a solution 0.068 M in A-(aq)? The temperature is 25oC. (b) For the reaction A(g) ⇋ B(g) + C(g), the equilibrium constant is 1.80 at 25.0oC and 4.95 at 75.0oC. Assuming ΔH and ΔS do not change with the temperature, calculate the value of the equilibrium constant at 50.0oC and the value of ΔSuniverse at 50.0oC.
(a) HA(aq) is a weak acid with a dissociation constant, Ka, of 1.0 x 10-11. What is the pH of a solution 0.065 M in A-(aq)? The temperature is 25oC. (b) For the reaction A(g) ⇋ B(g) + C(g), the equilibrium constant is 1.80 at 25.0oC and 4.14 at 75.0oC. Assuming ΔH and ΔS do not change with the temperature, calculate the value of the equilibrium constant at 50.0oC and the value of ΔSuniverse at 50.0oC.
#4 (a) HA(aq) is a weak acid with a dissociation constant, Ka, of 1.0 x 10-11. What is the pH of a solution 0.061 M in A-(aq)? The temperature is 25oC. (b) For the reaction A(g) ⇋ B(g) + C(g), the equilibrium constant is 1.80 at 25.0oC and 4.14 at 75.0oC. Assuming ΔH and ΔS do not change with the temperature, calculate the value of the equilibrium constant at 50.0oC and the value of ΔSuniverse at 50.0oC.