The KbKb for methylamine (CH3NH2)(CH3NH2) at 25 ∘C∘C is 4.4×10−44.4×10−4.
Part B. By using the value of KbKb, calculate ΔG∘ΔG∘ for the equilibrium in part A.
Part D. What is the value of ΔGΔG when [H+][H+] = 6.6×10−9 MM, [CH3NH+3][CH3NH3+] = 2.5×10−3 MM, and [CH3NH2][CH3NH2] = 9.70×10−2 MM?
The value of KaKa for nitrous acid (HNO2)(HNO2) at 25 ∘C∘C is 4.5×10−44.5×10−4. You may want to reference (Pages 833 - 836) Section19.7 while completing this problem.
1. Using the value of KaKa, calculate ΔG∘ΔG∘ for the dissociation of nitrous acid in aqueous solution.
2. What is the value of ΔGΔG when [H+][H+] = 5.6×10−2M5.6×10−2M , [NO−2][NO2−] = 6.2×10−4M6.2×10−4M and [HNO2][HNO2] = 0.21 MM ?
Consider the decomposition of barium carbonate: BaCO3(s)←→BaO(s)+CO2(g)
1. Using data from Appendix C in the textbook, calculate the equilibrium pressure of CO2CO2 at 1250 KK .
The KbKb for methylamine (CH3NH2)(CH3NH2) at 25 ∘C∘C is 4.4×10−44.4×10−4. Part B. By using the value...
The value of Ka for nitrous acid (HNO2) at 25 ∘Cis 4.5×10−4. You may want to reference(Pages 833 - 836) Section19.7 while completing this problem. Part A Write the chemical equation for the equilibrium that corresponds to Ka. Write the chemical equation for the equilibrium that corresponds to . H+(aq)+NO2−(aq)⇌HNO2(aq) HNO2(aq)⇌H+(aq)+NO2−(aq) HNO2(aq)⇌H−(aq)+NO2+(aq) HNO2(aq)+H+(aq)⇌H2NO2+(aq) HNO2(aq)+H−(aq)⇌H2NO2+(aq) Part B Using the value of Ka, calculate ΔG∘ for the dissociation of nitrous acid in aqueous solution. Express your answer using three significant figures. ΔG∘...
A) Calculate the pH of a 0.0116 M aqueous solution of methylamine (CH3NH2, Kb = 4.2×10-4) and the equilibrium concentrations of the weak base and its conjugate acid. pH = ? [CH3NH2]equilibrium = ? M [CH3NH3+ ]equilibrium = ? M B)Calculate the pH of a 0.0115 M aqueous solution of nitrous acid (HNO2, Ka= 4.6×10-4) and the equilibrium concentrations of the weak acid and its conjugate base. pH = ? [HNO2]equilibrium = ? M [NO2- ]equilibrium = ? M C)...
The value of Ka for nitrous acid (HNO2) at 25 ∘C is 4.5×10−4. You may want to reference (Pages 833 - 836) Section19.7 while completing this problem. 1. What is the value of ΔG when [H+] = 5.9×10−2M , [NO−2] = 6.3×10−4M and [HNO2] = 0.19 M ? Express your answer using three significant figure.
The value of Ka for nitrous acid (HNO2) at 25 ∘C is 4.5×10−4. Part D What is the value of AG when [H+] = 5.8 x 10-2M, [NOą] =6.4 x 10-4 M and (HNO2] = 0.21 M ? Express your answer using three significant figure. IVO AED A o 2 ? AG = Submit Previous Answers Request Answer X Incorrect; Try Again; 3 attempts remaining Recall that AG = AGº + RTinQ, where R is the gas constant, T is...
The equilibrium constant for the equation HNO3(aq) + H2O(l) = H, 0+ (aq) + NO2 (aq) is Kg = 5.6 x 10-4 M at 25.0 °C. Calculate the value of AGixn at 25.0 °C for nitrous acid when [NO2] = [H3O+] = [HNO2] = 1.00 M. AGixn = kJ/mol Will the acid spontaneously dissociate under these conditions? O no O yes Calculate the value of AGrxn for nitrous acid when [NO, ] = [H,O+] = 7.13 x 10- M and...