Question

Calculate ΔG for the reaction H2O (l) <=>H+ (aq) + OH- (aq) at 25C for the...

Calculate ΔG for the reaction H2O (l) <=>H+ (aq) + OH- (aq) at 25C for the following conditions in (kJ/mol)?

(a) [H+] = 1.0 x10-3 M, [OH-] = 1.0 x 10-4 M

(b) [H+] = 3.3 M, [OH-] = 4.8 x 10-4 M

Homework Answers

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
The rate law for the reaction H+(aq) + OH−(aq) ---> H2O(l) is Rate = k[H+ ][OH−...
The rate law for the reaction H+(aq) + OH−(aq) ---> H2O(l) is Rate = k[H+ ][OH− ], with
 k = 1.3 x 10^11 mol-1 L s-1 at 25 deg C. In an experiment, 0.500 L of 0.020 mol L-1 KOH(aq) is rapidly mixed with an equal volume of 0.020 mol L-1 HBr(aq). Calculate the time, in seconds, required for [H+ ] to decrease to 1.0x 10^-7 mol L-1.

B(OH)3(aq) + H2O(l) ⇆ B(OH)4-(aq) + H+(aq) Select the correct description of this reaction using Lewis...
B(OH)3(aq) + H2O(l) ⇆ B(OH)4-(aq) + H+(aq) Select the correct description of this reaction using Lewis acid-base theory. * In the forward reaction, B(OH)3 is the ? and H2O is the ? . * In the reverse reaction, B(OH)4- is the ? and H+ is the ? . answer choices for each lewis acid or lewis base
Determine the equilibrium constant for the following reaction         X(OH)2(s) + 2 H+(aq) = X2+(aq) +...
Determine the equilibrium constant for the following reaction         X(OH)2(s) + 2 H+(aq) = X2+(aq) + 2 H2O(l) given the chemical reactions below. X(OH)2(s) = X2+(aq) + 2 OH–(aq) K = 3 x 10–10 H2O(l) = H+(aq) + OH–(aq) K = 1.0 x 10–14
Urea (NH2CONH2), an important nitrogen fertilizer, is produced industrially by the reaction 2NH3(g)+CO2(g)→NH2CONH2(aq)+H2O(l) Given that ΔG∘...
Urea (NH2CONH2), an important nitrogen fertilizer, is produced industrially by the reaction 2NH3(g)+CO2(g)→NH2CONH2(aq)+H2O(l) Given that ΔG∘ = -13.6 kJ, calculate ΔG at 25 ∘C for the following sets of conditions. 1. 40 atm NH3, 40 atm CO2, 4.0 M NH2CONH2 2. 0.10 atm NH3, 0.10 atm CO2, 1.0 M NH2CONH2
The equilibrium constant, Ka, for the reaction below is 6.0*10^-3. Fe(H2O)6 ^3+ (aq) + H2O(l) <-->...
The equilibrium constant, Ka, for the reaction below is 6.0*10^-3. Fe(H2O)6 ^3+ (aq) + H2O(l) <--> Fe(H2O)5 (OH)^2+(aq) + H3O^+ (aq) a)Calculate the pH of the 0.10M solution of Fe(H2O)6^3+. b)Will a 1.0 M solution of iron (II) nitrate have a higher or lower pH than a 1.0 M solution of iron (III) nitrate?
The reaction 2 ClO2(aq) + 2 OH-(aq) ClO3-(aq) + ClO3-(aq) + H2O(l) was studied at a...
The reaction 2 ClO2(aq) + 2 OH-(aq) ClO3-(aq) + ClO3-(aq) + H2O(l) was studied at a certain temperature with the following results: Experiment [ClO2(aq)] (M) [OH-(aq)] (M) Rate (M/s) 1 0.0494 0.0494 0.0450 2 0.0494 0.0988 0.0899 3 0.0988 0.0494 0.180 4 0.0988 0.0988 0.360 (a) What is the rate law for this reaction? Rate = k [ClO2(aq)] [OH-(aq)] Rate = k [ClO2(aq)]2 [OH-(aq)] Rate = k [ClO2(aq)] [OH-(aq)]2 Rate = k [ClO2(aq)]2 [OH-(aq)]2 Rate = k [ClO2(aq)] [OH-(aq)]3 Rate...
You have found the following: NH3(aq) + H2O(l) <=> OH-(aq) + NH4+(aq) K = (1.8991x10^-5) OH-(aq)...
You have found the following: NH3(aq) + H2O(l) <=> OH-(aq) + NH4+(aq) K = (1.8991x10^-5) OH-(aq) + H+(aq) <=> H2O(l) K = (1.067x10^14) What is the value of K for the following reaction? NH3(aq) + H+(aq) <=> NH4+(aq)
Enzymes A(aq) ----->B(aq) <----- The ΔG°\' of the reaction is -7.510 kJ ·mol–1. Calculate the equilibrium...
Enzymes A(aq) ----->B(aq) <----- The ΔG°\' of the reaction is -7.510 kJ ·mol–1. Calculate the equilibrium constant for the reaction. (Assume a temperature of 25° C.) What is ΔG at body temperature (37.0° C) if the concentration of A is 1.8 M and the concentration of B is 0.75 M?
The standard Gibbs energy change for the reaction NH3(aq)+H2O(l)?NH+4(aq)+OH?(aq) is 29.05 kJmol?1 at 298 K. Use...
The standard Gibbs energy change for the reaction NH3(aq)+H2O(l)?NH+4(aq)+OH?(aq) is 29.05 kJmol?1 at 298 K. Use this thermodynamic quantity to decide in which direction the reaction is spontaneous when the concentrations of NH3(aq), NH+4(aq), and OH?(aq) are 0.10 M, 1.0
Urea (NH2CONH2), an important nitrogen fertilizer, is produced industrially by the following reaction: 2NH3(g)+CO2(g)?NH2CONH2(aq)+H2O(l) Given that...
Urea (NH2CONH2), an important nitrogen fertilizer, is produced industrially by the following reaction: 2NH3(g)+CO2(g)?NH2CONH2(aq)+H2O(l) Given that ?G? = ?13.6 kJ/mol, calculate ?G at 25?C for the following sets of conditions A. 40 atm NH3, 40 atm CO2, 5.0 M NH2CONH2 B. 8.0×10?2 atm  NH3, 8.0×10?2 atm  CO2, 1.0 M  NH2CONH2
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT