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Carbonic acid (H2CO3) is unstable in water and rapidly decomposes i to CO2(g) and H2O(l). Consequently,...
The enzyme carbonic anhydrase catalyzes the reaction CO2(g)+H2O(l)−→−HCO3−(aq)+H+(aq).CO2(g)+H2O(l)→ HCO3−(aq)+H+(aq). In water, without the enzyme, the reaction proceeds with a rate constant of 0.039s−10.039 s−1 at 25°C.25 °C. In the presence of the enzyme in water, the reaction proceeds with a rate constant of 1.0×106s−11.0×106 s−1 at 25°C.25 °C. Assuming the collision factor is the same for both situations, calculate the difference in activation energies for the uncatalyzed versus enzyme- catalyzed reaction.
1) why is CO2 the conjugate acid of bicarbonate? Please explaing CO2 (g) + H2O(l) ⇄ H2CO3 (aq) 2) Exercise increases metabolism and thus increase the amount of CO2 in the blood. Following a bout of intense exercise, the pH of your blood was found to be 7.1 and the HCO3− concentration in the blood to be 8 mM. Remember the overall reaction for the bicarbonate buffering system in the blood can be written as: H2CO3 (aq) ⇄ HCO3- (aq)...
Use the following chemical reaction a 6.8X1l0^-3 solution of carbonic acid: H2CO3 (aq) +H2O (l) <-> HCO3 (aq) + H3O . Ka1= 4.3x10^-7 . Ka2= 4.7x10^-11 a. if you add NaHCO3 to the solution, would the pH of the solution go up, down, or stay the same? b. Calculate the pH of the solution if you added 3.4 x10^-3 M NaHCO3.
a) The consecutive equilibria: CO2(g) <=>CO2(aq) + H2O(l) <=>H2CO3(aq) <=>H+(aq) + HCO3-(aq), explain why: A. carbonated beverages are less acidic than pure water. B. carbonated beverages contain measurably less water than the same volume of pure water. C. rainwater is slightly acidic b) A 1.0 M solution of a weak monoprotic acid with Ka = 1.0 10-6 would have a pH of: A. 1 B. 2 C. 3 D. 6 c) Ascorbic acid is a diprotic acid with Ka1 =...
10.39 The first-order rate constant for the dehydration of carbonic acid, H2CO3(aq) = CO2(g) + H2O(1) is about 1 x 102 s-. In view of this rather high rate constant, explain why it is necessary to have the enzyme carbonic anhydrase to enhance the rate of dehydration in the lungs.
10. The hydration of CO2 from the atmosphere according to the reaction CO2(g) + H2O(l) HCO3–(aq) + H+(aq) can be catalyzed by the enzyme carbonic anhydrase. Consider how a catalyst works. Will the catalyst affect the rate of both the forward and reverse reactions? Explain your reasoning. 10. The hydration of CO2 from the atmosphere according to the reaction CO2(e) + H20(1) HCO3(aq) + H+(aq) can be catalyzed by the enzyme carbonic anhydrase. Consider how a catalyst works. Will the...
Use the following data to calculate the Ka of carbonic acid at 253 K. H2CO3 (aq) <==> H+ (aq) + HCO3- (aq) A G° (kJ/mol) -623.2 Substance H2CO3 (aq) HCO3- (aq) H+ (aq) -586.8 0.00 Submit your answer in the following format: 1.23e4, use three sig figs
a) The consecutive equilibria: CO2(g) <=>CO2(aq) + H2O(l) <=>H2CO3(aq) <=>H+(aq) + HCO3-(aq), explain why: A. carbonated beverages are less acidic than pure water. B. carbonated beverages contain measurably less water than the same volume of pure water. C. rainwater is slightly acidic b) A 1.0 M solution of a weak monoprotic acid with Ka = 1.0 10-6 would have a pH of: A. 1 B. 2 C. 3 D. 6 c) Ascorbic acid is a diprotic acid with Ka1 =...
a Nitrous acid and sodium hydrogen carbonate, NaHCO3, are mixed in water. Choose a balanced net ionic equation for the acid-base reaction that could, in principle, occur. HNO2() + NaHCO3(s) + H2O(l) Na+ (aq) + HCO3(aq) + NO3- (aq) + H+ (aq) HNO2 (aq) + NaHCO3(aq) = NaNO2 (aq) + H2CO3(aq) HNO2 (aq) + HCO3- (aq) = NO2 (aq) + H2CO3(aq) HNO2 (aq) + NaHCO3(aq) = NaNO2 (aq) + H2O() + CO2(g)
Match the substance to the correct label for the following reaction: H2CO3 (aq) + H2O (l) ⇔ H3O+(aq) + HCO3−(aq) Question 5 options: 1234 H2O 1234 H2CO3 1234 HCO3- 1234 H3O+ 1. Acid 2. Base 3. Conjugate acid 4. Conjugate base