Carbonic anhydrase, an enzyme that converts carbon dioxide and water to carbonic acid as shown below, functions in the blood at an optimum pH of 7.0-7.5. Which of the following will lower the rate of carbonic anhydrase- catalyzed reaction? CO2 + H2O Carbonic anhydrase H₂CO3 O increasing the concentration of carbon dioxide O running the reaction at 4 °C O carrying out the reaction at pH 7.2 O adding more carbonic anhydrase

Carbonic anhydrase, an enzyme that converts carbon dioxide and water to carbonic acid as shown below, functions in the blood at an optimum pH of 7.0-7.5. Which of the following will lower the rate of carbonic anhydrase- catalyzed reaction? CO2 + H2O Carbonic anhydrase H₂CO3 O increasing the concentration of carbon dioxide O running the reaction at 4 °C O carrying out the reaction at pH 7.2 O adding more carbonic anhydrase

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.66PAE

See similar textbooks

Similar questions

What are the products of each of the following acid-base reactions? Indicate the acid and its conjugate base and the base and its conjugate acid. (a) HCIO4 + H2O (b) NH4 ++ H2O (c) HCO3 + OH
What are the equilibrium concentrations of acetic acid, the acetate ion, and H3O+ for a 0.10 M solution of acetic acid (K2 = 1.8 105)? What is the pH of the solution?
Describe any thermochemical (heat of reaction) evidence for the Arrhenius concept.
The binding of oxygen by hemoglobin (Hb), giving oxy-hemoglobin (HbO2), is partially regulated by the concentration of H3O+ and dissolved CO2 in the blood. Although the equilibrium is complicated, it can be summarized as HbO2(aq)+H3O+(aq)+CO2(g)CO2HbH++O2(g)+H2O(l) (a) Write the equilibrium constant expression for this reaction. (b) Explain why the production of lactic acid and CO2 in a muscle during exertion stimulates release of O2 from the oxy-hemoglobin in the blood passing through the muscle.
If you observe the following reaction at equilibrium, is it possible to tell whether the reaction stated with pure NO2 or with pure N2O4? 2NO2(g)N2O4(g)
Complete the changes in concentrations for each of the following reactions: (a) AgI(s)Ag+(aq)+I(aq)x (b) CaCO3(s)Ca2+(aq)+CO32(aq)x (c) Mg3(OH)2(s)Mg2+(aq)+2OH(aq)x (d) Mg3( PO4)2(s)3Mg2+(aq)+2PO43(aq)x (e) Ca5( PO4)3OH(s)OH(s)5Ca2+(aq)+3PO43(aq)+OH(aq)x
In this Chemical Reaction at equilibrium: N H 3 + H B r ⟺ N H 4 + + B r − If you upset the equilibrium by adding NH3, what will happen to the reaction equilibrium.
The dissociation of acetic acid, CH3COOH, has an equilibrium constant at 25 degrees celsius of 1.8 x 10-5. CH3COOH(aq) ⇋ CH3COO-(aq) + H+(aq) If the equilibrium concentration of CH3COOH is 0.46 moles in 0.500 L of water and that of CH3COO is 8.1 x 10-3 moles in the same 0.500 L, calculate the concentration of H + for the reaction.
Given a solution of acetic acid, with equilibrium net ionic equation (so only showing the ions in the reaction and not the spectator ions): CH3COOH (aq) + H20 () CH3COO (aq) + H3O* (aq) Have 4 beakers with acetic acid. Each beaker gets one of the following four things added to it. Match each thing with how the equilibrium responds when the thing is added. Prompts Submitted Answers sodium acetate Choose a match calcium acetate nothing sodium chloride shifts left to make more reactants acetic acid shifts right then left then right then left... shifts right to make more products
Le Châtelier’s principle is related ultimately to the rates ofthe forward and reverse steps in a reaction. Explain (a) why anincrease in reactant concentration shifts the equilibrium positionto the right but does not change K; (b) why a decrease in Vshiftsthe equilibrium position toward fewer moles of gas but does notchange K; (c) why a rise in Tshifts the equilibrium position of anexothermic reaction toward reactants and also changes K;and(d) why a rise in temperature of an endothermic reaction from T1to T₂ results in K₂ being larger than K1
Oxacarbazepine ( C15H12N2O) is used to treat epilepsy. What would happen to the equilibrium of oxacarbazepine in water when more oxacarbazepine is added to the system? a.) Ratef < Rateb and the equilibrium would shift to reactants (to the left) b.) Ratef > Rateb and the equilibrium would shift to reactants (to the left) c.) Ratef < Rateb and the equilibrium would shift to products (to the right) d.) Ratef > Rateb and the equilibrium would shift to products (to the right)
Find the equilibrium constant (Keq) for the following acid-base reaction and thendetermine the correct equilibrium arrow