Number 2 a to d if its okay but if its not okay then, a and b only then Ill ask the other two in separate LEARNING ACTIVITY 21. Consider the following hypothetical aqueous reaction:A(aq) – B(aq)A flask is charged with 0.200 mol of A in a total volume of 100.0 mL. The following data are collected:Time (min)Moles of A200.140400.100600.070800.0500.200a. Calculate the number of moles of B at each time in the table, assuming that there are no moleculesof B at time zero and that A cleanly converts to B with no intermediates.b. Calculate the average rate of disappearance of A for each 20-min interval in units of M/s.c. Calculate the average rate of disappearance of A from the start of reaction to t = 80 min in units ofM/s.d. Between t = 0 min and t = 60 min, what is the average rate of appearance of B in units of M/s?Assume that the volume of the solution is constant.2. For each of the following gas-phase reactions, write the rate expression in terms of the appearance ofeach product and disappearance of each reactant:a. Os(g) + H2O(g) → 2 O2(g) + Hz(g)b. 4 NH3(g) + 5 Oz(g) → 4 NO(g) + 6 H;O(g)c. 2 C2H2(g) + 5 O2(g) → 4 CO2(g) + 2 H2O(g)d. CaH;NH2(g) –→ CaHe(g) + NH3(g)3. Consider the reaction Os(g) + H2O(g) → 2 Oz(g) + H2(g). If the concentration of Os is decreasing at therate of 0.025 M/s, what are the rates of change in the concentrations of Oz and H2?

The rate of reaction is the transformation of a reactant or a product per unit of time. Due to this,…

2. For each of the following gas-phase reactions, write the rate expression in terms of the appearance of each product and disappearance of each reactant: a. Os(g) + H:O(g) → 2 O:(g) + H2(g) b. 4 NH3(g) + 5 Oz(g) → 4 NO(g) + 6 H;O(g) c. 2 C2H2(g) + 5 0:(g) → 4 CO2(g) + 2 H:O(g) d. CaH;NH2(g) –→ CaHe(g) + NH>(g)

2. For each of the following gas-phase reactions, write the rate expression in terms of the appearance of each product and disappearance of each reactant: a. Os(g) + H:O(g) → 2 O:(g) + H2(g) b. 4 NH3(g) + 5 Oz(g) → 4 NO(g) + 6 H;O(g) c. 2 C2H2(g) + 5 0:(g) → 4 CO2(g) + 2 H:O(g) d. CaH;NH2(g) –→ CaHe(g) + NH>(g)

Biochemistry

9th Edition

ISBN:9781305961135

Author:Mary K. Campbell, Shawn O. Farrell, Owen M. McDougal

Publisher:Mary K. Campbell, Shawn O. Farrell, Owen M. McDougal

Chapter2: Water: The Solvent For Biochemical Reactions

Section: Chapter Questions

Problem 40RE: MATHEMATICAL A catalog in the lab has a recipe for preparing 1 L of a TRIS buffer at 0.0500 M and...

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MATHEMATICAL A catalog in the lab has a recipe for preparing 1 L of a TRIS buffer at 0.0500 M and with pH 8.0: dissolve 2.02 g of TRIS (free base, MW=121.1 g/mol) and 5.25 g of TRIS hydrochloride (the acidic form, MW=157.6 g/mol) in a total volume of 1 L. Verify that this recipe is correct.
pH of solution 14.00 12.00 10.00 8.00 6.00 First 4.00 equivalence point 2.00 0 First midpoint Second equivalence point Third midpoint pH = pKa=12.32 Third equivalence point HPO4(aq) + OH(aq) PO4(aq) + H2O(1) Second midpoint pH = pKa = 7.21 H2PO4 (aq) + OH(aq) HPO42 (aq) + H2O(1) Using the Henderson- Hasselback equation, show how to create 2L of a 0.1 M KPhos pH 7.5 buffer using K2HPO4 and KH2PO4. The chart to the left should help you understand what pKa to start with. Show your work. pH = pKa = 2.16 H3PO4(aq) + OH(aq) H2PO4(aq) + H2O(l) 25.0 50.0 75.0 100.0 Volume of NaOH added (mL)
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