In the presence of zinc and potassium hydroxide, nitrobenzene (C6H5NO2) reacts with triethylene glycol (C6H1404) to produce azobenzene (C12H10N2), along with two other products. If you react 0.10 L of nitrobenzene with 0.30 L of triethylene glycol and recover 55 g of azobenzene, what is the whats the precent yield for this reaction? Hint: you need to be dense about this question!2 C6H5NO2(1) + 4 C6H1404(1) C12H10N2(1) + 4 C6H12O4(1) + 4 H2O(1)
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- Quinine ( C20 H24 N2 O2) is the most important alkaloid derived from cinchona bark. It is used as an antimalarial drug. For quinine, pK, = 5.1 and pK, = 9.7 ( pKp = – log Kp). Only 1 g quinine will dissolve in 1920.0 mL of solution. Calculate the pH of a saturated aqueous solution of quinine. Consider only the reaction | Q+ H2O= QH+ + OH- described by pK, where Q = quinine. pH =Only 15-14Assume that the reaction Arabinose +Pi <> Arabinose-6-P has a delta G of +13.0 kJ/mol and the reaction XTP <> XDP + Pi has a delta G of -25.7 kJ/mol. Calculate the delta G for the combined reaction Arabinose + XTP <> Arabinose-6-P + ADP, in kJ/mol to four significant figures.
- Draw dipeptide Arg-Thr at pH 6.0. Circle the six atoms that are restricted in one plane. Calculate its approximate pI assuming pKa for NH3+ is 10.0, pKa for COOH is 3.0, PKR for Arg is 12.0The main constituents in vinegar are water and ethanoic acid (CH3COOH). In order to determine the concentration of acid in homemade vinegar, a student titrated 25 cm3 of 001 M NaOH against the vinegar. The equation for the reaction is: CH3COOH(aq) + NaOH(aq) ® CH3COONa(aq) + H2O(l) The following titration results were obtained: Burette readings (cm3) Rough 1 2 Final burette reading 20.10 38.90 31.40 Initial burette reading 0.10 20.00 12.50 Volume of vinegar used 20.00 18.90 18.90 (a) What volume of vinegar should be used in the calculation? (b) What is the mole ratio of NaOH:CH3COOH? (c) Calculate the number of moles of alkali in 25 cm3 of NaOH solution used. (d) How many moles of acid were used in the titration? (e) Calculate the…The standard state free energy of hydrolysis of acetyl phosphate isΔG° = -42.3 kJ/mol. Acetyl-P + H2O acetate + Pi Calculate the free energy change for the acetyl phosphate hydrolysis in a solution of 2 mM acetate, 2 mM phosphate and 3 nM acetyl phosphate.
- A 100 mL solution of 0.1 M glycine at pH 1.72 was titrated with 2 M LIOH. The pH was monitored and the result were plotted as shown in the graph. The key points of the titration are designated as I to V. Identify the key point in the titration corresponding to the pH at which the carboxyl group is half deprotonated. 12 JL30 (V) 9.60 (IV) 8 5.97 pH 6 2.34 CII) 2 (I) 0.5 1.0 1.5 2.0 OH (equivalents) IV O Il and IV NextStearidonic acid (C18H28O2) is an unsaturated fatty acid obtained from oils isolated from hemp and blackcurrant (see also Problem 10.11). a. What fatty acid is formed when stearidonic acid is hydrogenated with excess Hạ and a Pd catalyst? b. What fatty acids are formed when stearidonic acid is hydrogenated with one equivalent of Hz and a Pd catalyst? c. Draw the structure of a possible product formed when stearidonic acid is hydrogenated with one equivalent of H2 and a Pd catalyst, and one double OH stearidonic acid bond is isomerized to a trans isomer. d. How do the melting points of the following fatty acids compare: stearidonic acid; one of the products formed in part (b); the product drawn in part (c)?A monoprotic weak acid, HA, dissociates in water according to the reaction HA(aq) = H+ (aq) + A¯(aq) The equilibrium concentrations of the reactants and products are [HA] = 0.220 M, [H+] = 3.00 × 10−4 M, and [A¯] = 3.00 × 10−4 M. Calculate the value of pKa for the acid HA. pKa =
- Benzene, C6H6, is an aromatic hydrocarbon that exists as a liquid at 298 K and 1 bar. The solubility of benzene in water, defined as the concentration of the saturated solution, is 2.23×10¬3 M at 298 K and 1 bar, and its standard Gibbs free energy of formation is AfG° (C6H6, ) = 124.3 kJ/mol. a. Calculate the standard Gibbs free energy change for the process of dissolution of benzene in water a. Find the chemical potential of the benzene solute standard state AFG° (C6H6, aq).Given the equation below, determine which statement is incorrect. 4C(s) + 6H2(g) + O2(g) → 2C2H5OH(1) AH°=555.4 kJ A) If the equation above is multiplied by two, AH° = - 1110.8 kJ B) For every 0.5 mol of O2, AH° = -277.7 kJ If the state of ethanol changes from the liquid state to the gas state, the value for AH° no loner applies. D) The value of 571.1 kJ applies to one mole of liquid ethanol. E) If the equation above is reversed, AH° = + 555.4 kJA monoprotic weak acid, HA, dissociates in water according to the reaction HA(aq) = H*(aq) + A¯(aq) The equilibrium concentrations of the reactants and products are [HA] = 0.290 M, H+| = 3.00 × 10¬4 M, and [A-] = 3.00 x 10-4 M. Calculate the value of pKa for the acid HA. pKa