Thermodynamic parameters (here the activation energy, enthalpy and entropy) for the release of a certain drug from a tablet formulation were measured and found to be: AH = -23.6 kJ mol¹ and AS = 59.9 J K¹ mol¹¹. Which ONE of the following is the value of AG for the release of the drug at 37.0 °C? -42.2 kJ/mol -5.0 kJ/mol -18.6 kJ/mol -25.8 kJ/mol -2.2 kJ/mol

Thermodynamic parameters (here the activation energy, enthalpy and entropy) for the release of a certain drug from a tablet formulation were measured and found to be: AH = -23.6 kJ mol¹ and AS = 59.9 J K¹ mol¹¹. Which ONE of the following is the value of AG for the release of the drug at 37.0 °C? -42.2 kJ/mol -5.0 kJ/mol -18.6 kJ/mol -25.8 kJ/mol -2.2 kJ/mol

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

A closed vessel of volume 2.1 L contains a mixture of neon and fluorine gas. The total pressure of the mixture in the vessel is 3.8 atm at 0.0 °C. When the mixture is heated to 15.0 °C, the entropy of the mixture increases by 0.338 J · K-'. Calculate the number of moles of neon and fluorine in the mixture. mol NNe mol NF2 II
Dissolution of ionic compounds generally involves an increase in entropy (+ΔS°), but for a few specific metal ions, dissolution of the ionic compound can lead to a decrease in entropy. For example, the dissolution of magnesium chloride (MgCl2) has a ΔS° = -115 J K-1 mol-1. Explain this decrease in entropy.
Consider the gas-phase equilibrium, CH3OH(g) CO(g) + 2H2(g). For this reaction, standard free-energy and standard enthalpy changes for this reaction are -60 kJ/mol at 200°C and +95 kJ/mol (independent of temperature). What is free-energy change for this reaction at 200°C when partial pressures of CO, H2 and CH3OH are 8.0, 8.0 and 0.05 bar. 23.68 kJ/mol O-23.68 kJ/mol O-52.68 kJ/mol 52.68 kJ/mol
For the reaction 2NO(g) + O2(g)- →2NO2(g) AH° = -114.2 kJ and AS° = -146.5 J/K The equilibrium constant for this reaction at 350.0 K is Assume that AH° and AS° are independent of temperature.
For the reaction 4HCI(g) + O2(g)→2H2O(g) + 2C2(g) AH° = -114.4 kJ and AS° = -128.9 J/K The equilibrium constant for this reaction at 267.0 K is Assume that AH° and AS° are independent of temperature.
8. Gaseous nitrosyl bromide, NOBr, is formed by the reaction 2NO(g) + Br,(g) 2 2NOBr(g) At 25°C, the equilibrium constant for this reaction is K, = 116 atm-1. The reaction as written is exothermic, or heat emitting. When the following amounts of the three gases are introduced into a 1-liter flask, is the reaction spontaneous in the forward or reverse direction, or is it at equilibrium? a) 0.045 atm NOBr, 0.01 atm NO, and 0.10 atm Br, at 25°C b) 0.045 atm NOBr, 0.10 atm NO, and 0.01 atm Br, at 25°C c) 0.108 atm NOBr, 0.10 atm NO, and 0.01 atm Br, at 0°C
1.Calculate the value of the Gibbs Free Energy at 298 K for the conversion of A to B if the enthalpy of the reaction is -6.13 kJ·mol-1 and the change in entropy is -24.4 J·K-1·mol-1: _______ KJ.mol^-1
Give typed explanation not written
Ag(+aq) + Cl-(aq) AgCl(s) ∆H = +112 kJIf ions are colorless, and AgCl is whiteWill the reaction appear “colorless” or “white” if:a) Some of the AgCl (s) is removed?b) The pressure is decreased?c) The temperature is raised?
The experiment is about spot tests for alcohols where sodium nitrite is added to concentrated sulfuric acid and a crystal of phenol. for the result it produced a dark deep green color. in adition to that the mixture was added to h20 and 10 percent NaOH solution for the result it also produced a dark deep green color Question what does the color of the results imply? explain
A student determines the value of the equilibrium constant to be 2.69×10-10 for the following reaction.Fe2O3(s) + 3H2(g)2Fe(s) + 3H2O(g)Based on this value of Keq:G° for this reaction is expected to be (greater, less) fill in the blank than zero.Calculate the free energy change for the reaction of 2.05 moles of Fe2O3(s) at standard conditions at 298K. G°rxn = ____kJ
Calculate the AH°, AS°, and AG° at 298 K for the following reaction: (Use the values found in Thermodynamic Properties to calculate your answers for questions a and b.) Al2O3(s) + 3 C(graphite) + 3 Cl₂(g) → 2 AICI 3(s) + 3 CO(g) 4.0 -64 a) ΔΗΟ kJ/mol b) AS° ✓ J/K.mol kJ/mol (Determine from the temperature, AH and AS) c) AGO 4.0 76.9 4.0 -89 (d) Is the reaction extensive at standard conditions and 298 K? O Yes O NO (e) Write the expression for K. (Format example: Kp = pHC12 / pH₂. pCl₂ would be entered as K_{p} = pHCI^{2}/pH_{2}. pCl_{2}.) Help chemPad XX (PCO)3 (pCl₂)³ ← Greek (PCO)^3/(pCl_2)^3 Your answer provides a different type of equation than was expected. (f) Calculate the value of K at 298 K 2.51e-16 X (Please answer to 3 significant figures.) (g) Estimate the value of K at 600 K. 1.79e-8 X (Please answer to 3 significant figures.)