Consider the following process: NaCl(s) water−→−−water→ Na+(aq) + Cl-(aq); ΔH = +4.2 kJ/mol Under what conditions (temperature) would you expect this process to be spontaneous? Select a relatively high temperature and a relatively low temperature, calculate (estimate) the relative values of ΔG to support your conclusion. The entropy increases in this process Please insert an image of your work
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Consider the following process:
NaCl(s) water−→−−water→ Na+(aq) + Cl-(aq); ΔH = +4.2 kJ/mol
Under what conditions (temperature) would you expect this process to be spontaneous? Select a relatively high temperature and a relatively low temperature, calculate (estimate) the relative values of ΔG to support your conclusion. The entropy increases in this process
Please insert an image of your work
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- Describe how you would make the following solution containing two enzymes. 1 mL total volume in Buffer X with 10nM of enzyme A and 50nM of enzyme B You are given a solution of enzyme A at 1 mg/mL and a solution of enzyme B at 1 mg/mL. The molecular weight of enzyme A is 75,000 g/mol and the molecular weight of enzyme B is 130,000 g/mol.Answer the following questions yes or no (Y/N): Is the michaelis-menten equation valid under experimental conditions? Is the michaelis-menten equation only valid for reactions that are at equilibrium? Is extrapolation to Vm inaccurate, but Km is accurately determined in the michaelis-menten equation? Is the michaelis-menten equation nonlinear? Is extrapolation to Vm inaccurate, and therefore Km cannot be accurately determined in the michaelis-menten equation?For this reaction: 6CO2 + 6H2O → C6H12O6 + 6O2, the products have 2760 kJ/mole more free energy than the reactants. So, which of the following statements best describes the reaction? a The reaction is endergonic because it converts molecules with less free energy to those with more free energy. b The reaction is exergonic because it converts molecules with less free energy to those with more free energy. c The reaction is exergonic because it converts molecules with more free energy to those with less free energy d The reaction is endergonic because it converts molecules with more free energy to those with less free energy.
- Write a stepwise mechanism for the following reaction.The phosphoryl group transfer potentials for glucose-1-phosphate and glucose-6-phosphate are 20.9 kJ/mol and 13.8 kJ/mol, respectively. (a) What is the equilibrium constant for the reaction shown below at 25 °C? (b) If a mixture was prepared containing 1 m glucose-6-phosphate and 1 x 10-3 M glucose-1-phosphate, what would be the thermodynamically favored direction for the reaction?Inspired by the sacrifices done by the protector Naevis, Winter was determined to continue Naevis’ experiments with the compounds discovered from Kwangya. Winter searched for all the surviving data from the aftermath of the battle against the Black Mamba and found the following graphs and values. The general reaction for the formation of compound Ae is as follows: Nvs + We + Luv + You → Ae (See picture) Table 1. Reaction rates of various Ae formation runs at 30 oC. Run Concentration of each component in Solution Initial rate, M/s [Nvs], M [We], M [Luv], M [You], M 1 0.053 0.082 0.092 0.046 8.44 x 10-10 2 0.029 0.096 0.092 0.034 1.87 x 10-10 3 0.053 0.074 0.092 0.034 6.24 x 10-10 She also found a numerical value for k = 7.1 x 10-5 but was not able to find its unit. Help her find the following: Order of the reaction with respect to Luv (round off to the nearest whole number) Unit of the rate constant Rate Law of…
- Derive an Equation that explains the realtionship between kE and kN with respect to the equilibrium constants provided in the reaction scheme provided below. Assume that the enzyme must bind with A before it binds with B. The two reactions are related by the following reaction scheme:provided below.For an enzyme kinetics experiment, a student prepared a reaction mixture by mixing 450 microliters of 0.75mM PNPP with 4.25ml of 0.2M Tris-HCl buffer. When he is ready to measure the absorbance, he added 0.3ml of Alkaline Phosphatase to the mixture and mixed thoroughly. What is the substrate concentration at the beginning of the reaction in mM ?For the reaction A → B at 298 K, the change in enthalpy is −7 kJ · mol−1and the change in entropy is −25 J · K−1 · mol−1. Is the reaction spontaneous? If not, should the temperature be increased or decreased to make the reaction spontaneous?
- For the series of reactions below, what is the overall reaction and the value of ∆Go’(kJ/mol) for this set of reactions? Is the reaction spontaneous? (1) 2 Pi+ H2O ➔Pyrophosphate+ H2O (with 5 mM Mg2+) (2) (Mg)Pyrophosphate + AMP ➔(Mg)ATP (3) (Mg)ATP + creatine ➔creatine-phosphate + (Mg)ADPIf you measured the rate of reaction at 20°C to be 1.11 x 10-5 M/s when using 0.080 M I1- and 0.040 M S2O82-. Approximately how long will the reaction take if you were to increase the temperature to 30 °C?The decomposition of crystalline N2O5 N2O5(s) → 2NO2(g) + 1/2O2(g) is an example of a reaction that is thermodynamically favored, even though it absorbs heat. At 25 °C we have the following values for the standard state enthalpy and free energy changes of the reaction: ∆H° = +109.6 kJ/mol ∆G° = -30.5 kJ/mol (a) Calculate ∆S ° at 25 °C. (b) Why is the entropy change so favorable for this reaction?