Assume for some DNA (molar mass: 10000DA), the AGº of denaturation is -20KJ/mol at 350K. In an experiment we dissolve 1g of the dsDNA in 1L of water at 350K. At the very beginning (t=0), all the sample was in the double helix form. What is the reaction quotient Q at
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- The value of ΔS° for the catalytic hydrogenation of acetylene to ethane, C2H2 (g) + 2H2 (g) → C2H6 (g) is __________ J/K∙ mol. A) -76.0 B) +440.9 C) -232.5 D) +232.5 E) +28.7The reaction glucose + phosphate ⇔ glucose-6-phosphate + H2O has ΔG° = 13.8 kJ mol-1. Calculate ΔGrxn in kJ mol-1 at 37.0 °C when [glucose] = 19.0 mmol L-1, [phosphate] = 6.90 mmol L-1, [glucose-6-phosphate] = 1.70 mmol L-1, and [H2O] = 55.5 mol L-1. (R = 8.3145 J mol-1 K-1)(a) Is the standard free-energy change, ΔG°, always largerthan ΔG? (b) For any process that occurs at constant temperatureand pressure, what is the significance of ΔG = 0?(c) For a certain process, ΔG is large and negative. Doesthis mean that the process necessarily has a low activationbarrier?
- The value of ΔS° for the catalytic hydrogenation of acetylene to ethene, C2H2 (g) + H2 (g) → C2H4 (g) is __________ J/K∙ mol. Substance S (J/K-mol) C2H2 200.8 H2 130.6 C2H4 219.4 a. -112.0 b. 550.8 c. -18.6 d. 112.0 e. 18.6True or False: 1. The initial concentration of an intermediate is assumed as 0 when using steady-state approximation. 2. A spontaneous reaction with ΔG = -1070 J/mol happens at 562 K, the Keq of this process is less than 1.Which processes shown in this figure involve the phasetransition H2O(l )----->H2O(g)?
- What are Pseudo unimolecular reactions? Explain with the help of a suitable example.Sucrose is hydrolyzed to glucose and fructose in a classic experiment in kinetics. The reaction is catalyzed by the enzyme invertase. Using the following data, determine, by Lineweaver-Burk method, whether the inhibition of this reaction by 2 M urea is competitive or noncompetitive Sucrose concentration (M) V, No I (arbitrary unit) V, With I (arbitrary unit) 0.0292 0.182 0.083 0.0584 0.265 0.119 0.0876 0.311 0.154 0.117 0.330 0.167 0.175 0.372 0.192When nitric acid is produced industrially, nitrogen monoxide, NO, is first formed at high temperature. Bakefetr reacts NO on cooling further with oxygen to nitrogen dioxide: 2 NO(g) + O2 ⇌ 2 NO2 (g) Table 1: Thermodynamic data at 25°C. Bond ΔfHom Som Cop,m NO(g) 90.25 210.76 29.34 O2(g) 0.00 205.14 29.36 NO2(g) 33.18 240.06 37.20 1) Calculate (with all relevant intermediate calculations) the standard reaction Gibbs free energy, ΔrG25o, for reaction (1) at 25°C from the data in Table 1 2) Calculate (with all relevant intermediate calculations) the equilibrium constant K25, for reaction (1) at 25°C. 3) Industrially, however, the reaction does not proceed at 25°C but at 500°C. Therefore, calculate (with all relevant intermediate calculations) the standard reaction Gibbs free energy, ΔrG500o, for reaction (1) at 500°C under the assumption that the standard molar heat capacities, Cop, in Table 1 are independent of temperature in the interval [25°C, 500°C]
- The activation energy of a certain gas reaction is 15.4 kJ/mol. Estimate the fraction of collisions that posses or exceed this value at A.) 298 K and B.) 600K. About how many times faster is the reaction when the temperature is doubled here? (Show all work)Calculate the entropy of activation for a collision between two structureless particles at 450 K, taking M = 92 g mol−1 and σ = 0.45 nm2.Combustion of glucose ( C6H12O6 ) is the main source of energy for animal cells: C6H12O6 ( s ) + 6O2 ( g ) → 6CO2 ( g ) + 6H2O ( l ) =ΔGrxn37°C−2872.kJ This energy is generally stored as ATP (adenosine triphosphate) molecules, which can release it when convenient by hydrolysis ("water-assisted decomposition") into ADP (adenosine diphosphate) molecules and a phosphate anion, often given the symbol Pi in biochemistry: ATP ( aq ) → ADP ( aq ) + Pi ( aq ) =ΔGrxn−35 to 70kJ The actual amount of free energy released by the hydrolysis of ATP varies, depending on the exact conditions inside the cell. Suppose under certain conditions hydrolysis of ATP actually releases −51.3/kJmol . Calculate the maximum number of ATP s that could be created from ADPs and Pi by the combustion of a molecule of glucose. Your answer must be a whole number.