The rate constant k for a certain reaction is measured at two different temperatures: temperature k 5.9 x 1010 3.5 x 1010 Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E for this reaction. Round your answer to 2 significant digits. 198.0 °C E = 137.0 °C mol ☐x10 X S
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- The table below shows the time-temperature course during reaction of NaOH sample of 2.02 g with 169 mL of 1M HCl.Plot the data, evaluate ΔT and calculate the reaction enthalpy. time/s t/ oC 0 19.75 15 19.80 30 19.85 45 19.89 60 19.97 75 20.02 90 19.98 105 20.13 120 20.34 135 20.87 150 21.62 165 22.40 180 23.20 200 24.49 220 25.81 240 27.09 260 27.37 280 27.35 300 27.34 320 27.31 340 27.31 360 27.27 380 27.25 400 27.24 Give your calculated enthalpy in kJ·mol-1to 3 significant figuresIn the gas phase reaction 2 A(g) + B(g) ⇋ 3 C (g) + 2 D (g), it was found that when 1.00 mol A, 2.00 mol B and 1.00 mol D were mixed and allowed to come to equilibrium at 25oC, the resulting mixture contained 0.9 mol C at a total pressure of 1.00 bar. Calculate the mole fractions of each species , Kx is , Kp is and isAssume no acid-base catalysis occurs and the following data: Under biological conditions (310 K) 1. dGb = -20.00 kJ/mol. 2. The dG of E +S binding to ES (dGs) is -3.00 kJ/mol. 3. dGd mismatch of energy in ES = +2.00 kJ/mol. What is the catalytic power (kcat/k_uncat) at 360 K? Use 1 decimal place.
- The global emissions of methane have been estimated to be near 9,390 million metric tons of CO2 equivalent, assuming there is a GWP of 25. Calculate the residence of methane in the atmosphere. If the concentration of methane in the atmosphere is 1.55 ppmv. Can an expert, please show me how to solve the question above?What is the Importance of kinetics and chemical equilibria in the development of point of care technologies? Please provide at least 2 insights. You may use this as reference: https://knowledge.electrochem.org/encycl/art-g01-glucose.htmif there is an enzyme is catalyzed reaction that is at equilibrium and it produces 0.1 M of substrate as well as 0.05 M of product. What do we know about this reaction under standard conditions?
- In the synthesis of hydrocarbons, the carbon source is carbon dioxide. Although the CO2 concentra?on in the atmosphere raises at a drama?c speed, point sources are probably the easier sources for a PtX process. Iden?fy 3 possible point sources, explain why CO2 is formed and what challenges each of the three CO2 streams presentsThe following reaction is carried out with [PCl5]i = 0.400 M at 25°C (i means initial) The reaction: PCl5(g)⇌PCl3(g)+Cl2(g) K= 0.00105 Using the small x approximation and "test x", could you please find the percent to two decimal places when testing x? Thank you so much.Hey, The issue I am having here is calculating the partial pressure, if I use P=(n/V)*R*T then I get the partial pressure of H2 as 23.2 but according to the teacher it should be 11.585 so instead of just calculating the the total moles of H2 in the reaction should n be a molar fraction?
- Find ∆H as a function of T for the reaction: CO2 (g) + C (s, graphite) = CO Given that ∆H 293= 41,400 cal Cp CO2= 5.166+15.77×10^-3 T - 95.78×10^-3 T² + 2.260×10^-9 T³ Cp CO= 6.6 + 2×10^-3 T Cp C (s, graphite)= 2.673 + 2.617×10^-3 T - 1.169×10^-5 T^-2Consider the reaction Mn+ + ne- ⇌ M. If ΔG*c = ΔG* + (1-α)nFE and η = E – Eeq, prove that ic = io exp[-(1-α)nFηa)/RT)].In Heat of solution from Solubility experiment: the slope of plot of Ln Sversus 1/T (K) = - 534 and the intercept = 2.964, calculate the solubility S