For a certain reaction, K. = 25.5 and k = 33.3 M.s. Calculate the value of the reverse rate constant, k, given that the reverse reaction is of the same molecularity as the forward reaction. Express your answer with the appropriate units. Include explicit multiplication within units, for example to enter M.s include (multiplication dot)
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- how do i find the time it took for the mixture to react from A = 0.600 to 0.800 when catalyst was added to the reactant?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 figuresThe 503 cm3 reactor was purged of air and methanol vapor was introduced until the pressure was 5.01 kPa. Then the inside ampoule containing 68.6 mg of nitrosyl chloride, NOCl was broken. After equilibrium was established, the partial pressure of NOCl was found to be 2.76 kPa. The test temperature was 50.00 ° C. Find the reaction Δ_rG^o: CH3ONO (g) + HCl (g) → CH3OH (g) + NOCl (g), at the test temperature.
- b) what is the velocity of a reaction when [S] = 20 mM, where Vmax = 100 umol/mL*sec, and 4 Km = 2mM? can you show me how he got 98 umol / mL*sec, very close to Vmx, as [S]>>Km, at zero order of the kinetics. step by step pleaseSuppose that in the reaction 2O3 → 3O2, a closed system initially contains 5.80 mol O2 and 6.20 mol O3. Then, after some time, 7.10 mol of O3 is present. Determine the proportionality constant, ? at this moment.Two chemical reactions illustrated in sample A and sample B are setup with the starting materials shown at t = 0 s. The composition of the sample is checked 5 s later to determine the new distribution of reactants and products. Calculate the reaction quotient Q, for Sample B at t = 5 s.
- The value of steric factor, P for the reaction between NO and Cl2 giving NOCl and Cl is 0.018 at 298 K. If the experimental value of A is 4.0 x 109 L mol-1 s-1, estimate the collision diameter for the reaction.Consider 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)].Synthesis gas, a mixture that includes the fuels CO and H₂,is used to produce liquid hydrocarbons and methanol. It is madeat pressures up to 100 atm by oxidation of methane followed bythe steam re-forming and water-gas shift reactions. Because theprocess is exothermic, temperatures reach 950–1100C, and theconditions are such that the amounts of H₂, CO, CO₂, CH₄, and H₂O leaving the reactor are close to the equilibrium amounts forthe steam re-forming and water-gas shift reactions:CH₄(g) +H₂O(g) ⇌CO(g)+ 3H₂(g) (steam re-forming)CO(g) +H₂O(g) ⇌CO₂(g)+ H₂g) (water-gas shift) (a) At 1000.°C, what are ΔG° and ΔH° for the steam re-formingreaction and for the water-gas shift reaction? (b) By doubling the steam re-forming step and adding it to thewater-gas shift step, we obtain the following combined reaction:2CH₄(g) +3H₂O(g) ⇌CO₂(g) +CO(g)+ 7H₂(g) Is this reaction spontaneous at 1000.°C in the standard state? (c) Is it spontaneous at 98 atm and 50.% conversion (when 50.%of…
- In a batch reactor, reactant A is steadily converted into product B. The initialconcentration of reactant A is 100 mg/L. During a 10-hour reaction course, it wasobserved that the concentration of A in the reactor decreased at a constant rate of 10mg/L per hour. Based on the result, you can determine that the transformation reactionA→B follows ( ) with respect to reactant A.Ethylene (CH2CH2) is the starting point for a wide array of industrial chemical syntheses. For example, worldwide about 8.0 x 1010kg of polyethylene are made from ethylene each year, for use in everything from household plumbing to artificial joints. Natural sources of ethylene are entirely inadequate to meet world demand, so ethane (CH3CH3) from natural gas is "cracked" in refineries at high temperature in a kinetically complex reaction that produces ethylene gas and hydrogen gas. Suppose an engineer studying ethane cracking fills a 30.0L reaction tank with 24.0atm of ethane gas and raises the temperature to 800.°C. He believes Kp= 0.040 at this temperature. Calculate the percent by mass of ethylene the engineer expects to find in the equilibrium gas mixture. Round your answer to 2 significant digits. Note for advanced students: the engineer may be mistaken about the correct value of Kp, and the mass percent of ethylene you calculate may not be what he actually observes.For the reaction CH4 + H2O— CO + 3H2 assume there are present initially 2 moles of CH4 1 mole of H2O and l mole of CO and 4 moles of H,. Determine the expression for the mole fractions as a function of the reaction coordinate.