Suppose that a gas phase reaction: 2A(g) 2B(g) +C(g) follows second order kinetics and goes to completion. If the reaction is allowed to proceed in a constant volume vessel at an initial pressure of 4 bar (only A is initially present). The total pressure of the reaction mixture at t= 0o is
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- Ethanol vapours were allowed to completely fill a large jug with a volume of 15.5L. The ethanol was burned yielding 5.5mL of pure liquid water in the bottom of the jug at the end of the reaction. C2H5OH + 3 O2 ? 2 CO2 + 3 H20 If the room temperature was 21.5 oC and the pressure was 0.996atm, calculate the percentage yield of the water gathered in the jug.Suppose that the typical diffusion coefficient for a reactant in aqueous solution at 25 °C is 5.2 × 10−9 m2 s−1. If the critical reaction distance is 0.4 nm, what value is expected for the second-order rate constant for the diffusion-controlled reaction?A typical diffusion constant for small molecules in aqueous solution at 25 °C is 6 × 10−9 m2 s−1. If the critical reaction distance is 0.5 nm, what value is expected for the second-order rate constant for a diffusion-controlled reaction?
- a. Ethanol vapours were allowed to completely fill a large jug with a volume of 15.5L. The ethanol was burned yielding 5.5mL of pure liquid water in the bottom of the jug at the end of the reaction. C2H5OH + 3 O2 ? 2 CO2 + 3 H20 If the room temperature was 21.5 oC and the pressure was 0.996atm, calculate the percentage yield of the water gathered in the jug. b. A 10.0 mL sample of sulfuric acid with an unknown concentration was titrated with 3.5 x 10-4 mol/L NaOH. If 20.4mL of the sodium hydroxide was required to completely neutralize the acid, determine the concentration of the sulfuric acid in the sample. Then, determine the original pH of the sulfuric acid sampleEthylene (CH2CH2) is the starting point for a wide array of industrial chemical syntheses. For example, worldwide about 8.0x10^10 kg 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 75.0 L reaction tank with 23.0 atm of ethane gas and raises the temperature to 750.°C. He believes Kp=6.0 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.The Gibbs free energy change at standard state for the reaction A+B+C->D+E is known to equal -20 kJ/mol. What is the activation energy for the forward rate constant for this reaction if the forward rate constant increases by 72% at T=44.6C compared to its value at 25 celsius?
- The Lineweaver-Burke equation of a reaction is 1/v = 0.3 (1/s) + 0.2.Question: What's the Vmax of the reaction?Derive the integrated form of a third-order rate law v = kr[A]2[B] in which the stoichiometry is 2 A + B → P and the reactants are initially present in (a) their stoichiometric proportions ([B]0 = 12[A]0); (b) with B present initially in twice that amount ([B]0 = [A]0). Express your rate law in terms of [A]0, [B]0, and x, where [A] = [A]0 − 2x.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.
- Derive an expression for the time dependence of the degree of polymerization for the stepwise polymerization of a hydroxyacid HO−R−COOH for which the rate law is d[A]/dt = −kr[A]2[OH], where A denotes the carboxylic acid group.Write down the kinetic equation for a simple reaction in a homogeneous medium 2A + B = 2C. Indicate the general and in relati on to all reactants reaction ordersa. Express the rate in terms of change of concentration of A with respect to time where 2A + B -> products, rate = k[A]-1. b. Give the derived integrated rate law.