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Pentene (C5H10) reacts with ethanoic acid to form pentyl ethanoate, the equilibrium CH3CO2H + C5H10 ➡ CH3CO2C5H11 being established when a solution of 0.020 moles of pentene and 0.010 moles of acetic acid in 600cm3 of an inert solvent was allowed to reach equilibrium at 150C, 0.0090 moles of pentyl ethanoate was formed.
- Write down an expression for the equilibrium constant Kc for the above reaction.
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- Pentene (C5H10) reacts with ethanoic acid to form pentyl ethanoate, the equilibrium CH3CO2H + C5H10 ➡ CH3CO2C5H11 being established when a solution of 0.020 moles of pentene and 0.010 moles of acetic acid in 600cm3 of an inert solvent was allowed to reach equilibrium at 150C, 0.0090 moles of pentyl ethanoate was formed. How many moles of pentene and ethanoic acid were present in the solution after equilibrium had been attained?Pentene (C5H10) reacts with ethanoic acid to form pentyl ethanoate, the equilibrium CH3CO2H + C5H10 ➡ CH3CO2C5H11 being established when a solution of 0.020 moles of pentene and 0.010 moles of acetic acid in 600cm3 of an inert solvent was allowed to reach equilibrium at 150C, 0.0090 moles of pentyl ethanoate was formed. Calculate the equilibrium concentration of the following in mol/dm3 C5H10, CH3CO2H, & CH3CO2C5H11 Hence Calculate KcThe equilibrium constant for the gas-phase isomerization of borneol (C10H17OH) to its isomer isoborneol at 503 K is 0.106. A mixture consisting of 7.50 g of borneol and 14.0 g of isoborneol in a container of volume 5.0 dm3 is heated to 503 K and allowed to come to equilibrium. Calculate the mole fractions of the two substances at equilibrium.
- The equilibrium constant for the gas-phase isomerization of borneol, C10H17OH, to isoborneol at 503 K is 0.106. A mixture consisting of 6.70 g of borneol and 12 .5 g of isoborneol in a container of volume 5.0 dm3 is heated to 503 K and allowed to come to equilibrium. Calculate the mole fractionsof the two substances at equilibrium.The following synthesis reaction was conducted at 325K: A2(g) + 3B2(g) ⇌ 2AB3(g). At this temperature, KP = 5.49 x 10-6. In a 3.00L flask, 0.175atm of A2(g) and 0.410atm of B2(g) are added and allowed to reach equilibrium. Calculate the pressure of AB3(g) in the system (in atm).Prebiotic reactions are reactions that might have occurred under the conditions prevalent on the Earth before the first living creatures emerged and that can lead to analogues of molecules necessary for life as we now know it. To qualify, a reaction must proceed with a favourable rate and have areasonable value for the equilibrium constant. An example of a prebiotic reaction is the formation of 5-hydroxymethyluracil (HMU) from uracil and formaldehyde (HCHO). Amino acid analogues can be formed from HMU under prebiotic conditions by reaction with various nucleophiles, such as H2S, HCN, indole, imidazole, etc. For the synthesis of HMU at pH = 7. the temperature dependence of the rate constant is given bylog k,/(dm3 mol-1 s-1) = 11.75- 5488/(T/K)and the temperature dependence of the equilibrium constant is given bylog K = -1.36 + 1794/(T/K)(a) Calculate the rate constants and equilibrium constants over a range of temperatures corresponding to possible prebiotic conditions, such as 0-50 oC.…
- Suppose that in an industrial process, N2 at 1.00 bar is mixed with H2 at 3.00 bar, for a total pressure of 4.00 bar, and the two gases are allowed to come to equilibrium with the product ammonia in a reactor of constant volume (in the presence of a catalyst, so the reaction proceeds quickly). At the temperature of the reaction , it has been determined experimentally that K = 977 for reaction R2. What are the equilibrium partial pressures of the three gases?In the gas-phase reaction A + B ⇋ C + 2 D, it was found that, when 2.00 mol A, 1.00 mol B, and 3.00 mol D were mixed and allowed to come to equilibrium at 25 °C, the resulting mixture contained 0.79 mol C at a total pressure of 1.00 bar. Calculate (i) the mole fractions of each species at equilibrium, (ii) K, and (iii) ΔrG⦵.Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 1.87 × 10⁻³ at a certain temperature. If 5.00 g of solid PH₃BCl₃ and 0.0700 g of BCl₃ are added to a 4.500 L reaction vessel, what will the equilibrium concentration of PH₃ be? PH₃BCl₃(s) ⇌ PH₃(g) + BCl₃(g) 1.) Set up the expression for Qc and then evaluate it to determine the direction of the reaction. Do not combine or simplify terms 2.) Based on the given values and your value for Qc, set up ICE table in order to determine the unknown. 3.) Based on your ICE table, set up the expression foe Kc in order to determine the unknown. 4.) Based on your ICE table and expression for Kc, solve for the partial pressure of PH3, at equilibrium.
- At 2300 K, the equilibrium constant for the formation of NO (g), is K = 1.7 x 10-3. N2 (g) + O2 (g) NO 2 NO (g) (a) The analysis shows that the concentrations of N2 and O2 are both 0.25 mol L-1, and that ofNO is 0.0042 mol L-1, under certain conditions. Is the system in balance? In caseaffirmative or negative, substantiate your answer.(b) If the system is not in equilibrium, in which direction should the reaction proceed?(c) When the system is in equilibrium, what are the equilibrium concentrations?The concentration of calcium carbonate in a sample of water saturated with the solid was found to be 7.00 x 10-5 moldm-3 at 200C. What is the solubility product of calcium carbonate at this temperature?For the reaction PCl5(g) <=> PCl3(g) + Cl2(g), the equilibrium constantKc = 1.1 * 10-2 at 400 K. What is the equilibrium constant for the reactionPCl3(g) + Cl2(g) <=> PCl5(g) at 400 K?