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- 7) For the reaction CO(g) + 3 H2(g) = H2O(g) + CH4(g), Kc = 190 at 1000 K. If a vessel is filled with these gases such that the initial concentrations are [CO] = 0.036 M, [H2] = 0.045, [H2O] = 0.020, 7) %3D %3D %3D and [CH4] = 0.031, in which direction will a reaction occur and why? A) it is at equilibrium because Q = 190 B) toward products because Q = 4.1 C) toward reactants because Q = 0.24 D) toward products because Q = 0.38 %3D %3D %3D %3D E) toward reactants because Q = 61 %3DConsider the reaction: NO(g) + C₂H₂(g) → HCN(g) + CO(g) + H(g), is The Arrhenius expression for the reaction is k(T) = 8.97 x 10-¹2 cm³ molec-¹ s¹ exp{-218 kJ mol-¹/RT} over the temperature range 1100 - 1500 K. Using transition state theory, calculate AH* and AS* for this reaction at 1300 K.O Ni(H₂O)2+ (aq) + 3SCN- (aq) = Ni(SCN); (aq) + 6H₂0(1) (a) Write the Kc expression for this equilibrium. (b) Would there be a shift to the right or to the left if KSCN solution was added to a solution containing this equilibrium? Explain your answer.
- (a) If Qc > Kc, how must the reaction proceed to reachequilibrium? (b) At the start of a certain reaction, onlyreactants are present; no products have been formed.What is the value of Qc at this point in the reaction?|The Kc for CO(g) + 3H,(g) = CH,(g) + H2O(g) is 9.17 x 10-2. If a 3.5L vessel is set up with .o155 mol CO, 3.50 x 10-3 mol H2, .0100 mol CH4, and 7.60 x 10-4 mol H2O, what is the reaction quotient Qc? In which direction will this reaction proceed to reach equilibrium?1. (a) If Qc < Kc, in which direction will a reaction proceed in order to reach equilibrium? (b) What condition must be satisfied so that Qc = Kc? %3D
- Iodine is sparingly soluble in water but much more so in carbon tetrachloride. The equilibrium constant, also called the partition coefficient, for the distribution of I2 between these two phases I2(aq) =12(CCI4) is 83 at 20°C. (a) A student adds 0.028 L of CCI4 to 0.213 L of an aqueous solution containing 0.037 g Iɔ. The mixture is shaken and the two phases are then allowed to separate. Calculate the fraction of I, remaining in the aqueous phase. 4.08.396 X (b) The student now repeats the extraction of I2 with another 0.028 L of CCI4. Calculate the fraction of I2 from the original solution that remains in the aqueous phase. 4.0 .0002608 (c) Compare the result in (b) with a single extraction using 0.056 L of CCI4. Comment on the difference. After a single extraction using 0.056 L of CCI4, the fraction of I2 that remains in the aqueous phase is 49 4.3 This result is larger than the result in (b), which means that a single large extraction is not as efficient as two separate smaller…Iodine is sparingly soluble in water but much more so in carbon tetrachloride. The equilibrium constant, also called the partition coefficient, for the distribution of I2 between these two phases I2(aq) =12(CCI4) is 83 at 20°C. (a) A student adds 0.028 L of CCI4 to 0.213 L of an aqueous solution containing 0.037 g I2. The mixture is shaken and the two phases are then allowed to separate. Calculate the fraction of I2 remaining in the aqueous phase. 4.0 (b) The student now repeats the extraction of I2 with another 0.028 L of CCI4. Calculate the fraction of I2 from the original solution that remains in the aqueous phase. 4.0 (c) Compare the result in (b) with a single extraction using 0.056 L of CCI4. Comment on the difference. After a single extraction using 0.056 L of CCI4, the fraction of I2 that remains in the aqueous phase is 40 This result is larger than the result in (b), which means that a single large extraction is not as efficient as two separate smaller extractions.2:26 1 Question 23 of 25 Submit Construct the expression for Kp for the following reaction. 2 C3H18(1) + 25 02(g) = 16 CO2(g) + 18 H20(1) 1 Drag the tiles into the numerator or denominator to form the expression. Kp = %3D 5 RESET 2(Pc,H») 25(Pc,H.) (PCaH,)25 Ро, 2(Ро.) 25(Ро.) (Рo) (Po.)25 Pco, 2(Pco,) 16(Pco.) (Pco,)? (Pco.)"® PH,0 2(Рн.о) 18(Рн,о) (Рн.о)? (PH,0)18
- Consider the water-gas shift reaction C02 + H2 → CO + H,0 Assume that equilibrium constant K(T) is K(1100K)=1 and K(1600 k)=3 and K(2100 K)=4.9. Further assume that the global forward reaction rate coefficient is kf = AT" exp (-) where 0 = 15000K, n =; and A = 1010 cm³mol-1s-1. Estimate the global reverse rate coefficient k, at 1100, 1600 and 2100 K(a) What are the units usually used to express the rates ofreactions occurring in solution? (b) As the temperatureincreases, does the reaction rate increase or decrease?(c) As a reaction proceeds, does the instantaneous reactionrate increase or decrease?How do I find the Reaction Quotient, E0cell and Ecell?