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Practice ProblemATTEMPT
The reaction of carbon dioxide and calcium hydroxide to produce calcium carbonate and water is represented by the equation
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Chemistry
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- Nitrogen dioxide is produced by reacting nitric oxide and oxygen: 2NO(g) + 02(g) $2NO2(g) ; AH° = -114 kJ Under which reaction conditions would you expect to have the greatest equilibrium yield of nitric oxide? O high temperature, high pressure O low temperature, high pressure O high temperature, low pressure O low temperature, low pressurearrow_forwardA mixture of PbS, O2, PbO, and SO2 are mixed in a reaction vessel and allowed to reach equilibrium. 2PbS(s) + 3O2(g) ⇋ 2PbO(s) + 2SO2(g) ΔH = –839.9 kJ Predict whether the reaction will shift towards the reactants, shift toward the products, or remain unchanged when the reaction mixture is heated. a) shift toward the products b) shift towards the reactants c) remain unchangedarrow_forwardFor the equilibrium: 2F2 (g) + O2 (g) + 600 kJ – 20F2 (g) where ke= 350 %3D Which of the following would result in a increase in the quantity of F2 Select 2 correct answer(s) removing some O2(g) increasing temperature (ignore pressure changes) removing some OF2(g) decreasing temperature (ignore pressure changes)arrow_forward
- Consider the equilibrium: 2NO2(g) <--> N2O4(g). Calculate ΔGo for the reaction given that the ΔHo = -58.03 kJ/mol and the ΔSo = -176.6 J/K at 100°C (A)-75.7 kJ/mol (B)7.84 kJ/mol (C)-124 kJ/mol (D)-40.4 kJ/molarrow_forwardGiven the following reaction: A (g) + 2B (g) + heat 2D (g) 20 (g) + Considering Le Châtelier's Principle, type in the boxes either no shift or shift to the right or shift to the left for each of the following cases: a) [D] is increased b) [C] is decreased c) Volume is decreased d) Temperature is increased e) Using a catalystarrow_forwardConsider the following system at equilibrium where ΔΗ° 108 kJ, and Kc = 1.29 × 10-2, at 600 K: = COC1₂ (g) ⇒ CO(g) + Cl₂ (9) If the temperature on the equilibrium system is suddenly decreased: The value of Ke increases decreases remains the same ccess The value of Qc Ois less than Ke Dis greater than K Ois equal to Ke The reaction must Orun in the forward direction to reestablish equilibrium run in the reverse direction to reestablish equilibrium Oremain in the current position, since it is already at equilibrium The concentration of Cl₂ will Oincrease decrease Oremain the same values I needed TONarrow_forward
- NO(g) =N{8) + 0(g) AH° = -90.2 kJ (a) (b) SO:(g) = SO(g) +O2(g) AH° = +98.9 kJ Using Le Chatelier's Principle, which of the following statements is TRUE? Select one: O a. Decrease in Temperature favors both Reaction (a) and Reaction (b) O b. None of the choices is correct. Oc. Increase in Temperature favors Reaction (a), which means that the decomposition is favored at high T. O d. Decreasing the reaction container will favor the formation of SO, and 02 (in Reaction (b)). O e. Increasing the reaction container volume will favor the formation of SO2 and 02 (in Reaction (b)).arrow_forwardA(g) + B(aq) <---> C(s) ΔHrxn= -453 kJ/mol If the [B] at equilibrium is decreased then the reaction willarrow_forwardConsider the following reaction at equilibrium: CO₂ (g) + H₂(g) → H₂O(g) + CO (g) 2 What would be the direction of the above reaction if we decrease the volume of the reaction container? The reaction will proceed (shift) to the left The reaction will proceed (shift) to the right. The reaction would not be affected.arrow_forward
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