Concept explainers
According to Le Châtelier's principle, does the equilibrium shift in the direction of products or reactants when
a.
b.
c.
d.
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- 10. 1) Please choose the corect expression and circle it. Le chatelier's Principle Summarized Below Change Concentration Pressure Volume Shifts Equilibrium Change Equilibrium Constant yes/no yes/no yes/no yes/no yes/no yes/no yes/no yes/no yes/no yes/no Temperature Catalyst ii) 250:(g)+0:(3)2SO:(g) The position of equilibrium moves to the right/left if the concentration of SO; is increased. Co.(g) CO(g)+O( If we increase the pressure of COg), the system will shift towards the reactants/products because it has a fewer/more number of moles of gas. CIHH:0 HO'+Cl+Heat If we decrease the temperature, the reaction will proceed towards the reactants/products because the system must regenerate/used the heat that was lost/gain. iii) Will the equilibrium in reactionarrow_forward4:15 Consider the equilibrium system described by the chemical reaction below. At equilibrium, a sample of gas from the system is collected into a 1.25 L flask at 25.0 °C. The flask is found to contain 2.35 g of NO2, 9.60 g of N₂O, and 4.50 g of O₂. What is the value of Kc for this reaction? 4 NO₂(g) 2 N₂O(g) + 3 O₂(g) Question 8 of 10 Kc = Based on the given data, set up the expression for Kc. Each reaction participant must be represented by one tile. Do not combine terms. [0.0409]² [0.218] [0.113] ³ [0.0409]¹ 0.480 Once the expression is constructed, solve for Kc. 3.57 x 10³ 1 [0.175]² [0.141] [0.0409] [0.175]4 0.0642 Submit [0.113]² [0.0409]³ [0.175] [0.113]4 28.7 Tap here or pull up for additional resources RESET [0.0511] [0.175]³ [0.113] 15.8 13.6arrow_forwardConsider the following system at equilibrium: P4 (g) + 6 H2 (g) = 4 PH3 (g) ΔΗ 110. 5 kJ If the volume was increased, what changes would have to occur to reestablish equilibrium? Select 2 correct answer(s) The reaction would shift right. The concentration of PH3 would increase. The concentration of P4 would increase The reaction would shift left. The concentration of H2 would decrease.arrow_forward
- 6. What is the correct equilibrium constant (K.) expression for the following reactions? (4 points) 2SO2(g) + O2(g) 2SO3(g) 4Cu(s) + O2(g) 2Cu2O(s)arrow_forward.50 mol of I2 and .50 mol of Br2 are placed in a 1.00 flask and allowed to reach equilibrium. At equilibrium, the flask contains .84 mol of IBr. What is the value of the Kc for this reaction? I2(g) + Br2(g) ---> 2 IBr(g) Group of answer choices 110 4.0 11 40.arrow_forwardFlag question Hydrogen peroxide decomposes according to the following reaction: 2H₂O2(g) — 2H₂O(g) + O2(9) In a particular experiment, 3.5 moles of H₂O2 were placed in a 2.0 L reaction chamber at 307°C. After equilibrium was reached, 1.6 moles of H₂O2 remained. What is Ke for the reaction?arrow_forward
- please have legible hand writing for the letters and numbersarrow_forward2. Given the following equilibrium systems, determine the effect on the equilibrium when the named "stress" is applied. Normally the addition of solids or liquids to an equilibrium has no effect. a 2 NH3 (g) + 92.5 kJ 5 N2(9) + 3 H2 (9) Stress Equilibrium Shift 1 Remove N2 (9) 2 Add NH3 (9) 3 Remove H2 (9) 4 Remove NH3 (9) Add O2 (g) 6 Decrease Pressure 7 Add Heat b Ag2CO3 (s) 5 2 Ag1+ (aq) + CO32 (aq) Stress Equilibrium Shift 1 Add CO32" (aq) Remove Ag* (aq) 1+ 2 3 Add A92CO3 (s) 4 Add heat CANNOT ANSWER 5 Evapourate water offarrow_forward302(9) = 203(g) O decreasing the volume will shift equilibrium in the direction of products O decreasing the volume will shift equilibrium in the direction of reactants no shift occurs Submit Request Answer Part B (6)o + (6)007 = (6)z007 decreasing the volume will shift equilibrium in the direction of products decreasing the volume will shift equilibrium in the direction of reactants no shift occurs Reguest Answer Submit Part C P.(g) + 50,(g) = P,010 (4) O decreasing the volume will shift equilibrium in the direction of products O decreasing the volume will shift alibrium in the direction of reactants no shift occurs Submit Reguest Answer Part D 2s0,(9) + 2H,0(g) = 2H,S(g) + 30,(g) O decreasing the volume will shift equilibrium in the direction of products decreasing the volume will shift equilibrium in the direction of reactants O no shift occurs O Oarrow_forward
- 1:18 Question 1 of 16 Consider the following chemical reaction at equilibrium: 2NO₂(g) = N₂O4(9) A) reactants If the container's volume is increased by a factor of 2, in which direction will the equilibrium shift? B) product Submit C) neither the reactants nor the product Tap here or pull up for additional resourcesarrow_forward4:15 Consider the equilibrium system described by the chemical reaction below. If 0.1908 moles of CO2, 0.0908 moles of H₂, 0.0092 moles of CO, and 0.0092 moles of H₂O are present in a 2.00 L reaction vessel at equilibrium at 300 K, what is the value of Kc of the reaction at this temperature? Question 5 of 10 CO₂(g) + H₂(g) = CO(g) + H₂O(g) 1 Based on the given data, set up the expression for Kc. Each reaction participant must be represented by one tile. Do not combine terms. Kc = Once the expression is constructed, solve for Kc. [0.1908] [0.0092] [0.0908]² [0.0092]² 1.1 Submit [0.0908] [0.0184] [2.00] [0.0184]² = [0.0954] [0.0046] [300] 200 Tap here or pull up for additional resources RESET [0.0454] [0.1908]² [0.0954]² 4.9 × 10-³arrow_forwardPhosgene COCl2, one of the gases used in chemical warfare in World War I, is produced by this simple exothermic reaction. Co (g) + Cl2 (9) COC2 (g) Phosgene What effect (increase, decrease, remain the same) does each of the following operations have on the amount of phosgene present at equilibrium? a.) Adding more Cl2 at constant volume b.) Lowering the temperature c.) Removing CO d.) Adding a catalyst e.) Decreasing the volume of the containerarrow_forward
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