For the endothermic reaction CaCO3 (s) <-----> CaO (s) + CO2 (g) Le Chtelier's principle predicts...
For the endothermic reaction CACO3(s) CaO(s) +CO2(8) Le Chatelier's principle predicts that will result in an increase in the number of moles of CO2. increasing the temperature decreasing the temperature increasing the pressure removing some of the CaCO3 (s) none of these
1) The reaction below is exothermic 2SO2 (g) + O2(g) ⇌ 2SO3(g) + heat Le Châtelier's Principle predicts that _______ will result in an increase in the number of moles of SO3 (g) in the reaction container. Which direction will the reaction shift: ? left or right A) increasing the volume of the container B) increasing the amount of SO2 C) removing some oxygen D) increasing the temperature E) decreasing the pressure 2) Consider the following reaction at equilibrium: 2SO2 (g) + O2 (g) ⇌ 2SO3 (g) + heat ΔH...
This equilibrium reaction is exothermic: 2SO2 (g) + O2 (g) <-> 2SO3 (g) (where <-> indicates equilibrium, or double headed arrows) Le Châtelier's principle predicts that __________ will result in an increase in the number of moles of SO3(g) in the reaction container. A) decreasing the liquid level B) removing some oxygen C) increasing the pressure D) increasing the volume of the container E) decreasing the pressure
CaCO3(s) ⇄ CaO(s) + CO2(g) 0.100 mol of CaCO3 and 0.100 mol CaO are placed in an 10.0 L evacuated container and heated to 385 K. When equilibrium is reached the pressure of CO2 is 0.220 atm. 0.300 atm of CO2 is added, while keeping the temperature constant and the system is allowed to reach again equilibrium. What will be the final mass of CaCO3? 7.47 g 12.54 g 18.01 g 2.00 g 10.01 g
Consider the following reaction at equilibrium, CaCO3(s) ↔ CaO(s) + CO2(g). Which of the following statements are true regarding this equilibrium? Select all that are True. a) If CaO(s) is added from the equilibrium mixture the reaction will remain unchanged. b) If CaO(s) is removed from the equilibrium mixture the reaction will shift to the left. c) If CO2(g) is added to the equilibrium mixture the reaction will shift to the right. d) If CO2(g) is added to the equilibrium...
Consider the reaction: CaCO3(s)⇌CaO(s)+CO2(g) An equilibrium mixture of this reaction at a certain temperature was found to have [CO2]= 0.458 M. What is the value of the equilibrium constant at this temperature?
12. At high temperatures, limestoned CaCO3 (s) e CaO (s) + CO2 (g,) If this reaction is run at 900°C and reaches equilibrium when [CO21-0.76 M, what is the value of Kp at this temperature? A. 0.76 B. 73 C. 56 D. 0.008 E. 96
CaCO3(s) = Cao (s)+CO2 (g) When heated strongly, solid calcium carbonate decomposes to produce solid calcium oxide and carbon dioxide gas, as represented by the equation above. A 2.0 mol sample of CaCO3(s) is placed in a rigid 100. L reaction vessel from which all the air has been evacuated. The vessel is heated to 898°C at which time the pressure of CO2(g) in the vessel is constant at 1.00 atm, while some CaCO3(s) remains in the vessel. a. Calculate...
For this question, consider the reaction: CaO(s) + CO2(g) --> CO2(g) + CaCO3(s). Part A: What is the value of ΣΔH°f_products? a) -1207 kJ b) -1028.6kJ c) -1522.4kJ d) -2524.1kJ Part B: What is the value of ΣΔH°f_reactants? a) -1207kJ b) -1544kJ c) -75.2kJ d) -1028.6kJ Part C: What is the heat of reaction? a) -202.1kJ b) -2235.6kJ c) -178.4kJ d) -195.2kJ Part D: Is the reaction endothermic or exothermic?
At 900 °C, K = 0.0108 for the reaction CaCO3(8) F CaO(s) + CO2(g) A mixture of CaCO3, CaO, and CO2 is placed in a 10.0-L vessel at 900 °C. For the following mixtures, will the amount of CaCO3 increase, decrease, or remain the same as the system approaches equilibrium? Part A 15.0 g CaCO3, 15.0 g CaO, and 4.25g CO2 increases decreases O remains the same Submit Request Answer Part B 2.50g CaCO3, 25.0 g CaO, and 5.66 g...