Answer is E)
For this Reaction, K = 1/Pco2
Using, LogK = -∆G°/2.303RT
logK = 130900/2.303×8.314×298
logK = 22.94
K = 1022.94
1/Pco2 = 1022.94
Pco2 = 1/1022.94
= 1.14×10-23 atm
9. Consider the following reaction: inputted, <GO CaO(s) + CO2(g) - CaCO3(s); AG° = -130.9 kJ...
Consider the following reaction: CaCO3(s)→CaO(s)+CO2(g). Estimate ΔG∘ for this reaction at each of the following temperatures. (Assume that ΔH∘ and ΔS∘ do not change too much within the given temperature range.) a.320 K b.1040 K c.1480 K Predict whether or not the reaction in part A will be spontaneous at 320 K . Predict whether or not the reaction in part B will be spontaneous at 1040 K . Predict whether or not the reaction in part C will be...
Consider the following reaction: CaCO3(s)→CaO(s)+CO2(g). Estimate ΔG∘ for this reaction at each of the following temperatures. (Assume that ΔH∘ and ΔS∘ do not change too much within the given temperature range.) A) 320 K B) 1045 K C) 1435 K Predict whether each reaction will be spontaneous or not.
Consider the following reaction: CaCO3(s)→CaO(s)+CO2(g). Estimate ΔG∘ for this reaction at each of the following temperatures. (Assume that ΔH∘ and ΔS∘ do not change too much within the given temperature range.) Part A: 300 K Part B: 1040 K Part C: 1445 K Part D: Predict whether or not the reaction in part A will be spontaneous or nonspontaneous at 300 K Part E: Predict whether or not the reaction in part B will be spontaneous at 1040 K Part...
Consider the following reaction: CaCO3(s)→CaO(s)+CO2(g) Estimate ΔG∘ for this reaction at each of the following temperatures. (Assume that ΔH∘ and ΔS∘ do not change too much within the given temperature range.) Predict whether or not the reaction in each part will be spontaneous. Express your answer using one decimal place and in kJ. A. 300 K B. 1050 K C. 1410 K
Consider the following reaction: CaCO3(s)→CaO(s)+CO2(g). Estimate ΔG∘ for this reaction at each of the following temperatures. (Assume that ΔH∘ and ΔS∘ do not change too much within the given temperature range.) Part A 315 K ΔG∘ Δ G ∘ = nothing kJ Part B 1085 K ΔG∘ Δ G ∘ = nothing kJ Part C 1465 K ΔG∘ Δ G ∘ = nothing kJ Part D Predict whether or not the reaction in part A will be spontaneous at 315...
Consider the following reaction: CaO (s) + CO2 (g) → CaCO3 (g) If 12.9 g of carbon dioxide, CO2, react, how many grams of calcium carbonate, CaCO3, are produced?
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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
Limestone is predominantly, CaCO3, which can undergo the reaction. CaCO3(s) ===> CaO(s) + CO2 (g). We know from experience that this reaction is not spontaneous, yet ∆S for the reaction is positive. How can the second law of thermodynamics explain that this reaction is not spontaneous?
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...