Delta S is positive for the reaction__.
a) CaO(s)+CO2(g)-->CaCO3(s)
b) N2(g)+3H2(g)-->2NH3(g)
c) 2SO3(g)--->2SO2(g) + O2(g)
d) Ag+(aq)+Cl-(aq)--->AgCl(s)
e) H2O(l)--->H2O(s)
*I know that C is the correct answer, I just need a detailed explanation as to why that is the correct answer.
Delta S is positive for the reaction__. a) CaO(s)+CO2(g)-->CaCO3(s) b) N2(g)+3H2(g)-->2NH3(g) c) 2SO3(g)--->2SO2(g) + O2(g) d)...
IU. AS is positive for the reaction A) CaO (s) + CO2 (g) CaCO3 (S) B) N2 (g) + 3H2(g) → 2NH3 (g) C) 2503 (g) - 2802 (g) + O2 (g) D) Ag+ (aq) + Cl- (aq) → AgCl (s) E) H20 (1) + H20 (s) 11. AS is positive for the reaction A)2 Ca(s) + O2 (g) 2 Cao (s) B) 2 KClO3 (s) 2KCI(S) + 30 (g) C) HCl (8) + NH3 (8) ► NH4Cl (s) D)...
given the following reaction caco3(s)--->cao(s) + co2(g) delta h = 178.1kj C(s,graphite) + O2(g) ---> CO2(g) deltaH=-393.5kj the enthalpy of the reaction CaCO3(s)--->CaO(s) + C(s,graphite) + O2(g) is ________kj.
Calculate D (delta) Hrxn for the reaction: CaO(s) + CO2(g) -----> CaCO3(s) given these reactions and their DH’s: 1) Ca(s) + CO2(g) + ½ O2(g) -----> CaCO3(s) D(delta)H = -814.1kJ 2) 2Ca(s) + O2(g) -----> 2 CaO (s) D(delta)H = -1269.8kJ
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...
Which of the following processes has a negative AS? A) CaCO3(s) → Cao(s) + CO2(g) B) H2O(g) → H2O(s) C) CO2(s) + CO2(g) D) C6H1206(s) → C6H1206(aq) E) AS cannot be negative
Predict the sign of the entropy change, ΔS∘, for each of the reaction displayed. Drag the appropriate items to their respective bins. Pb2+(aq)+2Cl−(aq)→PbCl2(s) CaCO3(s)→CaO(s)+CO2(g) 2NH3(g)→N2(g)+3H2(g) 2Mg(s)+O2(g)→2MgO(s) C5H12(g)+8O2(g)→5CO2(g)+6H2O(g) H2O(l)→H2O(g) Positive Negative
8) The Kh for A A) 9.33 is 4.9 10-10 What is the pH of a 0.0627 M aqueous NaA solution at 25.0 °C? B) 1.20 C) 8.75 D) 5.25 E) 10.00 SHORT ANSWER. Write the word or phrase that best completes each statement or answers the question. 9) The equilibrium-constant expressed as 1/Keq is for a reaction written in the direction. MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 10) AS is...
e. -1135 Given the following reactions: CaCO3 (s)-> Cao (s) + CO2 (g) C (s, graphite) + O2 (g)-> Co2 (g) AH-393.5 kJ the enthalpy of the reaction CaCO3 (s) -> CaO (s) + C (s, graphite) + O2 (g) ΔH = 178.1 kJ is kJ Select one: 4 a. 7.01 x 10 b. 571.6 ) c. 215.4 d. -215.4 ie. -571.6 Check Given the data in the table below, AH for the reaction
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?
Calculate ΔH for the following reaction, CaO(s) + CO2(g) → CaCO3(s) given the thermochemical equations below. 2 Ca(s) + O2(g) → 2 CaO(s) ΔH = -1270.2 kJ C(s) + O2(g) → CO2(g) ΔH = -393.5 kJ 2 Ca(s) + 2 C(s) + 3 O2(g) → 2 CaCO3(s) ΔH = -2413.8 kJ A compound contains C, H and O as the elements. A 20.0 g-sample is comprised of 1.34 g H and also 8.00 g of C. What...