At constant pressure for which of the reactions shown below should ΔH° be greater than ΔE° ?
I. 2 SO2(g) + O2(g) → 2
SO3(g)
II. C23H48(g) + 35
O2(g) → 23 CO2(g) + 24
H2O(l)
III. H2(g) + Cl2(g) → 2
HCl(g)
IV. N2O4(g) → 2
NO2(g)
At constant pressure for which of the reactions shown below should ΔH° be greater than ΔE°...
The enthalpy change, ΔH, for a reaction at constant pressure is defined as: ΔH = ΔE + PΔV. For which of the following reactions will ΔH be approximately equal to ΔE? Select all that apply. Group of answer choices 2 NO2(g) -> N2(g) + 2 O2(g) Ca(OH)2(aq) + H2SO4(aq) -> 2 H2O(l) + CaSO4(s) C(s) + O2(g) -> CO2(g) None of the above
Use data given below to calculate ΔrS∘ΔrS∘ for each of the reactions. Standard Thermodynamic Quantities for Selected Substances at 25 ∘C∘C Substance ΔrS∘ΔrS∘, JK−1mol−1JK−1mol−1 Cr(s)Cr(s) 23.8 Cr2O3Cr2O3(s)(s) 81.2 CO(g)CO(g) 197.7 CO2(g)CO2(g) 213.8 H2(g)H2(g) 130.7 H2O(g)H2O(g) 188.8 H2O(l)H2O(l) 70.0 HNO3(aq)HNO3(aq) 146.0 N2(g)N2(g) 191.6 N2O4(g)N2O4(g) 304.4 NO(g)NO(g) 210.8 NO2(g)NO2(g) 240.1 O2(g)O2(g) 205.2 SO2(g)SO2(g) 248.2 SO3(g)SO3(g) 256.8 A) 4NO2(g)+2H2O(l)+O2(g)→4HNO3(aq) B) Cr2O3Cr2O3(s)(s) +3CO(g)→2Cr(s)+3CO2(g) C) SO2(g)SO2(g) +12O2(g)→SO3(g) D) N2O4(g)+4H2(g)→N2(g)+4H2O(g)
More Equilibrium: Please write equilibrium expressions for the following reactions: 1. i. 2 SO2 (g) + O2 (g) 2 SO3 (g) il. NH4NOs (s) N2O (g) +2 H20 (g) i CaCO3 (s) + CaO (s) + CO2 (g) iv. HNO2 (aq) +H2O (I) HaO* (aq) + NO2 (aq) 2. Predict which way the equilibrium will shift for each of the following changes: CO (g) + H2 (g) C (s) H2O (g) + heat i. increase [H2O] ii. increase [C0] iii....
Calculate ΔH° for each of the following reactions, which occur in the atmosphere.(a) C2H4(g) + O3(g) → CH3CHO(g) + O2(g)(b) O3(g) + NO(g) → NO2(g) +O2(g)(c) SO3(g) + H2O(l) → H2SO4(aq)(d) 2 NO(g) + O2(g) → 2 NO2(g)
Which of the following reactions is an oxidation-reduction reaction? A) NH4HS(s) → NH3(g) + H2S(g) B) 2 NaHCO3(s) → Na2CO3(s) + H2O(g) + CO2(g) C) N2O4(g) → 2 NO2(g) D) 2 SO2(g) + O2(g) → 2 SO3(g) E) 2 HC2H3O2(aq) + Ba(OH)2(aq) → Ba(C2H3O2)2(aq) + 2 H2O(l)
Which of the following reactions would ΔH = ΔE? 2Al(s) + 6HCl(aq) --> 2AlCl3(aq) + 3H2(g) CaCO3(s) --> CaO(s) + CO2(g) C(s) + O2(g) --> CO2(g) C3H4(g) + 4O2(g) --> 3CO2(g) + 2H2O(l) Zn+2(aq) + 2OH-(aq) --> Zn(OH)2(s)
Calculate the volume change (in Liters) during the combustion of propane in which ΔE = -3083.67 kJ and ΔH = -3087.12 kJ at a constant pressure of exactly one atm and constant temperature. C3H8(g) + 5 O2(g) ↔ 3 CO2(g) + 4 H2O(l) The product of pressure and volume change should give units of L*atm. It can be shown that 1 L*atm = 101 J.
Use the enthalpies for the given reactions to compute the standard enthalpy change (ΔH°) for the reaction: 6 C (s) + 7 H2(g) → C6H14 (l) ΔHrxn = ? C6H14 (l)+19/2O2 (g)→6CO2(g)+ 7H2O(g). ΔH=–3505.8kJ C(s) + O2 (g) → CO2(g) ΔH=–393.5kJ H2(g) + 1/2 O2(g) → H2O(g). ΔH = – 242.0 kJ
For which of these reactions will the difference betweenΔH° and ΔE° be the greatest? a. 2H2O2(l) →2H2O(l) + O2(g) b. CaCO3(s)→ CaO(s) +CO2(g) c. NO(g) +O3(g) → NO2(g) + O2(g) d. 2C2H6(g) +7O2(g) → 4CO2(g) + 6H2O(l) e. 4NH3(g)+ 5O2(g) → 4NO(g) + 6H2O(g)
Consider each of the following systems at constant pressure. Mark each system where work is done by the surroundings on the system. (Select all that apply.) 1. CaCO3(s) → CaO(s) + CO2(g) 2. CO2(s) → CO2(g) 3. 2 SO2(g) + O2(g) → 2 SO3(g) 4. H2O(g) → H2O(l) 5. C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(g)