What are the coefficients for the following reaction when it is properly balanced? _02+CH4 →_CO2+ _H20 - -- --- О 1,3, 2, 1 O 2, 1, 3, 1 none of the above O 2, 1, 1, 2 О 2,3, 2, 2
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A: The Balanced Chemical Equation can be written as -
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- Which of the following reactions result in a positive ∆ Ssys? a. H2O(g) = H2O(l) b. H2(g) + I2(g) = 2 Hl(g) c. C2H2O2(g) = 2CO(g) + H2(g) d. H2O(g) + CO2 (g) = H2CO3(aq)SCE // PO43- (aq) , Ag3PO4 (saturated) / Ag h a s a n I n d i c a t o r e l e c t r o d e t h a t i s a c h o o s e : l i q u i d m e m b r an e e l e ct r o d e m et a l l i c e l e c tr o d e of t he s e co n d k in d g l a ss el e c t ro d e m e t a l li c el e c t ro d e of t h e f i r st k i n dWhich one of the following reactions will have a positive ∆S?A. CO2 (g) → CO2 (s)B. 2 Hg (l) + O2 (g) → 2 HgO (s)C. 2 NO2 (g) → N2O4 (g)D. BaF2 (s) → Ba2+ (aq) + 2 F-(aq)E .2 H2 (g) + O2 (g) → 2 H2O (g)
- 1. Given the SEPs: Br2(l) + 2e- ↔ 2Br- E0 = 1.078 V Br2(aq) + 2e- ↔ 2Br- E0 = 1.098 V a. Calculate the Keq for the reaction: Br2(l) ↔ Br2(aq)Calculate Eo for the following equation. Cr(s) + NO3-1(aq) →Cr+3(aq) + NO(g) Group of answer choices +0.213 V +0.844 V +1.701 V -1.701 V -0.644 V -0.844 V -0.213 V +0.644 VAt constant pressure and 25 C, what is the Delta rH for the following reaction: 2C2H6 (g) + 7O2(g) --> 4CO2(g) + H2O(l) if the complete consumption of 12.5g of C2H6 liberates 752.3 kJ of heat energy?
- 17 Calculate the ΔH°rxn for the following reaction. SiO2(s) + 4HCl(g) → SiCl4(g) + 2H2O(g) ΔH°f [SiO2(s)] = –910.9 kJ/mol; ΔH°f [SiCl4(g)] = –657.0 kJ/mol; ΔH°f [HCl(g)] = –92.3 kJ/mol; ΔH°f [H2O(g)] = –241.8 kJ/mol Group of answer choices –139.5 kJ –137.4 kJ –104.4 kJ 104.4 kJ 139.5 kJFrom the attached solution where did you get this? = S CO2 (g) + S H2O (l) - [ S C6H12O6 (s) + S O2(g)] = (213.7 J/mol-K + 69.9 J/mol-K) - (212.0 J/mol-K + 205.1 J/mol-K)I just was wondering why its not 2e- for the second reaction and just e-
- The equilibrium constant for the reaction2 NO1g2 + Br21g2 ∆ 2 NOBr1g2is Kc = 1.3 * 10-2 at 1000 K. (a) At this temperature doesthe equilibrium favor NO and Br2, or does it favor NOBr?(b) Calculate Kc for 2 NOBr1g2 ∆ 2 NO1g2 + Br21g2.(c) Calculate Kc for NOBr1g2 ∆ NO1g2 + 12 Br21g2.Which of the following reactions will have the most negative value for ΔrG°? Select one: 2Hg(g) + O2(g) ⇌ 2HgO(s) K=1.9×1010 CO(g) + Cl2(g) ⇌ COCl2(g) K=248 Cl(g) + O3(g) ⇌ ClO(g) + O2(g) K=1.1×106 2H2O(l) ⇌ 2H2(g) + O2(g) K=7.0×10-84 2HNO3(aq) + NO(g) ⇌ 3NO2(g) + H2O(l) K=1.2×10-9At 2452 oC, Keq = 97.7 for the reaction: 1/3 NO2(g) + 1/3 N2O(g) (equlibrium arrows) NO(g) (a) What is the value of Keq for the reaction NO(g) 1/3 NO2(g) + 1/3 N2O(g)?Keq = .(b) What is the value of Keq for the reaction NO2(g) + N2O(g) 3 NO(g)?Keq = .(c) What is the value of Keq for the reaction 3 NO(g) NO2(g) + N2O(g)?Keq = .