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27 Jun 2018

Q10. The given reaction has a AG x = 9.4 kJ at 25°C. Find AGxn when Roy = 0.115 atm and Pro 9.7 atm at 25°C. 3 NO2(g) + H2O(l) — 2 HNO3(1) + NO(g) a) -12.3 kJ c) 31.1 kJ b) 21.7 x 103 kJ d) 18.8 kJ

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28 Jun 2018
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Related questions

1. Calculate the standard entropy change for the reaction:

2NO2(g)+ H2O(g) --> HNO2(g) +HNO3(g)

Use thefollowing data: S°(NO2(g)) = 240.0 J mol-1K-1;S°(H2O(g)) = 118.7 J mol-1K-1; S°(HNO2(g)) =59.59 J mol-1K-1; S°(HNO3(g)) = 266.2 Jmol-1K-1.

A. -272.9 J/K

B. 272.9 J/K

C. 32.9 J/K

D. -32.9 J/K

E. 136.5 J/K

2. Calculate the standard free energy change, and determine whether ornot the following reaction is spontaneous under standardconditions:

H2O2(l)--> H2O(l) + ½O2(g)

Use thefollowing values for ΔGf°: H2O2(l)= -120.4 kJ/mol; H2O(l) = -237.2 kJ/mol.

A. -457.6 kJ; spontaneous

B. 475.6 kJ; not spontaneous

C. -116.8 kJ; spontaneous

D. 116.8 kJ; not spontaneous

E. -287.2 kJ; spontaneous

3. Youhave probably heard the two sayings, "Nothing lasts forever" and"Diamonds are forever". They can't both be right, which one iscorrect?! Calculate the standard free energychange at 298K for the conversion of diamonds to graphite anddetermine whether or not the reaction is spontaneous under standardconditions:

C(diamond)--> C(graphite);

ΔHf°(diamond)= 1.895 kJ/mol; S°(diamond) = 2.337 J mol- 1K-1; S°(graphite) =5.740 J mol-1K-1.

A. 2.19 kJ; not spontaneous

B. -1.90 kJ; spontaneous

C. -2.90 kJ; spontaneous

D. 1.90 kJ; not spontaneous

E. 4.04 kJ; not spontaneous

PLEASE SHOWHOW YOU GET THE ANSWER---THANKS!

4a. If 34.00 mL of 0.250 M methylamine, (Kb = 5.0 x 10-M at 25°C) is titrated with 0.500 M HCIO4, what is the pH of the equivalence point? [6 marks] 4b. For the reaction below, AH° = -275.4 kJ and AS™ = -263.45 J/K at 25°C. [4 marks] a) Calculate AG for the reaction at 25°C and when Pso = 1 x 10 atm and P = 0.10 atm. b) Is this reaction spontaneous under these conditions? Show all necessary reasoning to support your answer. SO2(g) + H2O(l) + 102(g) → H2SO4(1)

Below what temperature does the following reaction become nonspontaneous? 2 HNO3(aq) + NO(g) → 3 NO2(g) + H2O(l); ΔH = +136.5 kJ; ΔS = +287.5 J/K

(A) 39.2 K (B) 151 K (C) 475 K (D) This reaction is nonspontaneous at all temperatures. (E) This reaction is spontaneous at all temperature

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