Part A:
Determine ΔH∘f for NO(g)
Part B:
Determine ΔH∘f for BF3(g)
Part C:
Determine ΔH∘f for C6H6(l)
Part D:
Determine ΔH∘f for HF(g)
A)
Standard state of N is N2(g)
Standard state of O is O2(g)
So, the formation reaction is:
1/2 N2(g) + 1/2 O2(g) -> NO(g)
From table:
ΔHof(NO(g)) = 91.3 KJ/mol
Answer: 91.3 KJ/mol
B)
Standard state of B is B(s)
Standard state of F is F2(g)
So, the formation reaction is:
B(s) + 3/2 F2(g) -> BF3(g)
From table:
ΔHof(BF3(g)) = -1136.0 KJ/mol
Answer: -1136.0 KJ/mol
C)
Standard state of C is C(s,graphite)
Standard state of H is H2(g)
So, the formation reaction is:
6 C(s,graphite) + 3 H2(g) -> C6H6(l)
From table:
ΔHof(C6H6(l)) = 49.1 KJ/mol
Answer: 49.1 KJ/mol
D)
Standard state of H is H2(g)
Standard state of F is F2(g)
So, the formation reaction is:
1/2 H2(g) + 1/2 F2(g) -> HF(g)
From table:
ΔHof(HF(g)) = -273.3 KJ/mol
Answer: -273.3 KJ/mol
Part A: Determine ΔH∘f for NO(g) Part B: Determine ΔH∘f for BF3(g) Part C: Determine ΔH∘f...
Part A: Write an equation for the formation of NO(g) from its elements in their standard states. Express your answer as a chemical equation. Identify all of the phases in your answer. Part B: Write an equation for the formation of BF3(g) from its elements in their standard states. Express your answer as a chemical equation. Identify all of the phases in your answer. Part C: Write an equation for the formation of C6H6(l) from its elements in their standard...
Part B Find AH; for BF3 (g) from the given table. Substance AH kJ/mol 565.0 o 79.38 B(g) B(s) F(g) F2(g) BF3(8) BC1: (g) B,H6(8) B2O3(g) - 1136.0 -403.8 36.4 - 1273.5 Express your answer using one decimal place. IVO AQ – Oo ? AH; - kJ/mol Submit Request Answer
Use the ΔH°f values provided to determine ΔH°rxn for the following reaction CH4(g) + 3 Cl2(g) → CHCl3(l) + 3 HCl(g) ΔH°rxn = ? ΔH°f (kJ/mol): -75 -134 -92 A. +662 kJ B. +117 kJ C. -151 kJ D. -335 kJ The equation that corresponds to the enthalpy of formation for NH3(g) is A. N(g) + 3H(g) → NH3(g) B. N(g) + 3/2 H2(g) → NH3(g) C. 1/2 N2(g) + 3H(g) → NH3(g) D. 1/2 N2(g) + 3/2 H2(g) →...
Nitrogen Ahºf (kJ/mol) AG°f (kJ/mol) Sº (J/mol K) 191.6 N2(9) 0 0 N(g) 472.7 455.6 153.3 NH3(g) -46.1 -16.5 192.5 NH3(aq) -80.0 -27.0 111.0 NH4+ (aq) -132.0 -79.0 113.0 90.3 86.6 210.8 NO(9) NOCI(g) 51.7 66.1 261.8 NO2(g) 33.2 51.3 240.1 N20(9) 82.1 104.2 219.9 N204(9) 9.2 97.9 304.3 N204(0) -20.0 97.0 209.0 N205(s) -42.0 134.0 178.0 N2H4(0) 50.6 149.3 121.2 N2H3CH3 () 54.0 180.0 166.0 HNO3(aq) -207.4 -111.3 146.4 HNO3(1) -174.1 -80.7 155.6 HNO3(9) -135.1 -74.7 266.4 NH4ClO4(s) -295.0...
Thermodynamic Data at 25 C Substance CH4 (B) (kJmol AHof 74.6 -110.5 AGof 50.5 -137.2 S (Jmol 'K) 186.3 CO (B Cl2 (g) Cu (s) 197.7 223.1 33.2 42.6 Cuo (s) 157.3 -129.7 202.8 -92.3 -273.3 285.8 241.8 -173.23 -20.6 -95.3 -275.4 -237.1 -228.6 -79.9 33.4 186.9 173.8 70.0 188.8 155.6 205.8 HF H20 (9) HNO3 (1) 91.3 33.2 81.6 45.9 87.6 51.3 103.7 -16.4 191.6 210.8 240.1 220.0 192.8 NO2 (8) NH3 02 205.2 42.6 140.9 AgNO3 (s) 124.4...
Given the values of ΔH∘rxn, ΔS∘rxn, and T, determine ΔSuniv. Part A ΔH∘rxn=+84 kJ , ΔSrxn=+141 J/K , T= 308 K Express your answer as an integer. Part B ΔH∘rxn=+84 kJ , ΔSrxn=+141 J/K , T= 754 K Express your answer as an integer. Part C ΔH∘rxn=+84 kJ , ΔSrxn=− 141 J/K , T= 308 K Express your answer as an integer. Part D ΔH∘rxn=− 84 kJ , ΔSrxn=+ 141 J/K , T= 403 K Express your answer as an...
Part A Use the following additional data at 25 ∘C to calculate the standard molar entropy S∘ of O2 at 25 ∘C: ΔH∘f(KClO3)= −397.7kJ/mol , ΔH∘f(KCl)=−436.5kJ/mol , S∘(KClO3)=143.1J/(K⋅mol) , and S∘(KCl)=82.6J/(K⋅mol).
Part B Part complete ΔH∘rxn=+ 83 kJ , ΔSrxn=+ 146 J/K , T= 759 K Express your answer as an integer. -- SubmitPrevious AnswersRequest Answer Part C Part complete ΔH∘rxn=+ 83 kJ , ΔSrxn=− 146 J/K , T= 309 K Express your answer as an integer. -- ΔG Δ G = nothing kJ SubmitPrevious AnswersRequest Answer Part D Part complete ΔH∘rxn=− 83 kJ , ΔSrxn=+ 146 J/K , T= 407 K Express your answer as an integer. -- ΔG Δ...
Part A) What is ΔH∘rxn for the following chemical reaction? CO2(g)+2KOH(s)→H2O(g)+K2CO3(s) You can use the following table of standard heats of formation (ΔH∘f) to calculate the enthalpy of the given reaction. Element/ Compound Standard Heat of Formation (kJ/mol) Element/ Compound Standard Heat of Formation (kJ/mol) H(g) 218 N(g) 473 H2(g) 0 O2(g) 0 KOH(s) −424.7 O(g) 249 CO2(g) −393.5 K2CO3(s) −1150kJ C(g) 71 H2O(g) −241.8kJ C(s) 0 HNO3(aq) −206.6 Express the standard enthalpy of reaction to three significant figures and...
b and e only C2HsOHD+301(g)->2 CO-(3)+3 H0O) Using ΔΗ0's data given below, determine the ΔΗ (a) (3 marks) (b) Determine the D(O-O) in 02(g). (3 marks) (c) Determine the AS° and comment on its value. (2 marks) (d) Determine the AGo and comment on its value. (3 marks) Comment this (4 marks) A 25 °C, the liquid ethanol reacts very slowly with O2(g). observation and explain the inconsistence (if any) with your answer in part (d). (e) D (in kJ...