Given:
Hof(C8H18(l)) = -259.3 KJ/mol
Hof(O2(g)) = 0.0 KJ/mol
Hof(CO2(g)) = -393.51 KJ/mol
Hof(H2O(l)) = -285.83 KJ/mol
Balanced chemical equation is:
2 C8H18(l) + 25 O2(g) ---> 16 CO2(g) + 18 H2O(l)
ΔHo rxn = 16*Hof(CO2(g)) + 18*Hof(H2O(l)) - 2*Hof( C8H18(l)) -
25*Hof(O2(g))
ΔHo rxn = 16*(-393.51) + 18*(-285.83) - 2*(-259.3) - 25*(0.0)
ΔHo rxn = -10922.5 KJ
Given:
Sof(C8H18(l)) = 328.0 J/mol.K
Sof(O2(g)) = 205.7 J/mol.K
Sof(CO2(g)) = 213.74 J/mol.K
Sof(H2O(l)) = 69.91 J/mol.K
Balanced chemical equation is:
2 C8H18(l) + 25 O2(g) ---> 16 CO2(g) + 18 H2O(l)
ΔSo rxn = 16*Sof(CO2(g)) + 18*Sof(H2O(l)) - 2*Sof( C8H18(l)) -
25*Sof(O2(g))
ΔSo rxn = 16*(213.74) + 18*(69.91) - 2*(328.0) - 25*(205.7)
ΔSo rxn = -1120.28 J/K
At equilibrium,
ΔGo = 0.0 KJ/mol
We have:
ΔHo = -10922.5 KJ/mol
ΔSo = -1120.28 J/mol.K
= -1.12028 KJ/mol.K
use:
ΔGo = ΔHo - T*ΔSo
0.0 = -10922.5 - T *(-1.1203)
T = 9749.79 K
Answer: 9749.79 K
For the following reaction: 2C3H18(1) + 2502(g) → 16C02(g) + 18H20(1) Compound AH°F (kJ moll) Sº...
For the following reaction: 2CH3OH(l) + 3O2(g) → 2CO2(g) + 4H2O(l) Compound ΔH°f (kJ mol-1) S° (J mol-1 K-1) CH3OH (l) -238.40 127.19 O2 (g) 0.00 205.70 CO2 (g) -393.51 213.74 H2O (l) -285.83 69.91 Determine the temperature (to two decimal places in K) such that the reaction is in equilibrium in its standard states.
For the following reaction: CS2(g) + 3O2(g) → CO2(g) + 2SO2(g) Compound ΔH°f (kJ mol-1) S° (J mol-1 K-1) CS2 (g) 116.70 237.80 O2 (g) 0.00 205.70 CO2 (g) -393.51 213.74 SO2 (g) -296.84 248.20 Calculate ΔG°rx (in kJ) at 794.8 K for this reaction. Report your answer to two decimal places in standard notation (i.e. 123.45 kJ). Assume ΔH°f and S° do not vary as a function of temperature.
How do i set up this problem? answer is provided but struggling with how to actually solve it. 11. Calculate AS and AGº for the following reaction: C3H3(g) +502(g) → 3C02(g) + 4H2O(1) Using: Alf" C3H8, gas) = -103.85 kJ/mol; AH,^[ O2, gas)= 0 kJ/mol; AH [ CO2, gas]=-393.51 kJ/mol; AH?°[ H20, liquid]=-285.83 kJ/mol Smº[ C3Hs, gas) = 270.2 J/(K-mol); Smº[ O2, gas)= 205.14 J/(K-mol); Smº[ CO2, gas)= 213.74 J/(K-mol); Smº[ H2O, liquid)= 69.91 J/(K-moll (Ans ASⓇ = -375.0J/K and...
12. Using the data: CH«(9), AH; = +51.9 kJ mor', sº = 219.8 J mor' k' CO2(g), AH = -394.0 kJ mor', sº = 213.6 J mor' k' H2O(), AH = -286.0 kJ mor', sº = 69.96 J mor'' O2(g), AH = 0.00 kJ mor', sº = 205 J mor'' calculate the maximum amount of useful work that can be obtained, at 25.0 °C, from the process: C2H4(9) + 3 O2(g) → 2 CO2(g) + 2 H2O(1) a. 1332 kJ...
), is determined to be -7835.7 kJ mol!! The standard enthalpy change of combustion [to CO2(g) and H200) at 25°C of the organic solid pyrene, CH What is the AH of C16H10(s) based on this value? Use the following data: AH? H20 () --285.83 kJ moll: AH? CO2(8) --393.51 kJ mol! kJ mol!
For the following reaction: 2CH4(g) + O2(g) → 2CO(g) + 4H2(g) Compound ΔH°f (kJ mol-1) S° (J mol-1 K-1) CH4 (g) -74.87 188.66 O2 (g) 0.00 205.70 CO (g) -110.53 197.66 H2 (g) 0.00 130.68 Calculate ΔG°rx (in kJ) at 345.31 K for this reaction. Report your answer to two decimal places in standard notation (i.e. 123.45 kJ). Assume ΔH°f and S° do not vary as a function of temperature.
For the following reaction: 2Na(s) + 2H2O(l) → 2NaOH(s) + H2(g) Compound ΔH°f (kJ mol-1) S° (J mol-1 K-1) Na (s) 0.00 51.30 H2O (l) -285.83 69.91 NaOH (s) -425.93 64.46 H2 (g) 0.00 130.68 Calculate ΔG°rx (in kJ) at 391.96 K for this reaction. Assume ΔH°f and S° do not vary as a function of temperature.
4) What is AH°rxn for the following reaction? 2C8H18(1) + 1702(g) → 16CO(g) + 18H20(1) Use the 2 reactions below: 2C8H18(1) + 2502(g) → 16CO2(g) + 18H20(1) 2CO(g) + O2(g) → 2C02(g) AH°rxn =-11020. kJ/mol AH°rxn =-566.0 kJ/mol A) -6492 kJ/mol B) +6492 kJ/mol C) -1964 kJ/mol D) -11020. kJ/mol E) -11586 kJ/mol
For the reaction CO2(g) + H2(9)—-CO(g) +H30(9) AH° = 41.2 kJ and A Sº = 42.1 JK The equilibrium constant for this reaction at 252.0 K is Assume that AH and AS are independent of temperature. For the reaction N2(g) + 3H2(g) 2NH3(g) AH° = -92.2 kJ and AS™ = -198.7 J/K The equilibrium constant for this reaction at 347.0 K is Assume that AHⓇ and AS are independent of temperature.
Question 1 2C8H18 + 2502 - 16CO2 + 18H20 AH rxn--11020 kJ/mol rxn Look at above equation. How many kl of heat will be released when 7.00 grams of C8H18 is combusted? 23.1 k) 840 kJ 8.82 x 103 o 2190 kJ 6.07 x 103 9440 kj 138 kJ 338 k) A Moving to the next question prevents changes to this answer.