Calculate the standard enthalpy change for the reaction
2C8H18(I) + 17O2(g) → 16CO(g)+ 18H2O(1)
Given: 2C8H18(I) + 25O2(g) → 16CO2(g)+18H2O(I) ΔH° = -11,020 kJ/mol
2CO(g) + O 2(g) → 2CO2(g) ΔH° = -566.0 kJ/mol
-10.450 kJ/mol
-6,492 kJ/mol
6,492 kJ/mol
10,450 kJ/mol
15,550 kJ/mol
Lets number the reaction as 0, 1, 2 from top to bottom
required reaction should be written in terms of other reaction
This is Hess Law
required reaction can be written as:
reaction 0 = +1 * (reaction 1) -8 * (reaction 2)
So, ΔHo rxn for required reaction will be:
ΔHo rxn = +1 * ΔHo rxn(reaction 1) -8 * ΔHo rxn(reaction 2)
= +1 * (-11020.0) -8 * (-566.0)
= -6492 KJ/mol
Answer: -6492 KJ/mol
Lets number the reaction as 0, 1, 2 from top to bottom
required reaction should be written in terms of other reaction
This is Hess Law
required reaction can be written as:
reaction 0 = +1 * (reaction 1) -8 * (reaction 2)
So, ΔHo rxn for required reaction will be:
ΔHo rxn = +1 * ΔHo rxn(reaction 1) -8 * ΔHo rxn(reaction 2)
= +1 * (-11020.0) -8 * (-566.0)
= -6492 KJ
Answer: -6492 KJ
Calculate the standard enthalpy change for the reaction 2C8H18(I) + 17O2(g) → 16CO(g)+ 18H2O(1)
Calculate the standard enthalpy change for the reaction 2C8H18(l) + 17O2(g) →16CO(g) + 18H2O(l). Given 2C8H18(I) + 25O2(g) →16CO2(g) + 18H2O(I) ΔH°=-11,020 kJ/mol 2CO(g) + O2(g) → 2CO2(g) ΔH° = -566.0 kJ/mol 0 -6,492 kJ/mol 15,550 kJ/mol 10,450 kJ/mol -10.450 kJ/mol 6,492 kJ/mol
The combustion of octane, C8H18,C8H18, proceeds according to the reaction shown. 2C8H18(l)+25O2(g)⟶16CO2(g)+18H2O(l)2C8H18(l)+25O2(g)⟶16CO2(g)+18H2O(l) If 522 mol522 mol of octane combusts, what volume of carbon dioxide is produced at 38.0 ∘C38.0 ∘C and 0.995 atm?
The combustion of octane, C8H18,C8H18, proceeds according to the reaction shown. 2C8H18(l)+25O2(g)⟶16CO2(g)+18H2O(l)2C8H18(l)+25O2(g)⟶16CO2(g)+18H2O(l) If 4.10×102 mol4.10×102 mol of octane combusts, what volume of carbon dioxide is produced at 12.0 ∘C12.0 ∘C and 0.995 atm?
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
Let’s combust octane. (2C8H18 + 25O2 --> 16CO2 + 18H2O) delta G C8H18= 16.4 kj/mol, delta G CO2 = -394 kj/mol, delta G H2O = -229 kj/mol a. Please calculate the free energy of rxn for the burning of octane. b. Now give the lnKeq at STP. c. Next, give the lnKeq at 200C d. Follow with the free energy of reaction at this temperature
balanced chemical equation: 2C8H18(g)+25O2->16CO2(g)+18H2O(g) 0.320 mol of octane is allowed to react with 0.880 mol of oxygen. After the reaction how much Octane is left?
Balanced chemical equation: 2C8H18(g)+25O2(g)->16CO2(g)+18H2O(g) 0.320 mol of octane is allowed to react with 0.880 mol of oxygen. How many moles of water are produced in this reaction?
The combustion of octane, C8H18, proceeds according to the reaction shown. 2C8H18(l)+25O2(g)⟶16CO2(g)+18H2O(l) Calculate the volume of carbon dioxide produced when 562 moles of octane combusts at 28.0 °C and 1.00 bar.
The combustion of octane, C8H18, proceeds according to the reaction shown. 2C8H18(l)+25O2(g)⟶16CO2(g)+18H2O(l) If 442 mol of octane combusts, what volume of carbon dioxide is produced at 19.0 ∘C and 0.995 atm? ?=
The combustion of octane, C8H18, proceeds according to the reaction shown. 2C8H18(l)+25O2(g)⟶16CO2(g)+18H2O(l) If 498 mol of octane combusts, what volume of carbon dioxide is produced at 14.0 ∘C and 0.995 atm?