a. If 4.5 mol of ethane, C2H6, undergo combustion according to the unbalanced equation C2H6+O2---->CO2+H2O, how many moles of oxygen are required? b. How many moles of each product are formed?

Md Ariful Islam

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If 4.5 mol of ethane, C2H6, undergo combustionaccording to the unbalanced equation the amount of O2 is the samethat amount of ethane. C2H6 + O2 ----gt; CO2 + H2O, so it is 4.5 mol of O2 But when it is balanced equation the amount of O2 is next, C2H6 + 7/2 O2 ----gt; 2CO2 + 3H2O 4.5 mol* 7/2 = 15.72 mol
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If 2.39 mol of ethane undergoes combustion how many moles of O2 are required answer in units of mol

The reaction of ethane combustion: is as following:2C2H6 + 7O2 = 4CO2 + 6H2OSince the number of moles of ethane and oxygen must be equal, the number of moles of...

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Determine the number of moles of 02(g) that are required to react with 6.00 mol of C2H6 (g). 2C2H6(g)+7 O2(g)= CO2(g) +H2O (l) Please, show your complete solution. Thank you!

Mole ratio for C2H6 : O2 = 2:7Therefore 6 moles of C2H6 = 7 ×3 = 2121 moles of O2

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Calculate the number of moles of ethane (C2H3) needed to produce 10.0g of water. 2 C2H6 + 7 O2 => 4 CO2 + 6 H20

Moles of ethane =2 moles

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the standard enthalpy of combustion of ethane, carbon, and hydrogen are -1559.7 kJ/mol, -393kJ/mol and -286kJ/mol respectively. Use Hess'ss law to find the enthalpy of formation of ethane

ΔHform(C2H6)=ΔHcomb(C2H6)-(2ΔHcomb(C)+3ΔHcomb(H2))=-1559.7-(2(-393)+3(-286))=84,3 kJ/mol

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Define enthalpy of combustion. Calculate the enthalpy of combustion of methanol if the enthalpies of formation of CO2,H20 andCH3OH are respectively . -393.5kj/mol,-285.8kj/mol and -239.0kj/mol.

Answer: Enthalpy of combustion is the heat released during combustion of one mol amount of any substance by oxygen.You can calculate the combustion enthalpy of methanol using the enthalpy...

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Calculate the enthalpy of combustion of ethyne (C2H2) from the data below: ΔHf (CO2) = -393kJ/mol , ΔHf (H2O) = -286kJ/mol and ΔHf (C2H2) = -229kJ/mol *

Solution:The standard enthalpy of combustion is ΔH∘c. It is the heat evolved when 1 mol of a substance burns completely in oxygen at standard conditions.The balanced chemical equation of combustion of...

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The complete combustion of octane with oxygen, represented by the unbalanced chemical equation: C8H18 + O2 → CO2 + H2O 10 grams of octane and 10grams of oxygen will yield what mass of water?

Solution:The balanced chemical equation:2C8H18 + 25O2 → 16CO2 + 18H2O According to the chemical equation: n(C8H18)/2 = n(O2)/25 = n(H2O)/18Convert all given information into moles:Moles of octane = n(C8H18) = Mass...

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What is the enthalpy change if 105 g of ethane is burned in a combustion reaction whose molar enthalpy of combustion is -1251 kJ/mol. *

n = m / MM (C2H6) = 30.07 g/moln (C2H6) = 105 / 30.07 = 3.5 moldelta H (C2H6) = - 1251 x 3.5 = -4367 kJ

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Which molecule in the reaction below is the oxidizing agent? 2 C2H6(g) + 7 O2(g) → 4 CO2(g) + 6 H2O(g) A. O2 B. CO2 C. None D. C2H6 E. H2O

2C2-3H6+1 (g) + 7O20 -> 4C+4O2-2 + 6H2+1O-2O20 +4e--> 2O-2 ( oxidizing agent)C-3 -7e- -> C+4 (reducing agent)Answer: A.O2

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-Hexane (C6H14) is being used as a fuel. The Moles of Oxygen required for complete combustion of 1 Mole of the fuel is: Select one: a. 9.5 moles b. 10.25 moles c. 10 moles d. None of the above

C6H14+9.5O2=6CO2 +7H2OAnswer a - 9.5 mole

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