Consider the following unbalanced equation for the combustion of hexane: αc6h14(g)+βo2(g)→γco2(g)+δh2o(g) part a balance the equation. give your answer as an ordered set of numbers α, β, γ, use the least possible integers for the coefficients. α α , β, γ, δ = nothing request answer part b determine how many moles of o2 are required to react completely with 5.6 moles c6h14. express your answer using two significant figures. n n = nothing mol request answer provide feedback
2C₆H₁₄ + 19O₂ → 12CO₂ + 14H₂O
β = 19
γ = 12
δ = 14
53.2moles of O₂
Proper equation of the reaction:
αC₆H₁₄ + βO₂ → γCO₂ + δH₂O
This is a combustion reaction for a hydrocarbon. For the combustion of a hydrocarbon, the combustion equation is given below:
CₓHₙ + (x + )O₂ → xCO₂ + H₂O
From the given combustion equation, x = 6 and n = 14
β = x + = 6 + = 6 + 3.5 = 9
γ = 6
δ = = = 7
The complete reaction equation is therefore given as:
C₆H₁₄ + 9O₂ → 6CO₂ + 7H₂O
To express as whole number integers, we multiply the coefficients through by 2:
2C₆H₁₄ + 19O₂ → 12CO₂ + 14H₂O
From the reaction:
2 moles of hexane are required to completely react with 19 moles of O₂
∴ 5.6 moles of hexane would react with k moles of O₂
This gives: 5.6 x 19 = 2k
k = 53.2moles of O₂
(6.8mol C6H14)(19mol O2/2mol C6H14)= 64.6mol O2
62 moles of
Combustion is a type of chemical reaction in which a substance is reacted with oxygen to form carbon dioxide and water.
The balanced chemical reaction for combustion of
From the stoichiometry:
2 moles of hexane react with = 19 moles of oxygen
Thus 6.5 moles of hexane react with = moles of oxygen
Thus 62 moles of are required to react completely with 6.5 moles of .
32.5 moles of oxygen are required.
Number of moles of C₄H₁₀ = 5.00 mol
Number of moles of oxygen required = ?
2C₄H₁₀ + 13O₂ → 8CO₂ + 10H₂O
Now we will compare the moles of oxygen with C₄H₁₀ through balanced chemical equation.
C₄H₁₀ : O₂
2 : 13
5.00 : 13/2×5 = 32.5
So when 5 moles of C₄H₁₀ are present 32.5 moles of oxygen are required to react completely.
Part A : The value of are 2, 19, 12 and 14 respectively.
Part B : of are required to react with 6.4 moles of .
Part A :
The given unbalanced equation is,
The balanced equation is,
Part B :
From the balanced equation, we conclude that
2 moles of react with 19 moles of
6.4 moles of react with of
Therefore, of are required to react with 6.4 moles of .
The balanced equation is
2 C6H14 (g) + 19 O2 (g) --> 12 CO2 (g) + 14 H2O (g)Explanation:
For solving the stoichiometric calculations, we first need to do two steps. One of them is balancing the reaction equation. Here the balancing is done and we can see that 2 moles of hexane reacts with 19 moles of oxygen to produce 12 moles of carbon dioxide and 14 moles of water.
Now, for 2 moles of hexane, number of moles of oxygen required is 19.
So, for 7.2 moles of hexane, number of moles of oxygen required is.
So 68.4 moles of oxygen is required.
The balanced equation is C6H14(g) + 19/2O2(g) → 6CO2(g) + 7H2O(g). If you are given 7.9 moles C6H14, multiply it by a ratio of 19/2/1 to get the moles of oxygen. Then, you will get 75.05 moles of O2.
if multiplied with 2: 2C₆H₁₄(g) + 19O₂(g) → 12CO₂(g) + 14H₂O(g).
n(C₆H₁₄) = 6,4 mol.
From chemical reaction: n(C₆H₁₄) : n(O₂) = 2 : 19.
n(O₂) = 6,4 mol · 19 ÷ 2.
n(O₂) = 60,80 mol.
n - amount of substance.