Given the incomplete equation for the combustion of ethane, $2C_2H_6 + 7O_2 -> 4CO_2 + 6__$, what is the formula of the missing product?

Md Ariful Islam

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Md Ariful Islam

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In general any organic compound, when burned will generate an "oxide" of its atoms.

Carbon goes to $CO$ or $CO_2$ (the latter, if complete)
Hydrogen goes to $H_2O$
Nitrogen and Sulfur depend on the amount of $O_2$ available. If the amount is big enough they'll go for higher oxidation states such as $NO_2$, $SO_3$ but with less oxygen they'll settle for lower states like $NO$ and $SO_2$

Another way to solve this is to count the atoms that aren't in the right side. If you do the math you'll see we're missing 12 Hydrogen atoms and 6 Oxygen atoms, dividing by the stoichiometric coefficient that was given, we have 2 Hydrogen atoms and 1 Oxygen atom together to make a compound, which is obviously water.

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Can you write and balance the equation for the complete combustion of ethane, $C_2H_6$?

In a combustion reaction with a hydrocarbon in the reactant side you will always have $O_2$ as another reactant. As you will always have $CO_2$ and $H_2O$ as the products....

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The following reaction is an example what type of reaction? $2C_2H_6(g) + 7O_2(g) + 4CO_2(g) + 6H_2O(g)$

$C_2H_6 + 7/2O_2(g) rarr 2CO_2 +3H_2O(l)+Delta$ The carbon of ethane $(C,-III)$, undergoes formal 7 electron oxidation to give fully oxidized $CO_2$. What is reduced in the reaction? How does...

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In the equation $2C_2H_6 + 7O_2 -> 4CO_2 + 6H_2O$, if 15 g of $C_2H_6$ react with 45 g of $O_2$, how many grams of water will be produced?

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How do you calculate the energy required to produce 7.00 mol $Cl_2O_7$ on the basis of the following balanced equation: $2Cl_2(g) + 7O_2(g) + 130 kcal -> 2Cl_2O_7(g)$?

You gots... $2Cl_2(g) + 7O_2(g) + 130*kcal rarr 2Cl_2O_7(g)$ Another way of writing this is as... $2Cl_2(g) + 7O_2(g) rarr 2Cl_2O_7(g)$ $DeltaH_"rxn"^@=+130*kcal*mol^-1$ And when we write $mol^-1$ we mean per...

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In the equation $2C_2H_2(5) + 5O_2(5) -> 4CO_2(g) + 2H_2O(g)$, how many grams of oxygen gas are needed for the complete combustion of $1.8 * 10^2$ $g$ of acetylene?

Molecular mass of acetylene: $2 * MM_C + 2 * MM_H$ $MM_C$ = Molecular mass of carbon $MM_H$ = Molecular mass of hydrogen So, $2 * 12 + 2 *...

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For the balanced equation $2C_2H_5OH + 6O_2 -> 4CO_2 + 6H_2O$, how many moles of $O_2$ will react with 0.3020 moles of $CO_2$?

$O_2$ is a reagent and $CO_2$ is a product, therefore they won't react with each other.

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Using the following equation, $2C_2H_6 + 7O_2 -> 4CO_2 + 6H_2O$, if 2.5 g $C_2H_6$ react with 170 g $O_2$, what is the limiting reactant?

You have the stoichiometric equation, which tells you, unequivocally, that 2 equiv ethane reacts with 7 equiv dioxygen gas (alternatively 1 equiv ethane reacts with 3.5 equiv $O_2$). $"Moles...

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$2C_2H_2(l) + 5O_2(g) -> 4CO_2(g) + 2H_2O(g)$ If the acetylene tank contains 37.0 mol of $C_2H_2$ and the oxygen tank contains 81.0 mol of $O_2$, what is the limiting reactant for this reaction?

We might repropose the combustion reaction as... $HC-=CH(g) + 5/2O_2(g) rarr 2CO_2(g) + H_2O(l) + Delta_1$ …(I use the half-integral coefficients, because I find the arithmetic EASIER this way). And...

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When ethane, $C_2H_6$, reacts with chlorine gas the main product is $C_2H_5Cl$ but small amounts of $C_2H_4Cl_2$ are produced. What is the percent yield of $C_2H_5Cl$ if the reaction of 125g of ethane with 255g of chlorine gas produced 206g of $C2H_5Cl$?

The key here is to focus solely on the reaction that produces chloroethane, $"C"_2"H"_5"Cl"$, and ignore the one that produces dichloroethane, $"C"_2"H"_4"Cl"$, the side product of the reaction. Start by...

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