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How many oxygen atoms are in the products of the following reaction?
$C_6H_12O_6 + 6H_2O + 6O_2 -> 6CO_2 + 12 H_2O$
$C_6H_12O_6+6O_2rarr6CO_2 + 6H_2O$ Carbon and oxygen atoms have precise masses and charges. Since mass and charge are conserved in a chemical reaction, it follows that the reactants and the products...
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In the reaction $4NH_3+6NO->5N_2+6H_2O$, how many grams of ammonia will react with 27.8 grams of nitric oxide?
How many moles of nitric oxide reacted? $n_"NO"$ $=$ $(27.8*g)/(30.01*g*mol^-1)$ $=$ $0.927*mol$. Your stoichiometric equation CLEARLY shows that each equiv $NO$ requires $2/3" equiv"$ $"ammonia"$ for the comproportionation to occur....
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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?
$"Moles of dioxygen"$ $=$ $(45*g)/(32.00*g*mol^-1)=1.41*mol$. Clearly, there is insufficient dioxygen for complete combustion; i.e. complete combustion requires $1.75*mol$ $O_2$. We ASSUME incomplete combustion, i.e. $"COMPLETE COMBUSTION GIVES...."$ $C_2H_6(g) + 7/2O_2(g)...
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The equation, $6CO_2 + 6H_2O -> C_6H_12O_6 + 6O_2$, is what type of reaction?
Carbon dioxide on the left hand side, sugar and dioxygen on the right hand side. Is this magic? The name begins with a $"P"$. What do you call the reverse...
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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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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?
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...
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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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