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How would you determine the number of moles of $N_2$ that are required to produce 12 mol of $NH_3$ using the equation: $N_2+ 3H_2 -> 2NH_3$?
There is no coefficient in front of the $N_2$ in the reactants. This means that there is one mole of $N_2$ required in the balanced equation. There is a...
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Given the equation:$N_2+3H_2 rarr 2NH_3$, what volume of $NH_3$ at STP is produced if 25 grams of $N_2$ is reacted with an excess of $H_2$?
One thing I think it's interesting to note is that you'll never be able to have that reaction happen in the standard temperature and pressure; you can, however, have the...
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How many grams of $N_2$ are required to completely react with 3.03 grams of $H_2$ for the equation $N_2 + 3H_2 -> 2NH_3$?
Notice the coefficients of $N_2$ and $H_2$. Since the equation has an $N_2$ and $3H_2$, $3$ times as many moles of $H_2$ will be used as $N_2$ assuming a complete...
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Consider the reaction $N_2(g) + 3H_2(g) rightleftharpoons 2NH_3(g)$. What is the effect of decreasing the volume on the combined gas?
In this scenario, $"Le Chatelier's principle"$ would predict that the equilibrium would be driven to the side of the reaction that exerts least pressure, i.e. the product side. Note that...
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In the reaction $N_2(g) + 3H_2(g) -> 2NH_3(g)$, $N_2 = 10.00 M$, $H_2 = 8.00 M$, and $NH_3 = 2.00 M$. What is the equilibrium constant $K$, for this reaction?
Before doing any calculation, take a look at the values of the equilibrium concentrations for the three chemical species that take part in the reaction. Notice that the concentrations of...
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What is $K_(eq)$ for the reaction $N_2+3H_2 -> 2NH_3$ if the equilibrium concentrations are $[NH_3] = 3.0 M, [N_2] = 2.0M$, and $[H_2] = 1.0M$?
As you know, the equilibrium constant for a given chemical equilibrium depends on the equilibrium concentrations of the chemical species that take part in the reaction the stoichiometric...
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What is $K_(eq)$ for the reaction $N_2 + 3H_2 rightleftharpoons 2NH_3$ if the equilibrium concentrations are $[NH_3] = 3 M$, $[N_2] = 2 M$, and $[H_2] = 1 M$?
Use the definition of $K_(eq)$. $K_(eq) = (["products"]^(d,e,f, . . . ))/(["reactants"]^(a,b,c,. . . ))$ $= (["NH"_3]_(eq)^2)/(["H"_2]_(eq)^3["N"_2]_(eq))$ Just make sure you remember to use stoichiometric coefficients correctly. $3H_2$...
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Given the equation representing a system at equilibrium: $N_2(g) + 3H_2(g) rightleftharpoons 2NH_3(g) + "energy"$, what changes occur when the temperature of this system is decreased?
$"Le Chatelier's principle states that when a system at....."$ $"equilibrium is subject to an external stress, the equilibrium"$ $"will move so as to oppose the external stress"$. As I...
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How do you determine the amount of heat (in kJ) given off when $1.26 xx 10^4$ g of ammonia are produced according to the equation $N_2(g) + 3H_2(g) -> 2NH_3(g)$, $DeltaH°_(rxn)$ = -92.6 kJ/mol?
The problem provides you with the thermochemical equation that describes the synthesis of ammonia from nitrogen gas and hydrogen gas. $"N"_ (2(g)) + 3"H"_ (2(g)) -> 2"NH"_ (3(g))" "DeltaH_...
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If given: $Sn(s) + Cl_2(g) -> SnCl_2(s)$, $DeltaH = -325 kJ$ and $SnCl_2(s) + Cl_2(g) -> SnCl_4(l)$, $DeltaH = -186 kJ$, what is $DeltaH$ for this reaction? $Sn(s) + 2Cl_2(g) -> SnCl_4(l)$
First of all, write out the equations $Sn(s) + Cl_"2"(g) -> SnCl_"2"(s)$ $DeltaH = -325kJ$ $SnCl_"2"(s) + Cl_"2"(g) -> SnCl_"4"(l)$ $DeltaH = -186kJ$...
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