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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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Using the equation $N_2 + 3H_2 -> 2NH_3$, how many grams of hydrogen must react if the reaction needs 127 grams of $NH_3$?
$"3H"_2::"2NH"_3$ $3/2"H"_2::"1NH"_3$ $"Moles of NH"_3=127/17.0$ So $"moles of H"_2=3/2*127/17.0 = 11.2$ Mass of $"H"_2 = "11.2 mol" × "2.016 g/mol" = "22.6 g"$
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In the equation $N_2(g) + 3H_2(g) -> 2NH_3(g)$, 8.5 grams of hydrogen and 15.8 grams of nitrogen react to form ammonia. How many grams of ammonia are produced?
Moles of $N_2$ reactant $=$ $(15.8*g)/(28.02*g*mol^-1)$ $=$ $0.564$ $mol$. Moles of $H_2$ reactant $=$ $(8.5*g)/(2.02*g*mol^-1)$ $=$ $4.21$ $mol$. Dihydrogen is the reagent in excess (clearly!). Given that dinitrogen is the...
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You began with 22 grams of nitrogen, and produced 19 grams of ammonia, $NH_3$, According to the the mass calculations, you should be able to produce 26 grams of ammonia. What is the percent yield? $N_2 + 3H_2 ->2NH_3$
The is 73 %. The formula for percent yield is $color(blue)(bar(ul(|color(white)(a/a) "Percent yield" = "actual yield"/"theoretical yield" × 100 %color(white)(a/a)|)))" "$ ∴ $"Percent yield" = (19 color(red)(cancel(color(black)("g"))))/(26 color(red)(cancel(color(black)("g")))) ×...
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Given the equation: $N_2 + 3H_2 -> 2NH_3$ What volume of hydrogen is necessary to react with five liters of nitrogen to produce ammonia? (Assume constant temperature and pressure)
The important thing to remember about reactions that involve gases kept under the same conditions for pressure and temperature is that the that exist between the gases are equivalent to...
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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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At a certain temperature, 4.0 mol $NH_3$ is introduced into a 2.0 L container, and the $NH_3$ partially dissociates to $2NH_3(g)\rightleftharpoonsN_2(g)+3H_2(g)$.
At equilibrium, 2.0 mol $NH_3$ remains. What is the value of $K_c$?
Remember to include the coefficients in the change in concentratio, as well as the exponents. I get $K_c = 1.69$. If $K_p = K_c(RT)^(Deltan_"gas")$, what would $K_p$ be if this...
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