Grams of $N_2$ reacts with 84.29 grams of $H_2$ in the chemical equation: $N_2 + H_2-> NH_3$ How do you balance the chemical equation and determine the limiting reactant? How much $NH_3$ is produced?

Md Ariful Islam

0 like 0 dislike
1 views
Share with your friends

1 Answers

Md Ariful Islam

Call

Three equiv of hydrogen react with 1 equiv of nitrogen to give one equiv ammonia. Of course, I could double this reaction to remove the 1/2 coefficients, but the will remain the same.

If you have 84.29 g dihydrogen, there are $(84.29*cancelg)/(2.02*cancelg*mol^-1)$ $=$ $41.7$ $mol$ $H_2$. Stoichiometry requires 27.8 mol dinitrogen ($=$ $?? g$). I think you have omitted some of the starting conditions in the problem

0 like 0 dislike
1 views
Talk Doctor Online in Bissoy App
How do you balance this chemical equation: $N_2 + H_2 -> NH_3$?

Since there are $3$ hydrogen atoms in $NH_3$ and $2$ in $H_2$, we will need a multiple of $3H_2$ on the left to balance the right hand side. Then notice...

1 Answers 1 views
How many moles of $NH_3$ are produced when 18.5 grams of $N_2$ gas reacts with excess $H_2$ gas?

Firstly, fully balance the chemical equation. $N_2 + 3H_2 => 2NH_3$ Use this formula $n = m / M$ where: $n$ = number of moles $m$ = mass of...

1 Answers 1 views
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...

1 Answers 1 views
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...

1 Answers 1 views
In the following equations, determine which reactant is the limiting reactant and which reactant is in excess.? The amounts mixed together are shown below each reactant. a) 2NaOH(10g) + H2SO4(10g) →Na2SO4+2H2O

Chemistry occurs in MOLE quantities. Masses (weights) are what we measure. So, to calculate reactions we need to put everything into terms of Moles before we can solve them. We...

1 Answers 1 views
What is the volume of $NH_3$ produced in the following reaction when 3.0 L of $N_2$ reacts with 4.0 L of $H_2$?

The balanced reaction is the following: $N_2(g)+3H_2(g)->2NH_3(g)$ We will assume that this reaction is happening at constant pressure and that the temperature is not changing through the entire process, therefore,...

1 Answers 1 views
Ammonia is produced in the reaction $3H_2 + N_2 -> 2NH_3$. What mass of $NH_3$ could be produced if 12.5 $H_2$ reacts with excess nitrogen?

We ASSUME $(i)$ $12.5*g$ dihydrogen gas, and $(ii)$ QUANTITATIVE reaction with stoichiometric dinitrogen. (And the second assumption is a bit unwarranted). $"Moles of dihydrogen"=(12.5*g)/(2.016*g*mol^-1)=6.20*mol$...and thus $2.07*mol$ of dinitrogen are required....

1 Answers 1 views
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...

1 Answers 1 views
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...

1 Answers 1 views
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. $3H_2$...

1 Answers 1 views
X