1 Answers
Call
Talk Doctor Online in Bissoy App
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...
1 Answers 1 views
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?
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...
1 Answers 1 views
What is the total pressure of a container that has $NH_3(g)$ exerting a pressure of 34 torr, $N_2(g)$ exerting a pressure of 225 torr, and $H_2O(g)$ exerting a pressure of 55 torr?
According to Dalton's law of partial pressures, $P_(t otal) = P_1 + P_2 + P_3 ...$ So the total pressure of the system is merely the partial pressures of each...
1 Answers 1 views
A yield of $NH_3$ of approximately 98% can be obtained at 200 deg C and 1,000 atmospheres of pressure. How many grams of $N_2$ must react to form 1.7 grams of ammonia, $NH_3$?
We always have to read the problems completely to understand the question. In this case even when we have pressure and temperature conditions specified, they don't matter, first because they...
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
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...
1 Answers 1 views
Which equation is unbalanced?
$HCl(aq)+H_2O(l)rarr Cu^(2+) + 2NO_3^-$;
$Ca(OH)_2(s) stackrel(H_2O)rarr Ca^(2+) +2HO^-$;
$Ca(NO_3)_2(s) stackrel(H_2O)rarr Ca^(2+) +2NO_3^-$
;$NH_3(aq) +H_2O(l) rightleftharpoonsNH_4^+ + HO^-$;
$HCl(aq)+H_2O(l)rarr Cu^(2+) + 2NO_3^-$ $Ca(OH)_2(s) stackrel(H_2O)rarr Ca^(2+) +2HO^-$ $Ca(NO_3)_2(s) stackrel(H_2O)rarr Ca^(2+) +2NO_3^-$ $NH_3(aq) +H_2O(l) rightleftharpoonsNH_4^+ + HO^-$ And one of these things is not like the other ones.........
1 Answers 1 views
How does ammonia behave as a Bronsted base:
$"(i) "NH_3(g) + 7/2O_2(g) rarr 2NO_2(g) + 3H_2O$
$"(ii) "2NH_3(g) rarr NH_4^+ +NH_2^(-) $
$"(iii) "NH_3(g) + H_3CBr(g) rarr H_3CBr(g) + HBr(g)$
$"(iv) "NH_3(aq) +H_2O(l) rarr NH_4^+ + HO^-$?
Ammonia is a Bronsted base: $NH_3(aq) + H_2O(l) rightleftharpoons NH_4^+ + OH^-$ $pK_b = 4.75$ I am not going to solve this equation using $pK_b$, but most of the ammonia...
1 Answers 1 views