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According to Dalton's law of partial pressures,
So the total pressure of the system is merely the partial pressures of each component added together:
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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...
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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...
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The total pressure of a container that has $NH_3(g)$ exerting a pressure of 346 torr, $N_2(g)$ exerting a pressure of 225 torr, and $H_2O (g)$ exerting a pressure of 55 torr?
And thus....................... $P_"total"=P_"ammonia"+P_"dinitrogen"+P_"water vapour"$ $=(346+225+55)$ $mm*Hg$ $=626*"Torr"$. How many atmospheres is this? Can you think of a way to estimate the temperature at which this experiment was performed? I can...
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At 15°C, a 1.00 L container contains 6.41 mol $N_2$ and 3.82 mol $Ar$. What is the partial pressure of each gas, and what is the total pressure inside the container?
Here's an alternative approach for which you only have to use the equation once. According to Dalton's Law of Partial Pressures, the of a gas that's part of a...
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Find the partial pressure in a solution containing ethanol and 1-propanol with a total vapor pressure of $"56.3 torr"$? The pure vapor pressures are $"100.0 torr"$ and $"37.6 torr"$, respectively, and the solution has a mol fraction of $0.300$ of ethanol.
Consider Raoult's law compared with Dalton's law of partial pressures: $P_i = overbrace(chi_(i(l))P_i^"*")^"Raoult's Law" = underbrace(chi_(i(v))P_"tot")_"Dalton's Law"$, where: $P_i$ is the partial vapor pressure of component $i$, i.e....
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A mixture of $"N"_2$, $"O"_2$. and $"CO"_2$ has a total pressure of $"740 torr"$ In this mixture, the partial pressure of $"N"_2$ is $"120 torr"$ and the partial pressure of $"O"_2$ is $"400 torr"$. What is the partial pressure of $"CO"_2$ ?
From Dalton's Law of , the total pressure of a mixture of gases is the sum of the partial pressures of each gas. Therefore, the partial pressure of $"CO"_2$ is...
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A quantity of $N_2$ gas originally held at 4.75 am in a 1.00L container at 26°C is transferred to a 10.0 L container at 20°C. What is the total pressure in the new container?
Notice that the volume and the temperature of the gas change when going from the first container to the second container, but that the number of moles of gas remains...
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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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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.........
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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...
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