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A sample of carbon is placed in a rigid 1.50 L flask. Dinitrogen monoxide is added and the flask heated to 800C. When the system reached equilibrium the partial pressure of the carbon dioxide is found to be 0.030 atm and the partial pressure of the dinitrogen monoxide to be 1.48 atm. What is the partial pressure of nitrogen in the mixture.
The of nitrogen is 0.060 atm. First, write the balanced chemical equation for the equilibrium. C(s) +2N₂O(g) ⇌ CO₂(g) + 2N₂(g) There was no CO₂ or N₂ present at the...
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A container of gas with a pressure of 450 kPa contains three different gasses -hydrogen, oxygen, and nitrogen. If the partial pressure of the hydrogen is 210 kPa and the partial pressure of the oxygen is 125 kPa, what is the partial pressure of nitrogen?
According to Dalton's law of partial pressures, the total pressure is equivalent to the sum of the pressures of the individual gases (if they were present alone). Therefore, the...
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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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What is the oxidizing agent in $1/8"S"_8("orthorhombic") + "O"_2(g) -> "SO"_2(g)$, the formation reaction for sulfur dioxide gas?
Let's put it this way: what do you think of assigning oxygen the role of oxidizing agent? Does that make sense? If not, then we can do it another way....
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The equilibrium constant for the reaction: $PCl_5 rightleftharpoons PCl_3 + Cl_2$ is 0.0121. A vessel is charged with $PCl_5$, giving an initial pressure of 0.123 atmospheric. How do you calculate the partial pressure of $PCl_3$ at equilibrium?
$K_p=(P_(PCl_3)P_(Cl_2))/P_(PCl_5)=0.0121$ Initially, $P_(PCl_5)=0.123*atm$, if a quantity $x$ dissociates, then, $K_P=0.0121=x^2/(0.123-x)$ (I have assumed that the quoted equilibrium constant is $K_P$ not $K_c$. And if I am wrong, I am wrong)....
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Consider the following reaction: $Xe(g) + 2F_2(g) -> XeF_4(g)$. A reaction mixture initially contains 2.24 atm $Xe$ and 4.27 atm $F_2$. lf the equilibrium pressure of $Xe$ is 0.34 atm, how do you find the equilibrium constant ($K_p$) for the reaction?
The equilibrium reaction given to you looks like this $"Xe"_ ((g)) + color(red)(2)"F"_ (2(g)) rightleftharpoons "XeF"_ (4(g))$ You know that the mixture initially contains $"2.24 atm"$ of...
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A vessel contains a mixture of nitrogen and oxygen. If the partial pressure of nitrogen is 20 atmospheres and the partial pressure of oxygen is 42.8 atmospheres, what is the total pressure inside the vessel?
Datlon's law of Partial Pressures states that in a gaseous mixture, the exerted by a gaseous component is the same as the pressure it would exert if it ALONE occupied...
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At equilibrium, the partial pressure of $SO_2$ is 35.0 atm and that of $O_2$ is 15.9 atm. What is the partial pressure of $SO_3$ in atm?
$2SO_2+O_2rarr2SO_3$ $K_p=(p_(SO_3)^2)/(p_(SO_2)^2xxp_(O_2))$ $=$ $??$ We need to know $K_p$ in order to access $p_(SO_3)$.
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A mixture of two gases has a total pressure of 5.7 atm. If one gas has a partial pressure of 4.1 atm, what is the partial pressure of the other gas?
I got $"1.6 atm"$. DALTON'S LAW OF PARTIAL PRESSURES The equation that sums up what we have to do in this problem (pun intended) is Dalton's law of partial...
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If $\tt{\DeltaG°_(f,NO_2(g))=31.3" kJ"//"mol"}$ and $\tt{\DeltaG°_(f,NO(g))=86.6" kJ"//"mol"}$ at 298 K, then calculate $\tt{K_p}$ at 298 K?
Just like we did , this problem just reverses the situation. However, the $DeltaG_f^@$ of $"NO"_2(g)$ is incorrect, and it should be $"51.3 kJ/mol"$, as shown by two sources here:...
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