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What is the molecular structure of $"nitrous oxide"$, $N_2O$?
And how do we know? Well, by experiment, and measurement, but VESPER gives a good approximation. We have $2xx5+6=16$ $"valence electrons"$ to distribute over 3 centres. A structure of $N-=N^(+)-O^(-)$...
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How many moles of $NO_2$ are there in $1.81 * 10^24$ molecules of $NO_2$?
In finding the amount of moles there are, you first have to know what is and what it represents. Avogadro's number is $6.022$x$10^23$. That number can represent anything; in chemistry...
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A 1.50-g sample of nitrous oxide contains $2.05 * 10^22$ $N_2O$ molecules. How many nitrogen atoms are in this sample? How many nitrogen atoms are in 44.0 g of nitrous oxide?
Note: This answer may seem to be quite long, but that is because I have tried to explain each of the steps fully and clearly. If you want, you can...
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How many moles of nitrogen, N, are in 85.0 g of nitrous oxide, $N_2O$?
$"Moles of nitrous oxide"=(85*g)/(44.01*g*mol^-1)$ $=1.93*mol$. Since, clearly, there are $"2 moles of nitrogen atoms"$ $"per mole of nitrous oxide"$, we simply double the molar quantity of $"nitrous oxide:"$ $1.93*molxx2*mol*N*mol^-1NO=??mol$
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A sample of $N_2O$ gas has a density of 2.85 g/L at 298 K. What must be the pressure of the gas (in mmHg)?
From (PV = nRT) $P = (nRT/V) = (R("mass"/"f.wt")(T/V))$ $P = R("mass"/"Volume")(T/"f.wt.")$= $R("Density")(T/"f.wt.")$ Given: $R = 0.08206("L-Atm"/"mol-K")$ $"Density" = 2.85(g/L)$ $T = 298K$ $f.wt. = 44(g/"mol")$ $P = (0.08206"L-Atm"/"mol-K")(2.85g/L)(298K)(44g/"mol")^-1 =...
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My textbook says that that for a mixture of $15.2*g$ helium gas, and $30.6*g$ dioxygen gas, the partial pressure is dominated by the helium. Can you find $P_"He"$, and $P_"dioxygen"$ and $P_"Total"$?
$"Dalton's Law of Partial Pressures"$ states UNEQUIVOCALLY that in a gaseous mixture, the partial pressure exerted by a gaseous component is the SAME as it would exert if it ALONE...
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A container under $2558*"psi"$ pressure contains carbon dioxide and whose partial pressure is $54.6*"bar"$ and $NO_2$? What is $P_(NO_2)$ in atmospheres?
$"Dalton's Law of partial pressures"$ holds that in a gaseous mixture, the total pressure is the sum of the individual partial pressures; i.e. the sum of the pressures of the...
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The reaction $2NO_2 -> 2NO + O_2$ obeys the rate law $(Delta[O_2])/(Deltat) = (1.40 xx 10^-2 )[NO_2]^2$ at 500 K. If the initial concentration of $NO_2$ is 1.00 M, how long will it take for the $[NO_2]$ to decrease to 25.0% of its initial value?
I got $"71.4 s"$, after we have gone through the two half-lives for $"NO"_2$. This seems to be a second-order half-life (yes, that is a thing). I don't know...
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How is $"Mohr's salt"$ oxidized by $"potassium permanganate"$ to give $Fe^(3+)$ and $Mn^(2+)$? How is $"hydrogen peroxide"$ oxidized by the same reagent to give $"dioxygen gas"$?
You used the so-called $"Mohr's salt"$, which is a stable and convenient source of $"Fe(II) salt"$, i.e. $[(NH_4)_2Fe(SO_4)_2]*6H_2O$. We can ignore the ammonium and sulfate shrubbery, and represent the redox...
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How is $NO_2$ oxidized by $Cr_2O_7^(2-)$ to give nitrate ion?
$"Oxidation half equation:"$ $NO_2(g) +H_2O(l) rarr NO"_3^(-) +2H^+ + e^(-) $ $stackrel(+IV)Nrarrstackrel(+V)N$ Charge and mass are balanced so tick. $"Reduction half equation:"$ $Cr_2O_7^(2-)(aq) +14H^(+) +6e^(-) rarr 2Cr^(3+) +7H_2O $ $stackrel(VI+)"Cr"rarrstackrel(+III)"Cr"$...
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