A 1.47 g sample of a gaseous oxide of nitrogen occupies a volume of 1.23 L at 35°C and 763 mmHg. What is the most likely formula for the gas? NO NO2 NO3 N2O N2O4
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Temperature should be in Kelvin and pressure should be in atm. Temperature in Kelvin = 35 + 273.15 = 308.15 K Pressure in atm = 763 mmHg * (1 atm / 760 mmHg) = 1.004 atm Show more…
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Nitrogen forms several gaseous oxides. One of them has a density of $1.33 \mathrm{~g} / \mathrm{L}$ measured at $764 \mathrm{mmHg}$ and $150^{\circ} \mathrm{C}$. Write the formula of the compound. (a) NO (b) $\mathrm{N}_{2} \mathrm{O}$ (c) $\mathrm{NO}_{2}$ (d) $\mathrm{N}_{2} \mathrm{O}_{5}$
Ammonia gas is synthesized by combining hydrogen and nitrogen: $$ 3 \mathrm{H}_{2}(\mathrm{g})+\mathrm{N}_{2}(\mathrm{g}) \longrightarrow 2 \mathrm{NH}_{3}(\mathrm{g}) $$ (a) If you want to produce 562 g of $\mathrm{NH}_{3}$, what volume of $\mathrm{H}_{2}$ gas, at $56^{\circ} \mathrm{C}$ and $745 \mathrm{mm} \mathrm{Hg}$, is required? (b) To produce 562 g of $\mathrm{NH}_{3},$ what volume of air (the source of $\mathrm{N}_{2}$ ) is required if the air is introduced at $29^{\circ} \mathrm{C}$ and $745 \mathrm{mm}$ Hg? (Assume the air sample has $\left.78.1 \text { mole } \% N_{2} .\right)$
Ammonia gas is synthesized by combining hydrogen and nitrogen: $$ 3 \mathrm{H}_{2}(\mathrm{g})+\mathrm{N}_{2}(\mathrm{g}) \rightarrow 2 \mathrm{NH}_{3}(\mathrm{g}) $$ (a) If you want to produce 562 g of $\mathrm{NH}_{3}$, what volume of $\mathrm{H}_{2}$ gas, at $56^{\circ} \mathrm{C}$ and $745 \mathrm{mm} \mathrm{Hg}$ is required? (b) Nitrogen for this reaction will be obtained from air. What volume of air, measured at $29^{\circ} \mathrm{C}$ and $745 \mathrm{mm} \mathrm{Hg}$ pressure, will be required to provide the nitrogen needed to produce $562 \mathrm{g}$ of $\mathrm{NH}_{3}$ ? Assume the sample of air contains 78.1 mole $\% \mathrm{N}_{2}$
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