Nitrogen dioxide reacts with water to produce oxygen and ammonia. A 5.00 L sample of H2O(g) reacts at a temperature of 361 ∘C and a pressure of 715 mmHg . How many grams of NH3 can be produced? 4NO2(g)+6H2O(g)→7O2(g)+4NH3(g)
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- Temperature in Kelvin (K) = 361 °C + 273.15 = 634.15 K Show more…
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Nitrogen dioxide reacts with water to produce oxygen and ammonia. A 5.00-L sample of $\mathrm{H}_{2} \mathrm{O}(g)$ reacts at a temperature of $375^{\circ} \mathrm{C}$ and a pressure of $725 \mathrm{mmHg} .$ How many grams of $\mathrm{NH}_{3}$ can be produced? $(11.8,11.9)$ $$ 4 \mathrm{NO}_{2}(g)+6 \mathrm{H}_{2} \mathrm{O}(g) \longrightarrow 7 \mathrm{O}_{2}(g)+4 \mathrm{NH}_{3}(g) $$
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Nitrogen dioxide reacts with water to produce oxygen and ammonia: 4NO2(g) + 6H2O(g) --> 7O2(g) + 4NH3(g). At a temperature of 415 degrees C and a pressure of 725 mmHg, how many grams of NH3 can be produced when 4.00 L of NO2 reacts?
Ma Ednelyn L.
Nitrogen dioxide reacts with water to produce oxygen and ammonia. How many grams of $\mathrm{NH}_{3}$ can be produced when $4.00 \mathrm{~L}$ of $\mathrm{NO}_{2}$ reacts at $415^{\circ} \mathrm{C}$ and $725 \mathrm{mmHg}$ ? $$ 4 \mathrm{NO}_{2}(g)+6 \mathrm{H}_{2} \mathrm{O}(g) \longrightarrow 7 \mathrm{O}_{2}(g)+4 \mathrm{NH}_{3}(g) $$
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