Given the following reaction: N2(g) + 3 H2(g) --> 2 NH3(g) If the concentration of hydrogen decreases by 3 mol/L in 45 seconds, what is the corresponding rate of disappearance of nitrogen? 0.022 mol/L ·s 0.067 mol/L ·s 0.080 mol/L ·s 0.20 mol/L ·s
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Given reaction: N2(g) + 3 H2(g) → 2 NH3(g) Rate of reaction = -1/3 * Δ[H2]/Δt = Δ[N2]/Δt Show more…
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Given the following balanced equation, N2(g) + 3 H2(g) → 2 NH3(g) When [H2] is decreasing at 0.35 mol/L·s, at what rate is [NH3] increasing? 0.53 mol/L·s 0.12 mol/L·s 0.23 mol/L·s 0.12 mol/L·s 0.70 mol/L·s
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For the reaction; $4 \mathrm{NH}_{3(\mathrm{~g})}+5 \mathrm{O}_{2(\mathrm{~g})} \longrightarrow 4 \mathrm{NO}_{(\mathrm{g})}+6 \mathrm{H}_{2} \mathrm{O}_{(\mathrm{g})}$, the rate of reaction in terms of disappearance of $\mathrm{NH}_{3}$ is $-\frac{d\left[\mathrm{NH}_{3}\right]}{d t}$, then write the rate expression in terms of concentration of $\mathrm{O}_{2}, \mathrm{NO}$ and $\mathrm{H}_{2} \mathrm{O}$
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