Methanol can be produced by the following reaction: CO(g) + 2 H2(g) -> CH3OH(g). How is the rate of disappearance of hydrogen gas related to the rate of appearance of methanol? A) -?[H2] / ?t B) + 1/2 ?[CH3OH] / ?t C) +2 ?[CH3OH] / ?t D) none of these
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The chemical reaction given is CO(g) + 2 H2(g) → CH3OH(g). This reaction shows that carbon monoxide (CO) reacts with hydrogen gas (H2) to produce methanol (CH3OH). Show more…
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Methanol can be produced by the following reaction: $\mathrm{CO}(\mathrm{g})+2 \mathrm{H}_{2}(\mathrm{~g}) \rightarrow \mathrm{CH}_{3} \mathrm{OH}(\mathrm{g})$ How is the rate of disappearance of hydrogen gas related to the rate of appearance of methanol?$-\frac{\Delta\left[\mathrm{H}_{2}\right]}{\Delta \mathrm{t}}=?$ a. $+\frac{2 \Delta\left[\mathrm{CH}_{3} \mathrm{OH}\right]}{\Delta \mathrm{t}}$ b. $+\frac{1 \Delta\left[\mathrm{CH}_{3} \mathrm{OH}\right]}{2 \Delta \mathrm{t}}$ c. $+\frac{\Delta\left[\mathrm{H}_{4}\right]}{\Delta t}$ d. None of these
Here is one way to produce methanol: CO + 2 H2 → CH3OH. This reaction has a ΔH rxn = -128 kJ. How much heat (in kJ) is released when you completely react 4.04 g CO? A. -517 kJ B. -128 kJ C. -14,500 kJ D. -18.5 kJ E. none of the above
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Methanol, $\mathrm{CH}_{3} \mathrm{OH}$, is a clean-burning, easily handled fuel. It can be made by the direct reaction of $\mathrm{CO}$ and $\mathrm{H}_{2}$. $$ \mathrm{CO}(\mathrm{g})+2 \mathrm{H}_{2}(\mathrm{~g}) \longrightarrow \mathrm{CH}_{3} \mathrm{OH}(\ell) $$ (a) Starting with a mixture of $12.0 \mathrm{~g} \mathrm{H}_{2}$ and $74.5 \mathrm{~g} \mathrm{CO}$, which is the limiting reactant? (b) What mass of the excess reactant, in grams, is left after reaction is complete? (c) What mass of methanol can be obtained, in theory?
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