Consider the following gas phase reaction: CH3OH(g) + HI(g) CH3(g) + H?O(g) If 2.66 liters of CH3OH(g) gas at 117°C and 0.842 atm is used, what volume of HI(g) gas at the same temperature and pressure will be consumed? liters

Consider the following gas phase reaction: $CH_{3} OH (g) + HI (g) ? CH_{3} I (g) + H_{2} O (g)$ If $2.66$ liters of $CH_{3} OH (g)$ gas at $11 7^{?} C$ and $0.842$ atm is used, what volume of $HI (g)$ gas at the same temperature and pressure will be consumed? liters

Question

Consider the following gas phase reaction: CH3OH(g) + HI(g) CH3(g) + H?O(g) If 2.66 liters of CH3OH(g) gas at 117°C and 0.842 atm is used, what volume of HI(g) gas at the same temperature and pressure will be consumed? liters

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Consider the following gas phase reaction:

CH_{3} OH (g) + HI (g) ? CH_{3} I (g) + H_{2} O (g)

If

2.66

liters of

CH_{3} OH (g)

gas at

11 7^{?} C

and

0.842

atm is used, what volume of

HI (g)

gas at the same temperature and pressure will be consumed? liters

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