12. In rocket fuel (as in many of the balloons we blow up in class), hydrogen gas (H2) reacts with oxygen gas (O2) to form water vapor. a) Write a balanced reaction for the process. b) Suppose you have a mini rocket and access to 2.50 L of oxygen gas and 4.00 L of hydrogen gas. If you use up all of the gas possible blasting off your rocket, how many liters of water vapor did you produce (at the same temperature as the original mixture)

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kobenhavn kobenhavn · Answer 1 · 2021-03-26T04:57:39+01:00

Answer: a) [tex]2H_2(g)+O_2(g)\rightarrow 2H_2O(g)[/tex]

b) 4.00 L of [tex]H_2O[/tex] will be produced

Explanation:

a) The balanced chemical reaction is:

[tex]2H_2(g)+O_2(g)\rightarrow 2H_2O(g)[/tex]

b) According to avogadros law, equal moles of gases occupy equal volumes at same temperature and presure conditions.

According to stoichiometry :

2 L of [tex]H_2[/tex] require = 1 L of [tex]O_2[/tex]

Thus 4.00 L of [tex]H_2[/tex] will require=[tex]\frac{1}{2}\times 4.00=2.00L[/tex] of [tex]O_2[/tex]

Thus [tex]H_2[/tex] is the limiting reagent as it limits the formation of product and [tex]O_2[/tex] is the excess reagent.

As 2 L of [tex]H_2[/tex] give = 2 L of [tex]H_2O[/tex]

Thus 4.00 L of [tex]H_2[/tex] give =[tex]\frac{2}{2}\times 4.00=4.00L[/tex] of [tex]H_2O[/tex]

Thus 4.00 L of [tex]H_2O[/tex] will be produced

andromache andromache · Answer 2 · 2022-03-18T17:46:45+01:00

a. The balanced reaction for the process should be 2h_2(g) + O_2(g) ⇒2H_2O(g)

b. The number of liters of water vapor should be 4.00 liters of H_2O.

a. The balanced reaction for the process should be 2h_2(g) + O_2(g) ⇒2H_2O(g)

b. As per the law, the equal moles of gases occupied equal volumes at the similar temperature

So, the number of liters should be

= 2/2*4.00

= 4.00 of H_2O

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