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20g of hydrogen and 128g of oxygen are contained in a 20L flask at \small 200^{\circ}C. If a spark ignites the mixture, what will be the final pressure (in atm)?

Option: 1

19.39


Option: 2

17.34


Option: 3

20.23


Option: 4

22.34


Answers (1)

best_answer

We have:
  \mathrm{Moles \ of \ H_2=\frac{20}{2}=10\ moles}  

 \mathrm{Moles\ of\ O_2=\frac{128}{32}=4 \ moles} 

Now, the stoichiometric equation is given as follows:

\\\mathrm{2H_{2}\:+\: O_{2}\: \rightarrow \: 2H_{2}O}

Thus, according to the given equation, 4 moles of oxygen will react with 8 moles of hydrogen and thus 2 moles of hydrogen will remain unreacted and 8 moles of gaseous water molecules will be formed.
Thus, final pressure if given as :

P=\frac{(n_{H_2}+n_{H_2O})RT}{V}

      =\frac{[(2+8)(0.082)\times 473]}{20}

       =19.39atm

 

Posted by

Shailly goel

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