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Julli [10]
3 years ago
6

- How many moles of H2O are required to react to form 2.5 grams of CH ?

Chemistry
1 answer:
abruzzese [7]3 years ago
7 0

Answer:

0.312 moles of H2O

Explanation:

no. of moles of ch4= mass ÷ molar mass

                               =2.5 ÷ 16.04

                               =0.156 moles of ch4

According to balanced chemical equation

CH4        :        H2O

1 mole     :        2 moles

0.156 moles :       x moles  

by cross multiplication

x=  (0.156x2) ÷ 1

 = 0.312 moles of H2O

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From the unbalanced reaction: B2H6 + O2 ---> HBO2 + H2O
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Answer: 125 g

Explanation:

To calculate the moles :

\text{Moles of solute}=\frac{\text{given mass}}{\text{Molar Mass}}    

\text{Moles of} B_2H_6=\frac{36.1g}{17}=1.30moles

The balanced reaction is:

B_2H_6+3O_2\rightarrow 2HBO_2+2H_2O

According to stoichiometry :

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Thus 1.30 moles of B_2H_6 will require=\frac{3}{1}\times 1.30=3.90moles  of O_2

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Thus 125 g of O_2 will be needed to burn 36.1 g of B_2H_6

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