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2 years ago

The empirical formula for a compound is C2H4NO. If its molar mass is 232.2 g/mol, what is the molecular formula of the compound?

Chemistry

1 answer:

Irina18 [472]2 years ago

4 0

Empirical formula mass

C2H4NO
2(12)+4(1)+14+16
30+24+4
58g/mol

Molar mass=232.2g/mol

Find n

Molar mass/Empirical formula mass
232.2/58
4

Molecular formula

n×Empirical formula
4(C2H4NO)
C8H16(NO)_4

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When a piece of metal is irradiated with UV radiation (λ = 162 nm), electrons are ejected with a kinetic energy of 3.54×10-19 J.

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From the Question we are told that

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If 15 g of C₂H₆ reacts with 60.0 g of O₂, how many moles of water (H₂O) will be produced?

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Explanation:

Hello,

In this case, the undergoing chemical reaction is:

$2C_2H_6 + 7O_2 \rightarrow 4CO_2 + 6H_2O$

Next, we identify the limiting reactant by computing the available moles of ethane and the moles of ethane consumed by 60.0 grams of oxygen:

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Thus, we notice there are less available moles, for that reason, the ethane is the limiting reactant. Finally, we can compute the produced moles of water by:

$n_{H_2O}=0.50molC_2H_6*\frac{6molH_2O}{2molC_2H_6}\\\\n_{H_2O}=1.5molH_2O$

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