The molar mass of a compound is 92 g/mol. Analysis of a sample of the compound indicates that it contains 0.606g of N and 1.390g of O. Find its molecular formula.

The molecular formula shows the actual number of atoms of each element present in a compound. The molecular formula is different for different compounds.

The molecular formula of the given compound in the question is

An empirical formula is calculated first to find the molecular formula. First, let us calculate the empirical formula for the compound.

The data given in the question is as N is 0.606g  and O is  1.390g

After solving the equation,

Divide it by the smallest outcomes

The empirical formula is NO2. Now we have to find the molecular formula.

After solving the equation the value of 'n' is 2.

Hence, The molecular formula

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N2O4

Explanation:

To obtain the molecular formula of the compound, first, let us calculate the empirical formula for the compound. This is illustrated below:

N = 0.606g

O = 1.390g

Next, we divide the above by their molar masses

N = 0.606/14 = 0.0432

O = 1.390/16 = 0.0869

Next, we divide by the smallest

N = 0.0432/0.0432 = 1

O = 0.0869/0.0432 = 2

The empirical formula is NO2

The molecular formula is given by:

[NO2]n = 92

[14 + (16x2)]n = 92

[14 +32]n = 92

46n = 92

Divide both side by the coefficient of n i.e 46

n = 92/46

n = 2

The molecular formula = [NO2]n = [NO2]2 = N2O4

your answer is a. the enthalpy of formation for a pure element in its standard state is always positive.