A compound of nitrogen and oxygen is 30.46% by mass N and 69.54% by mass O. The molar mass if the compound was determined to be 92 g/mol.
a. What is the empirical formula of the compound?
b. What is the molecular formula of the compound?

 characteristic molar mass of an element is simply the atomic mass in g/mol. However, molar mass can also be calculated by multiplying the atomic mass in amu by the molar mass constant (1 g/mol).

Explanation:

o calculate the molar mass of a compound with multiple atoms, sum all the atomic mass of the constituent atoms. so the answer to your question is B

answer: the enthalpy of the overall chemical reaction is +87.88 kj or +88 kj.

according to hess's law, the overall enthalpy of a reaction is the difference between the sum of enthalpy values of all the products and the sum of enthalpy values of all the reactants.

δh(reaction) = ∑nδh(products) - ∑nδh(reactants)

δh(reaction) = [δh +δh] - [δh]

δh(reaction) = [1(-287.02) + 1(0) ] - [1(-374.9)] kj = +87.88 kj

here, δh (pcl3) = -287.02 kj, δh(cl2) = 0, δh(pcl5) = -374.9 kj

therefore, enthalpy of the overall reaction is +87.88 kj or +88 kj.

3 1/4 %

explanation: