What is the molecular formula for the compound with a formula mass of 58.12 and an empirical formula of c2h5?

C₄H₁₀

Explanation:

The empirical formula is the reduced formula of the molecule. So, calling n the number of empirical formulas, the molecule formula will be:

n(C₂H₅)

The molar mass of C is 12 g/mol, and of H is 1 g/mol. So, the total mass will be:

nx(2x12 + 5x1) = 58.12

29n = 58.12

n = 2

Then, the molecular formula is:

2(C₂H₅) = C₄H₁₀

n+h→nh3

we must remember that nitrogen and hydrogen are both diatomic molecules in their standard gas form. this adjusts the equation to

n2+h2→nh3

now we need to adjust coefficients in order to balance the atoms on each side of the equation. currently we have 2 atoms of nitrogen and 2 atoms of hydrogen on the reactant side and 1 atom of nitrogen and 3 atoms of hydrogen on the product side.

we can balance the hydrogens by placing a coefficient of 2 in front of ammonia and a coefficient of 3 in front of the hydrogen.

n2+3h2→2nh3

this gives us 6 hydrogen on each side and coincidentally the nitrogens now equal 2 on each side.

answer; i believe that the correct answer is (c) explore the outer planets; / plz check good luck