Please help with steps to solve both thank you. A compound has an empirical form

Question

Please help with steps to solve both thank you. A compound has an empirical formula of CH_2Cl. An independent analysis gave a value of 99.0 for its molar mass. What is the molecular formula of the compound? CH_2Cl C_2H_4Cl_2 C_2H_2Cl_4 C_3H_6Cl_3 C_3H_3Cl_6 Given: 3H_2(g) + N_2(g) implies 2NH_3(g) If the reaction starts with 0.500 mol of H_2, how many atoms of hydrogen in the compound NH_3 would you expect to make? 3.01 times 1023 atoms 6.02 times 1023 atoms 12.04 times 1023 atoms 1 atom 6 atoms

Explanation / Answer

3)

given empirical formula is CH2Cl

now

let the molecular formula be (CH2Cl)n

where

n = molar mass / empirical mass

now

mass of emprical formula CH2Cl = 49.5 g

given

molar mass = 99

so

n = 99 / 49.5

n = 2

so

the molecular formula is (CH2Cl)2 = C2H4Cl2

so

the answer is b) C2H4Cl

4)

3H2 + N2 ---> 2 NH3

we can see that

moles of NH3 formed = (2/3) x moles of H2

moles of NH3 formed = 2 x 0.5 / 3

moles of NH3 formed = 1/3

now

1 mole of NH3 contains 3 moles of H atoms

so

moles of H atoms = 3 x 1/3 = 1

now

we know that

number of atoms = moles x 6.02 x 10^23

so

number of H atoms = 1 x 6.02 x 10^23 = 6.02 x 10^23

so

the answer is b) 6.02 x 10^23 atoms

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