a chemist needs 46 mol of ammonia for a reaction to complete. he has 46 grams available but needs ammonia as a liquid (D=2.4g/ml). does he have enough? ammonia has an atomic weight of 17 grams

If the chemist needs 46 moles and he has 46 grams, that isn't enough.

im trying to do the dimensional analysis for it but i keep getting up to a point and stopping.

i get as far as....

46g x 1mole/17g x ___/ mole

... im not really sure what to do after that.

46 grams x (1 mole NH3/17 g NH3) = 2.70 moles. 2.70 moles is < 46 moles.

To determine if the chemist has enough ammonia in grams to meet the required quantity in moles, we need to convert the moles of ammonia to grams using its molar mass.

The molar mass of ammonia (NH₃) is calculated by adding up the atomic masses of nitrogen (N) and hydrogen (H):
Molar Mass(NH₃) = (1 × Atomic Mass(N)) + (3 × Atomic Mass(H))
Molar Mass(NH₃) = (1 × 14 g/mol) + (3 × 1 g/mol)
Molar Mass(NH₃) = 17 g/mol

Given that the chemist has 46 mol of ammonia, we can calculate the required mass of ammonia in grams:
Mass(NH₃) = Moles(NH₃) × Molar Mass(NH₃)
Mass(NH₃) = 46 mol × 17 g/mol
Mass(NH₃) = 782 g

Now, let's check whether the chemist has enough ammonia in grams. The chemist has 46 grams of ammonia available, and since the density of ammonia (D) is 2.4 g/mL, we can calculate the volume of ammonia:
Volume(NH₃) = Mass(NH₃) / Density(NH₃)
Volume(NH₃) = 46 g / 2.4 g/mL
Volume(NH₃) ≈ 19.17 mL

Since the chemist needs ammonia in liquid form, we compare the volume of ammonia obtained (19.17 mL) with the required volume. If the obtained volume is less than the required volume, then the chemist does not have enough ammonia to complete the reaction.