Given the following balanced reaction between liquid ammonia and oxygen gas to produce nitrous oxide gas and water, how many grams of water, h2o, are produced from 317 grams of ammonia and excess oxygen? (to find the molar mass in the problem use the periodic table and round the mass to the hundreds place for calculation).
(a) 224 g
(b) 335 g
(c) 503 g

(C) 503 g

Explanation:

Balanced reaction:

2NH₃ + 2O₂ → N₂O + 3H₂O

Stoichiometry:

317 g NH₃ × (1 mol NH₃ / 17.03 g NH₃) = 18.61 mol NH₃

18.61 mol NH₃ × (3 mol H₂O / 2 mol NH₃) = 27.92 mol H₂O

27.92 mol H₂O × (18.02 g H₂O / mol H₂O) = 503 g H₂O

(C) 503 g of water, H2O, are produced from 317 grams of ammonia and excess oxygen

Explanation:

Molar mass of

Molar mass of

The conversions are

Step 1:

Mass to moles by dividing with molar mass

Step 2:

Moles to moles by using mole ratio of i.e., 2 : 3

Step 3:

Moles to mass by multiplying with molar mass

is formed.

(Answer)

Please note :

To convert moles to mass, we multiply by molar mass  

To convert mass to moles, we divide by molar mass

Molar mass is the mass of 1 mole of the substance

For example molar mass of is

(we just add the atomic mass of the atoms to get the molar mass of the substance).

explanation:

let the different atoms be x and y. each with four protons and same mass will be represented as follows.

mass number is number of protons + number of neutrons.

            and  

since, it is given that one has a negative charge while the other is neutral. therefore, there will be increase in number of protons and the atom will be represented as follows.

according to periodic table, mass number of beryllium is 9 and it has atomic number 4 so, the atoms will be and .  

the protons and neutrons will be located inside the nucleus whereas the electrons will be revolving around the nucleus.