The mass of ammonia required to produce 2.40 × 10⁵ kg of (NH₄)₂SO₄ is 6.18 * 10⁴ Kg of ammonia.
<h3>What mass in kilograms of ammonia are required to produce 2.40 × 10⁵ kg of (NH₄)₂SO₄?</h3>
The mass of ammonia required to produce 2.40 × 10⁵ kg of (NH₄)₂SO₄ is determined from the mole ratio of the reaction.
The mole ratio of the reaction is obtained from the balanced equation of the reaction given below:
- 2NH₃(g) + H₂SO₄(aq) → (NH₄)₂SO₄(aq)
Mole ratio of NH₃ and (NH₄)₂SO₄ is 2: 1
Mass of 2 moles of ammonia = 2 * 17 = 34 g
Mass of 1 mole of (NH₄)₂SO₄ = 132 g
Mass of ammonia required = 34/132 * 2.40 × 10⁵ kg
Mass of ammonia required = 6.18 * 10⁴ Kg of ammonia.
In conclusion, the mole ratio is used to determine the mass of ammonia required.
Learn more about mole ratio at: brainly.com/question/19099163
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Answer:
The difference between the Thompson's plum pudding model and the Rutherford atom model is the location of the electrons (option a).
Explanation:
While Thompson compared his atom to a plum pudding, where the electrons floated freely in the pudding, Rutherford established the arrangement of the electrons in orbitals, which were found around the atomic nucleus like the planets around the sun.
Rutherford's findings also established the existence of a small, positively charged nucleus.
<em>Thompson and Rutherford models did not differentiate between the charges of electrons and protons
, overall charges or overall size of the atom.</em>
50 degrees, the angle of incident is always equal to the angle of reflection
The correct answer is A, Volume
