How many grams of H2SO4 do I need to use in order to produce 3.01 moles of water? consider the equation. _Ca(OH)2 + _H2SO4 = _CaSO4 + _H20

148 g H₂SO₄

General Formulas and Concepts:

Chemistry - Stoichiometry

Explanation:

Step 1: Define

RxN:   Ca(OH)₂ + H₂SO₄ → CaSO₄ + H₂O

Given:   3.01 moles H₂O

Step 2: Balance RxN

Ca(OH)₂ + H₂SO₄ → CaSO₄ + 2H₂O

Step 3: Define conversions

Molar Mass of H - 1.01 g/mol

Molar Mass of S - 32.07 g/mol

Molar Mass of O - 16.00 g/mol

Molar Mass of H₂SO₄ - 2(1.01) + 32.07 + 4(16.00) = 98.09 g/mol

Step 4: Stoichiometry

= 147.625 g H₂SO₄

Step 5: Check

We are given 3 sig figs. Follow sig fig rules.

147.625 g H₂SO₄ ≈ 148 g H₂SO₄

hydrocarbons are organic compounds that contain only hydrogens and carbons. they can be saturated (those which contain only carbon-carbon single bonds) or unsaturated (those which contain carbon-carbon double or triple bonds) in nature. hydrocarbons can undergo several reactions like substitution, elimination etc.  

on substituting one or more hydrogen atoms in hydrocarbon it results in the formation of haloalkane. as the halogen atoms are large compared to the carbon and hydrogen atoms, due to which the molecular weight increases and the bond become polar because of presence electronegative halogen atom and results in the increase in boiling point of the haloalkane.

thus, the correct option is (b) that is the boiling point of the new compound increases on substituting a hydrogen atom with a halogen in a hydrocarbon.