Methanol, ch, oh (mm = 32.05 g/mol), is prepared industrially from this gas-phase reaction:
co(g) + 2h2(g) - ch2oh()
in a laboratory test, a reaction vessel was filled with 63.4 g co (mm = 28.01 g/mol) and 97.2 g of hz.
how many grams of methanol would be produced in a complete reaction? which reactant remains left
over at the end of the reaction? how many grams of it remain?

Hydrogen will left.

Mass of hydrogen left = 88 g            

Mass of methane produced = 73.72 g

Explanation:

Given data:

Molar mass of methanol = 32.05 g/mol

Mass of carbon monoxide = 63.4 g

Molar mass of carbon monoxide = 28.01 g/mol

Mass of hydrogen gas = 97.2 g

Molar mass of hydrogen gas = 2 g/mol

Mass of  methanol = ?

Excess reactant = ?

Amount of excess reactant left = ?

Solution:

Chemical equation:

CO(g) + 2H₂(g)   → CH₃OH(g)

Number of moles of CO

Number of moles = mass/ molar mass

Number of moles = 63.4 g/ 28.01 g/mol

Number of moles = 2.3 mol

Number of moles of H₂:

Number of moles = mass/ molar mass

Number of moles = 97.2 g/ 2 g/mol

Number of moles = 48.6  mol

Now we compare the moles of methane with hydrogen and carbon monoxide gas through balanced chemical equation.

                       CO     :     CH₃OH

                        1        :          1

                        2.3    :        2.3

                      H₂        :        CH₃OH

                        2        :            1

                       48.6    :            1/2×48.6 = 24.45 mol

Number of moles of methane produced by CO are less so it will limiting reactant.

Mass of methane = moles × molar mass

Mass of methane = 2.3 mol × 32.05 g/mol

Mass of methane = 73.72 g

The hydrogen gas is in excess amount. Some of its amount will remain at the end of reaction unreacted.

Amount of hydrogen remain unreacted:

                              CO          :        H₂

                                1            :         2

                               2.3         :         2×2.3 = 4.6 mole

so 4.6 moles of H₂ react with 2.3 moles of CO.

Total number of moles of hydrogen = 48.6 mole

Number of moles left = 48.6 - 4.6 = 44 moles

Mass of hydrogen left = moles  × molar mass

Mass of hydrogen left = 44 mol  × 2g/mol

Mass of hydrogen left = 88 g            

a electronegativity decreases beacuse the size of nucleus is bigger.

water and alcohols have similar properties because water molecules contain hydroxyl groups that can form hydrogen bonds with other water molecules and with alcohol molecules, and likewise alcohol molecules can form hydrogen bonds with other alcohol molecules as well as with water.