The value of AH° for the reaction below is +128.1 kJ CH3OH (I)-CO (g) + 2H2 (g) How much heat is consumed when 87.1 g of hydrogen gas is formed? A) 2.76 x 103 kJ B) 5.52 x 103 kJ C) -5.52 x 103 kJ D) -2.76 x 103 kJ E) -128.1 kJ

A) 2.76 x 103 kJ

Explanation:

CH3OH (I)>CO (g) + 2H2 (g)

Number of moles contained in 87.1g of hydrogen gas= mass of hydrogen gas/ molar mass of hydrogen gas

Molar mass of hydrogen gas= 2gmol-1

Number of moles hydrogen gas = 87.1g/2gmol-1= 43.55 moles of hydrogen

1 mole of methanol yields 2 moles of hydrogen

x moles of methanol yields 43.55 moles of hydrogen

x= 43.55 moles of hydrogen × 1 mole of methanol/2 moles of hydrogen

x= 21.775 moles of methanol

Then;

If 1 mole of methanol absorbs 128KJ of energy

21.775 moles of methanol will absorb 21.775 × 128/1 = 2.7×10^3 KJ of heat

one negative thing it that it can kill water animals. another negative thing is it can cause the destruction of ecosystem. one way water pollution can be reduced is to conserve energy.