Water gas (a mixture of carbon monoxide and hydrogen) is prepared by passing steam over red-hot coke: c(s) + h2o(g) → co(g) + h2(g) for many years, water gas was used as a fuel in industry and for domestic cooking. compare the heat produced by the complete combustion of 1 mole of methane (ch4) with a mole of water gas (0.50 mole h2 and 0.50 mole co) under standard conditions. (assume liquid water is formed.) what is the difference between the two values?

-605,5 kJ/mol of energy

Explanation:

Combustion of CH₄, CO and H₂ are:

CH₄(g) + 2O₂(g) → CO₂(g) + 2H₂O(l)   ΔH = -890 kJ/mol

CO(g) + ¹/₂O₂(g) → CO₂(g) ΔH = -283 kJ/mol

H₂(g) + ¹/₂O₂(g) → H₂O(l) ΔH = -286 kJ/mol

The heat combustion of methane gives -890 kJ/mol of energy. The water gas gives the average of energy between the reactions, that is:

-283kJ/mol -286kJ/mol /2 = -284,5 kJ/mol of energy

Difference between the two values is:

-890kJ/mol - (-284,5kJ/mol) = -605,5 kJ/mol of energy

I hope it helps!

there all right good

explanation:

number of molecules / avogadro's number * molecule molecular = mass

explanation:

we define a gram-molecular weight as the mass of one mole of any element or compound. a mole contains avogadro's number of units (molecules) –  

6.022

x

10

23

. so, dividing the number of molecules by avogadro's number gives us the number of moles. multiplying that by the molecular weight gives us the mass. from the periodic table we find the gram-molecular weight of u to be238 and of f to be19. so,  

u

f

6

will have a gram-molecular weight of 352g.