The following thermochemical equation is for the reaction of methane(g) with water(g) to form hydrogen(g) and carbon monoxide(g). CH4(g) + H2O(g)3H2(g) + CO(g) H = 206 kJ When 4.20 grams of methane(g) react with excess water(g), kJ of energy are.

54.075KJ

Explanation:

Since methane is the limiting reactant.

From the reaction equation,

16 g of methane absorbs 206 KJ of energy

4.20 g of methane will absorb 4.20 × 206/16 = 54.075KJ of energy was absorbed.

From the equation, the value of the enthalpy of reaction is positive, this means that energy is absorbed in the reaction of methane and water. Hence the answer.

in 1783 cavendish was working with his hydrogen gas and found that when he burned it and condensed the vapor it was water. this was very significant since it disproved the greek theory of elements completely since water was not a simple substance but the product of two gases. it was lavoisier who hearing of the experiment gave cavendish's gas the name hydrogen ("water-producer") and added that hydrogen burned by combining with oxygen and that water was a hydrogen-oxygen combination.

explanation: