The standard heat of formation for cdo(s) is -258 kj/mol at 298 k. write the formation equation for cdo(s) that goes with this value of δh°. use the pull-down boxes to specify states. write fractions with a slash, such as 1/2 for one half. if a box is not needed leave it blank.

Cd(s) + 1/2 O₂(g) ⇒ CdO(s) ΔH° = -258 kJ/mol

Explanation:

The standard heat of formation corresponds to the reaction of synthesis of 1 mole of the desired product from the simple substances in their most stable form under standard conditions (1 bar, 25°C). The resulting thermochemical equation is:

Cd(s) + 1/2 O₂(g) ⇒ CdO(s) ΔH° = -258 kJ/mol

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: