At 25°c and constant pressure, carbon monoxide gas combines with oxygen gas to give carbon dioxide gas with the evolution of 10.1 kj per gram of carbon monoxide consumed. what is the value of δh for the reaction as represented by the equation below.

Answer : The value of for the reaction is, -565.6 kJ

Explanation :

First we have to calculate the molar mass of CO.

Molar mass CO = Atomic mass of C + Atomic mass of O  = 12 + 16 = 28 g/mole

Now we have to calculate the moles of CO.

Now we have to calculate the value of for the reaction.

The balanced equation will be,

From the balanced chemical reaction we conclude that,

As, of CO release heat = 10.1 kJ

So, 2 mole of CO release heat =

Therefore, the value of for the reaction is, -565.6 kJ (The negative sign indicates the amount of energy is released)

it means there are 3 atoms of oxygen

> b takes place in the gas phase in an isothermal tubular reactor. the feed is one mole of a per one mole of c, an inert. the entering temperature and pressure are 427°c and 10 atm, respectively. the gas constant r = 0.08206 atm · l/mol · k.