Question

The reaction of carbon dioxide(g) with hydrogen(g) to form carbon monoxide(g) and water(g) proceeds as follows:CO2(g) + H2(g) --->CO(g) + H2O(g)When 16.4 grams of CO2(g) react with sufficient H2(g) , 15.4 kJ of energy areabsorbed .What is the value of --->H for the chemical equation given?ΔHrxn = kJ

Answer 1

ΔHrxn = 41.3 kJ

Step-by-step explanation:

Let's consider the following equation.

CO₂(g) + H₂(g) ⇒ CO(g) + H₂O(g)

When 16.4 g of CO₂ react 15.4 kJ of energy are absorbed. In the balanced equation, there is 1 mole of CO₂, so we have to calculate the heat absorbed per mole of CO₂. Taking into account that the molar mass of CO₂ is 44.01 g/mol, the enthalpy of reaction (ΔHrxn) is:

`1molCO_(2).(44.01gCO_(2))/(1molCO_(2)) .(15.4kJ)/(16.4gCO_(2)) =41.3kJ`