Question

Given the following information: aHCO3(s)+85 kJ Na2CO3(s)+H2O(1) CO2(g) Calculate the amount of heat (ink) required to decompose 2.24 mol NaHCO3(s). You must show your work to receive credit .

Answer 1

The amount of heat required comes out to be 190.4 KJ

Step-by-step explanation:

The reaction for the decomposition of
`NaHCO_(3)` is shown below
`\textrm{NaHCO}_(3)\left ( s \right )\rightarrow \textrm{Na}_(2)\textrm{CO}_(3)\left ( s \right )+\textrm{H}_(2)\textrm{O}\left ( l \right )+\textrm{CO}_(2)\left ( g \right )`

Amount of heat required to decompose 1 mole
`NaHCO_(3)` = 85 KJ

Amount of heat required to decompose 2.24 mole
`NaHCO_(3)` =
`\left ( 2.24 \textrm{ mole} * 85 \textrm{ KJ} \right ) = 190.4 \textrm{ KJ}`

Amount of heat required = 190.4 KJ