Question

how much heat is evolved when 12 gram of CO react with an O2 according to the following reaction
4CO +2NO2 -》4CO2+ N2
H = -1198 kilo Joule​

Answer 1

Answer:

incomeplete question is this

Answer 2

The amount of heat released for the given amount of CO is 128.8 kJ

Explanation:

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

Given mass of CO = 12 g

Molar mass of CO = 28 g/mol

Putting values in above equation, we get:

$\text{Moles of CO}=\frac{12g}{28g/mol}=0.43mol$

Sign convention of heat:

When heat is absorbed, the sign of heat is taken to be positive and when heat is released, the sign of heat is taken to be negative.

For the given chemical equation:

$4CO+2NO_2\rightarrow 4CO_2+N_2;\Delta H=-1198kJ$

By Stoichiometry of the reaction:

4 moles of CO releases 1198 kJ of heat

So, 0.43 moles of Co will release = $\frac{1198}{4}\times 0.43=128.8kJ$ of heat

Learn more about heat released or stoichiometry:

https://brainly.in/question/13308680

https://brainly.com/question/14034197

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