What is the standard heat of reaction for the formation of NO2(g) from NO(g) and O2(g)? Write the balanced equation first. You can find the standard heats of formation in table 17.4 of your book on page 580. (Show all work including the equation you use to solve). (5 points). See page 581 for an example.

The answer to your question is ΔHf = -114.2 kJ/mol

Explanation:

Balanced chemical reaction

                2NO(g)  +  O₂(g)   ⇒   2NO₂(g)

Standard heat of formation

ΔHf NO (g) = 90.3 kJ/mol

ΔHf O₂ (g) = 0.0 kJ/mol

ΔHf NO₂ (g) = 33.2 kJ/mol

- For this reaction

ΔHf = ∑ΔHf products - ∑Hf reactants

-Substitution

ΔHf = 2(33.2) - 2(90.3) - 0

-Simplification

ΔHf = 66.4 - 180.6

-Result

ΔHf = -114.2 kJ/mol

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explanation:

answer : one can design an experiment using a liquid and an additive that can be added to the liquid and observe the chemical changes in the reaction species.

one would need a beaker which is filled with a known amount of the liquid in which thermometer is placed to measure the temperature changes; after addition of the additive to the liquid solution one can note down the temperature change and find whether the reaction is endothermic or exothermic in nature. by subtracting the initial temperature value with the final temperature one can find the temperature changes.

various combinations of liquid and additive can be used. liquid in this case can be a known quantity of water and additives can be epsom salt or without epsom salt the experiment can be conducted to notice the changes. water and ice, hydrogen peroxide and dry yeast, vinegar and baking soda,etc.