Given the thermochemical equation, H2 (8) + Br2 (1) ► 2HBr(g), AH = -72.4 kJ/mol, calculate the amount of heat released when a kilogram of
H2 (g) is consumed in this reaction.

Solved

Show answers

Ответ:

whereswoodruff

16.10.2021

Chemistry

$K=3.9*10^{-82}$

Explanation:

Reactions:

$NO_2 (g) \longleftrightarrow NO (g) +O (g)$

With: $K_1=\frac{[NO][O]}{[NO_2]}=6.8*10^{-49}$

$O_3 (g) + NO (g) \longleftrightarrow NO_2 (g) + O_2 (g)$

With: $K_2=\frac{[NO_2}{[O_3][NO]}=5.8*10^{-34}$

To achive the reaction we combine those two reactions:

$NO_2 (g) + O_3 (g) + NO (g) \longleftrightarrow NO (g) + O (g) + NO_2 (g)$

$O_3 (g) \longleftrightarrow O (g) + O_2 (g)$

The equilibrium constant:

$K= K_1*K_2=(6.8*10^{-49})*(5.8*10^{-34})=3.9*10^{-82}$

0,0(0 оценок)

Ask your question to the AI advisor

Ai-bot is an expert in any field and is the perfect companion for reliable and useful answers and advice on a variety of topics, including science, history, technology, art, sports, health, culture and more.

Ask your question

More tips

Answers on questions: Chemistry

Ask an AI advisor a question

I want advice

Given the thermochemical equation, H2 (8) + Br2 (1) ► 2HBr(g), AH = -72.4 kJ/mol, calculate the amount of heat released when a kilogram of H2 (g) is consumed in this reaction.