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3 years ago

Explain the difference between physical equilibrium and chemical equilibrium. Give two examples of each.

Chemistry

1 answer:

olganol [36]3 years ago

5 0

Explanation:

In a chemical equilibrium, there are different reactants and products are involved. For example, reaction equation for self-ionization is as follows.

$H_{2}O \rightleftharpoons H^{+} + OH^{-}$

This reaction is a chemical equilibrium. Also, nitrogen dioxide when present in equilibrium with nitrogen tetraoxide represents chemical equilibrium.

$2NO_{2} \rightleftarrow N_{2}O_{4}$

On the other hand, in a physical equilibrium same substance is present in different physical states. For example, when ice is present in equilibrium with water then it shows physical equilibrium.

$H_{2}O(s) \rightleftharpoons H_{2}O(l)$

And, liquid water present in equilibrium with water vapor also represents physical equilibrium.

$H_{2}O(l) \rightleftarrow H_{2}O(g)$

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Cecil writes the equation for the reaction of hydrogen and oxygen below.

Wittaler [7]

Answer:

C) to show that atoms are conserved in chemical reactions

Explanation:

When writing a chemical reaction, we should always consider the Mass Conservation Law, which basically states that; in an isolated system; the total mass should remain constant, this is, the total mass of the reactives should be equal to the total mass of the products

For this case, we should add the apporpiate coefficients in order to be in compliance with this law:

2H₂ + O₂ → 2H₂O

So, we can check the above statement:

For reactives (left side):

For product (right side):

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Read 2 more answers

Calculate the standard enthalpy change for the reaction at 25 ∘ 25 ∘ C. Standard enthalpy of formation values can be found in th

WINSTONCH [101]

<u>Answer:</u> The standard enthalpy change of the reaction is coming out to be -16.3 kJ

<u>Explanation:</u>

Enthalpy change is defined as the difference in enthalpies of all the product and the reactants each multiplied with their respective number of moles. It is represented as $\Delta H$

The equation used to calculate enthalpy change is of a reaction is:

$\Delta H_{rxn}=\sum [n\times \Delta H_f(product)]-\sum [n\times \Delta H_f(reactant)]$

For the given chemical reaction:

$Mg(OH)_2(s)+2HCl(g)\rightarrow MgCl_2(s)+2H_2O(g)$

The equation for the enthalpy change of the above reaction is:

$\Delta H_{rxn}=[(1\times \Delta H_f_{(MgCl_2(s))})+(2\times \Delta H_f_{(H_2O(g))})]-[(1\times \Delta H_f_{(Mg(OH)_2(s))})+(2\times \Delta H_f_{(HCl(g))})]$

We are given:

$\Delta H_f_{(Mg(OH)_2(s))}=-924.5kJ/mol\\\Delta H_f_{(HCl(g))}=-92.30kJ/mol\\\Delta H_f_{(MgCl_2(s))}=-641.8kJ/mol\\\Delta H_f_{(H_2O(g))}=-241.8kJ/mol$