The balanced equation for formation of dihydrogen phosphate from Phosphoric acid in water should be explained. Concept Introduction: The law of conservation of mass states that no atoms can be created or destroyed in a chemical reaction , therefore, the number of atoms present in the reactants is equal to the number of atoms present in the products. Bronsted Acid: An acid donates (loses) H + ion. Bronsted Base: A base accepts (gains) H + ion.

Question

Using the conditions of spontaneity to deduce the signs of AH and AS Use the observations about each chemical reaction in the table below to decide the sign (positive or negative) of the reaction enthalpy AH and reaction entropy AS. Note: if you have not been given enough information to decide a sign, select the "unknown" option. reaction observations conclusions A This reaction is always spontaneous, but proceeds slower at temperatures above 120. °C. ΔΗ is (pick one) AS is (pick one) ΔΗ is (pick one) B This reaction is spontaneous except above 117. °C. AS is (pick one) ΔΗ is (pick one) This reaction is slower below 20. °C than C above. AS is |(pick one) ? 18 Ar 1

Answer 1

Question

Chapter 3.6, Problem 3.5CYU

(a)

Interpretation Introduction

Interpretation:

The balanced equation for formation of dihydrogen phosphate from Phosphoric acid in water should be explained.

Concept Introduction:

The law of conservation of mass states that no atoms can be created or destroyed in a chemical reaction, therefore, the number of atoms present in the reactants is equal to the number of atoms present in the products.

Bronsted Acid: An acid donates (loses)H+ ion.

Bronsted Base: A base accepts (gains)H+ ion.

(b)

Interpretation Introduction

Interpretation:

The net ionic equation for the ionization of dihydrogen phosphate in water and the nature of the dihydrogen phosphate should be explained.

Concept Introduction:

The law of conservation of mass states that no atoms can be created or destroyed in a chemical reaction, therefore, the number of atoms present in the reactants is equal to the number of atoms present in the products.

Bronsted acid: An acid donates (loses) H+ ion.

Bronsted Base: A base accepts (gains) H+ ion.

Amphiprotic substance: An amphiprotic substance is a substance that can donate or accept a proton.

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