Calculate ∆ H for the reaction 2 NH 3 ( g ) + 1 2 O 2 ( g ) → N 2 H 4 ( l ) + H 2 O ( l ) given the following data: 2 NH 3 ( g ) + 3 N 2 O ( g ) → 4 N 2 ( g ) + 3 H 2 O ( l ) Δ H = − 1010. KJ N 2 O ( g ) + 3 H 2 ( g ) → N 2 H 4 ( l ) + H 2 O ( l ) Δ H = − 317 KJ N 2 H 4 ( l ) + O 2 ( g ) → N 2 ( g ) + 2 H 2 O ( l ) Δ H = − 623 KJ H 2 ( g ) + 1 2 O 2 ( g ) → H 2 O ( l ) Δ H = − 286 K J

Q: Expert Answer

Interpretation Introduction Interpretation : The enthalpy change ΔH of given reaction has to be calculated and the feasibility of ammonia synthesis should be discussed. Concept Introduction: Hess's Law: The enthalpy change along with a chemical reaction is self-determining of the route by which the chemical reaction take place. The enthalpy change of a reaction is equal to were the reaction take place in a single step or multiple steps. Formula: ΔH ( total ) = ∑ ΔH ( number of steps ) ...... (1) Rules: The sign of enthalpy is inverted when the reaction is inverted. The amounts of reactants and products is straight comparative to the level of ΔH in a reaction. If the coefficients in a balanced reaction are multiplied by numeral, the ΔH value is multiplied by the similar numeral. Explanation Explanation To calculate: The enthalpy change ΔH 2NH 3 +3N 2 O → 4N 2 +H 2 O ΔH 1 = -1010 KJ ...... (1) 3N 2 H 4 +3H 2 O → 3N 2 O+9H 2 ΔH 2 = -3(-317 KJ) ...... (2) 9H 2 + 9 2 O 2 → 9H 2 O ΔH3 = 9(-286KJ) ...... (3) 4N 2 +8H 2 O → 4N 2 H 4 +4O 2 ΔH4 = -4(-623 KJ) ...... (4) Given: 2NH 3(g) +3N 2 O (g) → 4N 2(g) +3H 2 O (l) ΔH 1 =-1010KJ ...... (1) N 2 O (g) +3H 2(g) → N 2 H 4(l) +H 2 O (l) ΔH 2 = -317 KJ

Question

Still sussing out bartleby?

Answer 1

BuyFind

Chemistry: An Atoms First Approach

2nd Edition

Steven S. Zumdahl + 1 other

Publisher: Cengage Learning

ISBN: 9781305079243

Solutions

Chapter

Section

Answer 2

BuyFind

Chemistry: An Atoms First Approach

2nd Edition

Steven S. Zumdahl + 1 other

Publisher: Cengage Learning

ISBN: 9781305079243

Solutions

Chapter

Section

Answer 3

Solutions

Chapter

Section

Answer 4

Chapter

Section

Answer 5

Interpretation Introduction

Interpretation: The enthalpy change ΔH of given reaction has to be calculated and the feasibility of ammonia synthesis should be discussed.

Concept Introduction:

Hess's Law:

The enthalpy change along with a chemical reaction is self-determining of the route by which the chemical reaction take place.
The enthalpy change of a reaction is equal to were the reaction take place in a single step or multiple steps.

Formula:

ΔH(total)= ∑ΔH(number of steps)......(1)

Rules:

The sign of enthalpy is inverted when the reaction is inverted.
The amounts of reactants and products is straight comparative to the level of ΔH in a reaction. If the coefficients in a balanced reaction are multiplied by numeral, the ΔH value is multiplied by the similar numeral.

Explanation of Solution

Explanation

To calculate: The enthalpy change ΔH

2NH3+3N2O→4N2+H2O ΔH1 = -1010 KJ......(1)3N2H4+3H2O→3N2O+9H2 ΔH2 = -3(-317 KJ)......(2)9H2+92O2→9H2O ΔH3 = 9(-286KJ)......(3)4N2+8H2O→4N2H4+4O2 ΔH4 = -4(-623 KJ)......(4)

Given:

2NH3(g)+3N2O(g)→4N2(g)+3H2O(l) ΔH1 =-1010KJ......(1)N2O(g)+3H2(g)→N2H4(l)+H2O(l) ΔH2 = -317 KJ

Chemistry: An Atoms First Approach

Solutions

Chemistry: An Atoms First Approach

Explanation of Solution

Still sussing out bartleby?

The Solution to Your Study Problems

Chapter 7 Solutions

Additional Science Textbook Solutions