1answer.
Ask question
Login Signup
Ask question
All categories
  • English
  • Mathematics
  • Social Studies
  • Business
  • History
  • Health
  • Geography
  • Biology
  • Physics
  • Chemistry
  • Computers and Technology
  • Arts
  • World Languages
  • Spanish
  • French
  • German
  • Advanced Placement (AP)
  • SAT
  • Medicine
  • Law
  • Engineering
just olya [345]
4 years ago
9

Use bond energies to calculate δhrxn for the reaction. n2(g)+3cl2(g)→2ncl3(g)

Chemistry
2 answers:
Jobisdone [24]4 years ago
3 0
ΔHrxn = ΣδΗ(bond breaking) - ΣδΗ(bond making)

Bond enthalpies,
N ≡ N ⇒ 945 kJ mol⁻¹
N - Cl ⇒ 192 kJ mol⁻¹
Cl - Cl⇒ 242 kJ mol⁻¹

According to the balanced equation,
ΣδΗ(bond breaking)  = N ≡ N x 1 + Cl - Cl x 3
                                  = 945 + 3(242)
                                  = 1671 kJ mol⁻¹
ΣδΗ(bond making)    = N - Cl x 3 x 2
                                 = 192 x 6
                                 = 1152 kJ mol⁻¹

δHrxn = ΣδΗ(bond breaking) - ΣδΗ(bond making)
          = 1671 kJ mol⁻¹ - 1152 kJ mol⁻¹
          = 519 kJ mol⁻¹
Anna [14]4 years ago
3 0

The value of \Delta {H_{{\text{reaction}}}} of the reaction {{\text{N}}_{\text{2}}}\left( g \right) + 3{\text{C}}{{\text{l}}_2}\left( g \right) \to 2{\text{NC}}{{\text{l}}_3}\left( g \right) is \boxed{519\;{\text{kJ/mol}}}.

Further explanation:

Heat of reaction:

The heat released or absorbed in a chemical reaction due to the difference in the bond energies (BE) of reactants and products in the reaction is known as the heat of reaction. It is represented by\Delta {H_{{\text{reaction}}}}.

The heat of reaction \left( {\Delta {H_{{\text{reaction}}}}} \right)can have two values:

Case I: If the reaction is endothermic, more energy needs to be supplied to the system than that released by it. So \Delta {H_{{\text{reaction}}}} comes out to be positive.

Case II: If the reaction is exothermic, more energy is released by the system than that supplied to it. So \Delta {H_{{\text{reaction}}}} comes out to be negative.

The formula to calculate the heat of reaction is,

\boxed{\Delta {H_{{\text{reaction}}}} = \sum {\text{B}}{{\text{E}}_{{\text{reactant bond broken}}}} - \sum {\text{B}}{{\text{E}}_{{\text{product bond formed}}}}}

Here,

\Delta {H_{{\text{reaction}}}} is the heat of reaction.

{\text{B}}{{\text{E}}_{{\text{product bond formed}}}} is the bond energy of bond formation in products.

{\text{B}}{{\text{E}}_{{\text{reactant bond broken}}}} is the bond energy of bond breakage in reactants.

The given reaction occurs as follows:

{{\text{N}}_{\text{2}}}\left( g \right) + 3{\text{C}}{{\text{l}}_2}\left( g \right) \to 2{\text{NC}}{{\text{l}}_3}\left( g \right)

The number of broken bonds is 1 N-N triple bond and 3 Cl-Cl bonds.

The number of bonds formed is 6 N-Cl bonds.

The formula to calculate the enthalpy of the given reaction is as follows:

\Delta {H_{{\text{reaction}}}} = \left[ {\left( {1{\text{B}}{{\text{E}}_{{\text{N}} - {\text{N}}}} + 3{\text{B}}{{\text{E}}_{{\text{Cl}} - {\text{Cl}}}}} \right) - \left( {{\text{6B}}{{\text{E}}_{{\text{N}} - {\text{Cl}}}}} \right)} \right]                   …… (1)

The bond energy of N-N triple bond is 945 kJ/mol.

The bond energy of N-Cl bond is 192 kJ/mol.

The bond energy of Cl-Cl bond is 242 kJ/mol.

Substitute 945 kJ/mol for{\text{B}}{{\text{E}}_{{\text{N}} - {\text{N}}}}, 192 kJ/mol for{\text{B}}{{\text{E}}_{{\text{N}} - {\text{Cl}}}}, 242 kJ/mol for{\text{B}}{{\text{E}}_{{\text{Cl}} - {\text{Cl}}}}, in equation (1).

\Delta {H_{{\text{reaction}}}}&=\left[ {\left( {\left( {{\text{1 mol}}} \right)\left( {945\;{\text{kJ/mol}}} \right) + \left( {{\text{3 mol}}} \right)\left( {242\;{\text{kJ/mol}}} \right)} \right) - \left( {{\text{6 mol}}} \right)\left( {192\;{\text{kJ/mol}}} \right)} \right]\\\begin{aligned}&=\left[{\left({94{\text{5 kJ/mol}} + 72{\text{6 kJ/mol}}} \right) - 115{\text{2 kJ/mol}}} \right]\\&=\left[{167{\text{1 kJ/mol}} - 115{\text{2 kJ/mol}}} \right] \\ \end{aligned}

Learn more:

1. Calculate the enthalpy change using Hess’s Law: brainly.com/question/11293201

2. Find the enthalpy of decomposition of 1 mole of MgO: brainly.com/question/2416245

Answer details:

Grade: Senior School

Subject: Chemistry

Chapter: Thermodynamics

Keywords: N2, Cl2, NCl3, bond energies, N-Cl bond, N-N bond, Cl-Cl bond, 519 kJ/mol, heat of reaction, released, absorbed, exothermic, endothermic, positive, negative.

You might be interested in
The atomic number of aluminum is 13. What is the correct designation of the electron configuration of aluminum?.
Svetlanka [38]

Answer:

Its 1s22s22p63s23p1 ik it looks a lil goofy but i think its right

Explanation:

3 0
1 year ago
Umm im looking to practice for my quiz and I cant check if my answers are correct can someone tell me the correct answer
DerKrebs [107]
C should be the correct answer dd
4 0
3 years ago
You are testing an unknown liquid to determine its identity. First you heat the liquid and find that it turns to gas at 80 degre
SVETLANKA909090 [29]

Answer: The answer is <u><em>(Boiling Point) </em></u>:)

<u><em /></u>

7 0
3 years ago
What types of elements are usually found in meteorites
riadik2000 [5.3K]
Nickel,Iron,and metal hoped it helped -Krystin
8 0
3 years ago
Read 2 more answers
How many grams of O2 are formed from 13.34 moles of KClO3? Provide your final answer rounded to two decimal places.
trasher [3.6K]

Answer:

640.32 g

Explanation:

2KClO₃ → 2KCl + 3O₂

First we <u>convert KClO₃ moles to O₂ moles,</u> using the <em>stoichiometric coefficients</em>:

  • 13.34 mol KClO₃ * \frac{3molO_{2}}{2molKClO_{3}} = 20.01 mol O₂

Then we <u>convert O₂ moles to grams</u>, using its <em>molar mass</em>:

  • 20.01 mol O₂ * 32 g/mol = 640.32 g

So 640.32 g of O₂ are formed from 13.34 moles of KClO₃.

5 0
3 years ago
Other questions:
  • Scientists believe that ancient bacteria represents the first evidence of life on Earth. Which of these best describes the proce
    9·1 answer
  • If 4.0 mol aluminum and 7.0 mol hydrogen bromide react according to the following equation, how many moles of hydrogen are forme
    15·1 answer
  • Determain the number of moles in 2.24l of ch4 at stp
    12·1 answer
  • Which of the following statements is true?
    13·1 answer
  • How many mol of C3H8 are consumed when 3 mol of CO2 are produced ?
    10·1 answer
  • How many moles are in 11.5 L of a gas at STP?
    6·1 answer
  • What is the structure for a-d glucose
    13·1 answer
  • For each of the following compounds, decide whether the compound's solubility in aqueous solution changes with pH. If the solubi
    6·1 answer
  • Hellppppp
    7·1 answer
  • What is the relative rate of diffusion of hydrogen and nitrogen ​
    9·1 answer
Add answer
Login
Not registered? Fast signup
Signup
Login Signup
Ask question!