Hydrazine (N 2 H 4 ) is used as a fuel in liquid-fueled rockets. When hydrazine reacts with oxygen gas, nitrogen gas and water vapor are produced. Write a balanced equation and use bond energies from Table 3-3 to estimate ∆ H for this reaction.

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Interpretation Introduction Interpretation: The balanced equation for the reaction of hydrazine with oxygen is to be stated. The value of Δ H ° for this reaction is to be calculated using the bond energies from Table 3-3 . Concept introduction: The expression to calculate the value of Δ H ° is, Δ H ° = ∑ n p D ° ( bonds broken ) − ∑ n r D ° ( bonds formed ) To determine: The balanced equation for the reaction of hydrazine with oxygen; the value of Δ H ° for this reaction is to be calculated using the bond energies from Table 3-3 . Explanation The balanced reaction is, N 2 H 4 ( l ) + O 2 ( g ) → N 2 ( g ) + 2 H 2 O ( g ) Reaction between hydrazine ( N 2 H 4 ) with oxygen ( O 2 ) yields nitrogen gas ( N 2 ) and water ( H 2 O ) . The balanced reaction is, N 2 H 4 ( l ) + O 2 ( g ) → N 2 ( g ) + 2 H 2 O ( g ) The required value of Δ H ° for the given reaction is 5 9 0 k J _ . Refer to Table 3-3 . The value of bond energy, D ° ( kJ/mol ) , for the given reactant and product is, Bonds D ° ( kJ/mol ) N − H 391 N − N 160 N ≡ N 941 O − H 467 O = O 495 The formula of Δ H ° is, Δ H ° = ∑ n p D ° ( bonds broken ) − ∑ n r D ° ( bonds formed ) Where, n p is the number of moles of each product

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Chemistry: An Atoms First Approach

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Chemistry: An Atoms First Approach

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Steven S. Zumdahl + 1 other

Publisher: Cengage Learning

ISBN: 9781305079243

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Interpretation Introduction

Interpretation: The balanced equation for the reaction of hydrazine with oxygen is to be stated. The value of ΔH° for this reaction is to be calculated using the bond energies from Table 3-3 .

Concept introduction: The expression to calculate the value of ΔH° is,

ΔH°=∑npD°(bonds broken)−∑nrD°(bonds formed)

To determine: The balanced equation for the reaction of hydrazine with oxygen; the value of ΔH° for this reaction is to be calculated using the bond energies from Table 3-3 .

Explanation of Solution

The balanced reaction is,

N2H4(l)+O2(g)→N2(g)+2H2O(g)

Reaction between hydrazine (N2H4) with oxygen (O2) yields nitrogen gas (N2) and water (H2O) . The balanced reaction is,

N2H4(l)+O2(g)→N2(g)+2H2O(g)

The required value of ΔH° for the given reaction is 590 kJ_ .

Refer to Table 3-3 .

The value of bond energy, D°(kJ/mol) , for the given reactant and product is,

Bonds	D°(kJ/mol)
N−H	391
N−N	160
N≡N	941
O−H	467
O=O	495

The formula of ΔH° is,

ΔH°=∑npD°(bonds broken)−∑nrD°(bonds formed)

Where,

np is the number of moles of each product

Hydrazine (N 2 H 4 ) is used as a fuel in liquid-fueled rockets. When hydrazine reacts with oxygen gas, nitrogen gas and water vapor are produced. Write a balanced equation and use bond energies from Table 3-3 to estimate ∆ H for this reaction.

Chemistry: An Atoms First Approach

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Chemistry: An Atoms First Approach

Hydrazine (N₂H₄) is used as a fuel in liquid-fueled rockets. When hydrazine reacts with oxygen gas, nitrogen gas and water vapor are produced. Write a balanced equation and use bond energies from Table 3-3 to estimate ∆H for this reaction.

Explanation of Solution

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Hydrazine (N 2 H 4 ) is used as a fuel in liquid-fueled rockets. When hydrazine reacts with oxygen gas, nitrogen gas and water vapor are produced. Write a balanced equation and use bond energies from Table 3-3 to estimate ∆ H for this reaction.

Chemistry: An Atoms First Approach

Solutions

Chemistry: An Atoms First Approach