Hydrazine (N2H4) is a fuel used by some spacecraft. It is normally oxidized by N2O4according to this equation: N2H4(...
Hydrazine (N2H4) is a fuel used by some spacecraft. It is normally oxidized by N2O4according to this equation:
N2H4(l)+N2O4(g)→2N2O(g)+2H2O(g)
Standard Enthalpies of Formation at 25 ∘C
| Substance | ΔH∘f(kJ/mol) |
| N2H4(l) | 50.6 |
| N2H4(g) | 95.4 |
| N2O(g) | 81.6 |
| N2O4(l) | −19.5 |
| N2O4(g) | 9.16 |
| H2O(l) | −285.8 |
| H2O(g) | −241.8 |
Calculate ΔH∘rxn for this reaction using standard enthalpies of formation.
Express your answer using one decimal place.
Homework Answers
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Hydrazine (N2H4) is a fuel used by some spacecraft. It is normally oxidized by N2O4according to this equation: N2H4(...
Hydrazine (N2H4) is a fuel used by some spacecraft. It is normally oxidized by N2O4 according to the following equation...
Hydrazine (N2H4) is a fuel used by some spacecraft. It is normally oxidized by N2O4 according to the following equation:N2H4(l)+N2O4(g)->2N2O(g)+2H2O(g)Calculate delta Hrxn for this reaction using standard enthalpies of formation.I am having trouble finding the standard enthalpies of all of the reactants and products
A fuel mixture used in the early days of rocketry consisted of two liquids, hydrazine (N2H4)...
A fuel mixture used in the early days of rocketry consisted of two liquids, hydrazine (N2H4) and dinitrogen tetroxide (N2O4) which ignite on contact to form nitrogen gas and water vapor. How many grams of nitrogen gas form when 1.00 x 10^2 g of N2H4 and 2.00 x 10^2 g of N2O4 are mixed? So, I tried solving this but not sure what they mean by "mixed". The balanced chemical equation is: 2 N2H4 + N2O4 = 3 N2 +...
Standard Enthalpies of Formation, in kJ/mol N2(g) 0 NO2(g) +33.2 &nbs
Standard Enthalpies of Formation, in kJ/mol N2(g) 0 NO2(g) +33.2 NH3(g) -45.9 H2O(l) -285.8 NO(g) +90.3 N2O(g) -82.1 H2O(g) -241.8 Use the data above to calculate ΔH for the reaction: 6 NO2(g) + 8 NH3(g) => 7 N2(g) + 12 H2O(g) ΔH = ?
1. Hydrazine is used to remove dissolved oxygen from the water in water heating systems. N2H4(l) + O2(g) à 2H2O(l) + N2(g) What is the free energy changed observed when 1.00...
1. Hydrazine is used to remove dissolved oxygen from the water in water heating systems. N2H4(l) + O2(g) à 2H2O(l) + N2(g) What is the free energy changed observed when 1.00 mole of N2H4 is oxidized? (for hydrazine ∆G°f = 149.2 kJ/mol) What is the free energy change for the oxidation of 1.00 pound (454 g) of hydrazine? 2. Calculate the standard free energy change and equilibrium constant for the following reaction at 25 °C. 4Ag(aq) + O2(g) + 4H+(aq)...
1).From the standard enthalpies of formation, calculate ΔH°rxn for the reaction C6H12(l) + 9O2(g) → 6CO2(g)...
1).From the standard enthalpies of formation, calculate ΔH°rxn for the reaction C6H12(l) + 9O2(g) → 6CO2(g) + 6H2O(l) For C6H12(l), ΔH°f = –151.9 kJ/mol (5 points) Substance ∆H°f , kJ/mol C6H12(l) –151.9 O2(g) 0 H2O(l) –285.8 CO2(g) –393.5 2).Determine the amount of heat (in kJ) given off when 1.26 × 104 g of ammonia are produced according to the equation N2(g) + 3H2(g) → 2NH3(g) ΔH°= –92.6 kJ/mol Assume that the reaction takes place under standard conditions at 25oC.
(6 pts.) Using Hess’s Law and the values for Standard Enthalpies of Formation from the table...
(6 pts.) Using Hess’s Law and the values for Standard Enthalpies of Formation from the table provided, calculate the enthalpy of reaction ΔH°rxn (in kJ) for each of the following reactions: Standard Enthalpies of Formation substance ΔHf° in kJ/mol Mg(s) 0 MgO(s) -601.6 HCl(aq) -167.2 MgCl2(aq) -801.2 H2(g) 0 H2O(l) -285.8 Reaction #1: Mg (s) + 2HCl (aq) è MgCl2 (aq) + H2 (g) Reaction #2: MgO (s) + 2HCl (aq) è MgCl2 (aq) + H2O (l) 2. (4 pts.)...
TABLE 7.2 Some Standard Molar Enthalpies of Fa AcHº at 298.15 K Substance kJ/mola Substance CO(g) CO2(g) CH4(g) C2H2(g)...
TABLE 7.2 Some Standard Molar Enthalpies of Fa AcHº at 298.15 K Substance kJ/mola Substance CO(g) CO2(g) CH4(g) C2H2(g) C2H4(g) C2H6(g) C3H8(g) C4H10(g) CH3OH(1) C2H5OH(1) HF(g) HCl(g) -110.5 -393.5 - 74.81 226.7 52.26 -84.68 - 103.8 – 125.6 –238.7 –277.7 -271.1 -92.31 HBr(g) HI(g) H2O(g) H2O(1) H2S(g) NH3(g) NO(g) N2O(g) NO2(g) N204(8) SO2(g) SO3(g) aValues are for reactions in which one mole of substance is formed. M been rounded off to four significant figures. (Reference to Equation 7.22): A Hº...
avuuuw ac mallianned at 25 L and I bar. 86. Use data from Table 7.2, together...
avuuuw ac mallianned at 25 L and I bar. 86. Use data from Table 7.2, together with the fact that AHº = -3509 kJ mol-1 for the complete combustion of pentane, C5H12(1), to calculate A Hº for the reac- tion below. 5 CO(g) + 11 H2(g) → C5H12(1) + 5 H2O(1) ApHº = ? TABLE 7.2 Some Standard Molar Enthalpies of Formation, AHº at 298.15 K du Substance kJ/mola Substance kJ/mola CO(g) -110.5 HBr(g) -36.40 CO2(g) -393.5 HI(g) 26.48 CH_(8)...
Methanol (CH3OH) is used as a fuel in race cars. Part A Write a balanced equation...
Methanol (CH3OH) is used as a fuel in race cars. Part A Write a balanced equation for the combustion of liquid methanol in air, assuming H2O(g) as a product. Express your answer as a chemical equation. Identify all of the phases in your answer. SubmitPrevious AnswersRequest Answer Incorrect; Try Again; 5 attempts remaining Part B Calculate the standard enthalpy change for the combustion of 1 mol of liquid methanol, assuming H2O(g) as a product. Express your answer using four significant...
Thermodynamic properties of pure substances Standard thermodynamic quantities for selected substances at 25 ° C listed...
Thermodynamic properties of pure
substances
Standard thermodynamic quantities for selected substances at 25
°
C listed alphabetically by most important atom.
substance
Δ
Hf
°
(kJ/mol)
Δ
Gf
°
(kJ/mol)
S
°
(J/mol∙K)
Aluminum
Al3+ (aq)
---
-485.0
---
Al (s)
0
0
28.3
Al2O3 (s)
-1675.7
-1582.3
50.9
Al(OH)3 (s)
---
-1147.25
---
Bromine
Br− (aq)
---
-104.0
---
Br2 (l)
0
0
152.2
Br2 (g)
30.9
3.1
245.5
HBr (g)
-36.3
-53.4
198.7
Calcium
Ca2+ (aq)
---
-553.6...
TABLE 7.2 Some Standard Molar Enthalpies of Fa AcHº at 298.15 K Substance kJ/mola Substance CO(g) CO2(g) CH4(g) C2H2(g) C2H4(g) C2H6(g) C3H8(g) C4H10(g) CH3OH(1) C2H5OH(1) HF(g) HCl(g) -110.5 -393.5 - 74.81 226.7 52.26 -84.68 - 103.8 – 125.6 –238.7 –277.7 -271.1 -92.31 HBr(g) HI(g) H2O(g) H2O(1) H2S(g) NH3(g) NO(g) N2O(g) NO2(g) N204(8) SO2(g) SO3(g) aValues are for reactions in which one mole of substance is formed. M been rounded off to four significant figures. (Reference to Equation 7.22): A Hº...
avuuuw ac mallianned at 25 L and I bar. 86. Use data from Table 7.2, together with the fact that AHº = -3509 kJ mol-1 for the complete combustion of pentane, C5H12(1), to calculate A Hº for the reac- tion below. 5 CO(g) + 11 H2(g) → C5H12(1) + 5 H2O(1) ApHº = ? TABLE 7.2 Some Standard Molar Enthalpies of Formation, AHº at 298.15 K du Substance kJ/mola Substance kJ/mola CO(g) -110.5 HBr(g) -36.40 CO2(g) -393.5 HI(g) 26.48 CH_(8)...
Thermodynamic properties of pure
substances
Standard thermodynamic quantities for selected substances at 25
°
C listed alphabetically by most important atom.
substance
Δ
Hf
°
(kJ/mol)
Δ
Gf
°
(kJ/mol)
S
°
(J/mol∙K)
Aluminum
Al3+ (aq)
---
-485.0
---
Al (s)
0
0
28.3
Al2O3 (s)
-1675.7
-1582.3
50.9
Al(OH)3 (s)
---
-1147.25
---
Bromine
Br− (aq)
---
-104.0
---
Br2 (l)
0
0
152.2
Br2 (g)
30.9
3.1
245.5
HBr (g)
-36.3
-53.4
198.7
Calcium
Ca2+ (aq)
---
-553.6...
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