C3H8 (g) +502(g) → 3CO2 (g) +4H₂O(g) AHxn=-2044 kJ Spontaneous at all temperatures 2N2(g) + O2(g) →2N₂O(g) AHxn= +163.2 kJ Spontaneous at high temperatures 4NH3(g) + 502(g) → 4NO(g) + 6H₂O(g) AHxn-906 kJ Spontaneous at low temperatures Nonspontaneous at all temperatures

C3H8 (g) +502(g) → 3CO2 (g) +4H₂O(g) AHxn=-2044 kJ Spontaneous at all temperatures 2N2(g) + O2(g) →2N₂O(g) AHxn= +163.2 kJ Spontaneous at high temperatures 4NH3(g) + 502(g) → 4NO(g) + 6H₂O(g) AHxn-906 kJ Spontaneous at low temperatures Nonspontaneous at all temperatures

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: Determine ΔH for the third reaction from the information given. 1/2 N2(g) + O2(g) ↔ NO2(g) ΔH =…

A: The two reactions given are, 1) 1/2 N2 (g) + O2 (g) ↔ NO2 (g) ΔH = 33.85 KJ2) N2 (g)…

Q: Given the thermal chemical reactions below Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g) ∆H°= −26.7 kJ…

A: Enthalpy measures the heat content of a system. If change of enthalpy is positive then the reaction…

Q: Consider the following thermochemical data to: 2CO2(g) → 2 C (s, graphite) + 2 O2 (g) H2 (g) +…

A: Given Equation No Reaction. ∆H°(kJ/mol) A 2CO2 (g) → 2 C (s, graphite)…

Q: Determine ΔrH° in kJ/mol for the reaction, 4 NO(g) + 6 H2O(g) →4 NH3(g) + 5 O2(g) using the…

Q: Consider the reaction N2(g)+3H2(g)→2NH3(g),N2(g)+3H2(g)→2NH3(g), ΔHΔH =−92.3kJ mol−1=−92.3kJ mol−1…

Q: Calculate ΔH° for the combustion of methane. CH4 (g) + 2 O2 (g) → CO2 (g) + 2 H2O (g) Given the…

A: We have to calculate the ∆H° for Reaction.

Q: Given the following combustion data for three different fuels: CH4 (g), C8H18 (l) and CH3OH (l), CH4…

A: The ratio of energy to the molar mass is known as energy density.

Q: THERMODYNAMICS: Use the given standard enthalpies of formation to calculate the ΔHo (in kJ) for the…

A: Concept is based on Hesses law:

Q: Using the equations Ca(s) + 1/2 O₂ (g) → CaO (s) ∆H° = -450 kJ/mol CO₂ (g) → C (s) + O₂ (g) ∆H° =…

A: The given equation are Ca(s) + 1/2 O₂ (g) → CaO (s) ∆H° = -450 kJ/mol ......…

Q: Determine

A: We will calculate ∆H rxn by doing operation in giving equation

Q: Calculate the standard enthalpy of the reaction for the process 3RO(g) → R20(g) + RO2(g) using the…

Q: THERMODYNAMICS: Use the given standard enthalpies of formation to calculate the ΔHo (in kJ) for the…

A: The standard enthalpy of a reaction is determined from the difference between the molar enthalpies…

Q: Given the following enthalpy change values for the reactions below: A + B → 2C ; ΔrH = 169.9 kJ…

A: Given thermochemical equations are A + B → 2C ; ΔrH = 169.9 kJ mol-1 ------ (i) C + 2D → E + F ;…

Q: Calculate ΔHrxn for the following reaction: CaO(s)+CO2(g)→CaCO3(s) Use the following reactions and…

A: "Hess law" helps in the evaluation of enthalpy change (Delta H) for any specific reaction. When the…

Q: Calculate the reaction enthalpy change at 1450 K for the reaction: 1/2 H2 (g) + Cl2 (g) → HCl (g)…

A: The objective of the question is to determine the enthalpy change for the given reaction.

Q: Using the equations 2 Sr(s) + O₂ (g) → 2 SrO (s) ∆H° = -1184 kJ/mol CO₂ (g) → C (s) + O₂ (g) ∆H° =…

A: Given:

Q: THERMODYNAMICS: Use the given standard enthalpies of formation to calculate the ΔHo (in kJ) for the…

Q: hat is ΔHof of Al2S3(s)? 2Al2S3(s) + 9O2(g) → 2Al2O3(s) + 6SO2(g) ΔHo = -3684.2 kJ ΔHof…

A: The reaction : 2Al2S3(s) + 9O2(g) → 2Al2O3(s) + 6SO2(g) ΔHo = -3684.2 kJ ΔHof Al2O3(s) =…

Q: Calculate the ΔH for the reaction: Na2O (s) + SO3 (g) --> Na2SO4 (g) ΔH

A: Target equation :- Na2O (s) + SO3 (g) --> Na2SO4 (g)…

Q: Determine ΔrH° in kJ/mol for the reaction, 4 NO(g) + 6 H2O(g) →4 NH3(g) + 5 O2(g) using the…

Q: Given the following combustion data for three different fuels: CH4 (g), C8H18 (l) and CH3OH (l),…

A: For fuel CH4 energy per gram is CH4 (g) + 2 O2 (g) → CO2 (g) + 2 H2O (l) ΔH° = −890 kJenergy per…

Q: Given the following enthalpy change values for the reactions below: A + B → 2C ; ΔrH = 305.5 kJ…

A: According to the Hess's law we know that when a chemical equation is written as the sum of overall…

Q: The enthalpy change for the following reaction is -36.2 kJ 2A(s) + B(g) → C(g) Determine the ΔH…

A: Answer:- This question is answered by using the simple concept of Hess law of constant heat…

Q: Use the given standard enthalpies of formation to calculate the ΔHo (in kJ) for the hypothetical…

Q: The Enthalpy of Vaporization of 1-chlorobutane, C4H9Cl, is 30.4 kJ/mol at a boiling point of 78.6…

Q: Consider the reactions 2 K2O(s) + O2(g) → 2 K2O2(s) ΔH = -265 kJ 8 KO2(s) → 4 K2O(s) + 6 O2(g) ΔH =…

A: The enthalpy of any reaction is an additive property. So if the enthalpy of two or more reaction is…

Q: Given the standard enthalpy changes for the following two reactions: (1) 2Pb(s) + 02(g)→2P60(s) AH°…

A: We have to calculate the standard enthalpy change for the reaction PbO(s) + Zn(s) → Pb(s) + ZnO(s).

Q: etermine the enthalpy for the reaction shown below. CS2(l) + 3O2(g) --> CO2(g) + 2SO2(g)…

Q: Determine the enthalpy of reaction for HCI(g) + NaNO2(s) -> HNO2 (l) + NaCl(s) 2NaCl(s) + H2O(l) →…

A: Given data 2NaCl(s) + H2O(l) → 2HCI(g) + Na2O(s); ∆H ° =-507.1 kJ/mol NO(g) + NO2(g) + Na2O(s)→…

Q: Using the equations 2 Sr(s) + O₂ (g) → 2 SrO (s) ∆H° = -1184 kJ/mol SrO (s) + CO₂ (g) → SrCO₃ (s)…

A: The given reactions given are as follows: The required equation is:

Q: Use the following information to calculate the standard enthalpy of formation of NO>(g) at 298 K?…

Q: Calculate total work done (in Joules) when 50 g of iron is dissolved in HCl in an open beaker at…

Q: Determine the enthalpy for the reaction shown below. CS2(l) + 3O2(g) --> CO2(g) + 2SO2(g)…

A: In this question, we have to find out the correct answer of given problem by the help of…

Q: -393.5 kJ mol AH°rxn = -285.8 kJ mol AH°rxn = - 3119.6 kJ mol" AH°rxn C(graphite) + O:(g)→CO2(g)…

Q: Using the following thermochemical data: 2Sb(s) + 6HF(g) → 2SbF3(s) + 3H2(g) ΔH° =…

Question

Part C
In addition, predict under what temperatures (all temperatures, low temperatures, or high temperatures), if any, the reaction is spontaneous.
Drag the appropriate items to their respective bins.
Submit
C3H8 (g) + 50₂(g) →
3CO2 (g) + 4H₂O(g)
AHxn=-2044 kJ
Spontaneous at all
temperatures
2N₂(g) + O₂(g) →2N₂O(g)
AHxn = +163.2 kJ
Spontaneous at high
temperatures
Previous Answers Request Answer
4NH3 (g) +502(g) →
4NO(g) + 6H₂O(g)
AHixn = -906 kJ
Spontaneous at low
temperatures
Reset Help
Nonspontaneous at all
temperatures

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1: Criterion to decide spontaneity of the reaction!

VIEW

Step 2: Checking the spontaneity of combustion reaction of propane

VIEW

Step 3: Checking the spontaneity of nitrous oxide formation

VIEW

Step 4: Checking the spontaneity of combustion reaction of ammonia

VIEW

Solution

VIEW

Step by step

Solved in 5 steps with 6 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Calculate the standard enthalpy of formation of CO2 from the following data: C(s, graphite) + ½ O2(g) → CO(g) ∆H°25°C = –110.5 kJ CO2(g) + C(s, graphite) → 2 CO(g)∆H°25°C = 172.5 kJ
56
Consider the following thermochemical data: Cl2(g) → 2Cl(g) ΔH° = 242.3 kJ I2(g) → 2l(g) ΔH° = 151.0 kJ ICl(g) → l(g) + Cl(g) ΔH° = 211.3 kJ I2(s) → I2(g) ΔH° = 62.8 kJ Calculate ΔH° for the following reaction: ½I2(s) + ½Cl2(g) → ICl(g)
Using the equations H₂ (g) + F₂ (g) → 2 HF (g) ∆H° = -79.2 kJ/mol C (s) + 2 F₂ (g) → CF₄ (g) ∆H° = 141.3 kJ/mol Determine the enthalpy for the reaction C (s) + 4 HF (g) → CF₄ (g) + 2 H₂ (g).
Given the following Fe,03 (s) + 3 CO (g) →2 Fe (s) + 3 CO2 (g) AG' = - 29.4 kJ 3 Fe203 (s) + Co (g) →2 Fez04 (s) + CO, (g) AG° = -61.6 kJ Calculate AG° for Fez04 (s) + CO (g) → Fe (s) + Fe,03 (s) + CO2 (g)
THERMODYNAMICS: Use the given standard enthalpies of formation to calculate the ΔHo (in kJ) for the hypothetical reaction: (Round off the final answer to ONE decimal place. Do not include the unit.) 2X2D (g) + 3M2 (g) → 2X2M (l) + 2DM2 (g) ΔHof for X2D (g) = -22.4 kJ/mol ΔHof for DM2 (g) = -290.7 kJ/mol ΔHof for X2M (l) = -288.3 kJ/mol ΔHof for M2 (g) = 0 kJ/mol show sol'n please.
Given the data below, H°, for the reaction rxn 3C12 (g) + PH3 (g) → PCI3 (g) + 3HCI (g) is kJ. AH° (PCI3 (g) = -288.07 kJ/mol AH°F (HCI (g)) = -92.30 kJ/mol AH°r (PH3 (g)) = 5.40 kJ/mol 570.37 O The AH°, of Cl2 (g) is needed for the calculation. -385.77 385.77 -570.37
How much heat must be removed from a 90.5 g sample of benzene (M = 78.11 g mol-1) to cool the sample from 305 K to 215 K? The following physical data may be useful.ΔfusH = 9.8 kJ mol-1ΔvapH = 30.8 kJ mol-1Cs(l) = 1.73 J g-1 K-1Cs(s) = 1.51 J g-1 K-1Cs(g) = 82.4 J g-1 K-1 Tm = 279.0 KTb = 353.3 K Note: The word 'removed' in the question already accounts for the negative sign involved in the heat transfer. Express your answer to three significant figures.
Calculate ΔHo for the process ½ N2(g) + ½ O2(g) → NO(g) from the following information N2(g) + 2 O2(g) → 2 NO2(g) ΔHo = -105.8 kJ/mol 2 NO(g) + O2 → 2 NO2(g) ΔHo = -216.7 kJ/mol
Hess's Law Given the following data: 4C(s) + 3H2(g) + 1/2O2(g) → HCOC(CH2)(CH3)(l) ΔH°=-139.0 kJ CH3CH2OH(l) + 1/2O2(g) → CH3CHO(l) + H2O(l) ΔH°=-204.0 kJ 2C(s) + 3H2(g) + 1/2O2(g) → CH3CH2OH(l) ΔH°=-278.0 kJ H2(g) + 1/2O2(g) → H2O(l) ΔH°=-286.0 kJ calculate ΔH° for the reaction:2CH3CHO(l) → HCOC(CH2)(CH3)(l) + H2O(l)
Consider the reaction: 8 H2O (l) + 4CO2 (g)→4 CH3OH (l) + 6 O2 (g) ΔH = +2905.6 kJ What is ΔH for the following reaction? 2 CH3OH (l) + 3 O2 (g) →4 H2O (l) + 2 CO2 (g)