Question

Consider the oxidation of CO to CO2: CO(g)+12O2(g)→CO2(g) Reactant or product ΔH∘f(kJ/mol) S∘(J/mol⋅K) CO -110.5 197.7...

Consider the oxidation of CO to CO2:
CO(g)+12O2(g)→CO2(g)
Reactant or product ΔH∘f(kJ/mol) S∘(J/mol⋅K)
CO -110.5 197.7
O2 0 205.2
CO2 -393.5 213.8

Part A

Calculate ΔG∘rxn at 25∘C.

Express your answer to one decimal place with the appropriate units.
ΔG∘rxn =

SubmitMy AnswersGive Up

Incorrect; Try Again; 4 attempts remaining

Your answer does not have the correct dimensions.

Part B

Determine whether the reaction is spontaneous at standard conditions.

Determine whether the reaction is spontaneous at standard conditions.
spontaneous
nonspontaneous
Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Given the values of ΔH∘rxn, ΔS∘rxn, and T below, determine ΔSuniv. Part A ΔH∘rxn= 117 kJ...
Given the values of ΔH∘rxn, ΔS∘rxn, and T below, determine ΔSuniv. Part A ΔH∘rxn= 117 kJ , ΔS∘rxn=− 263 J/K , T= 291 K . ΔSuniv= −1.3•102 J/K SubmitMy AnswersGive Up Incorrect; Try Again; 3 attempts remaining Part B ΔH∘rxn=− 117 kJ , ΔS∘rxn= 263 J/K , T= 291 K . ΔSuniv= J/K SubmitMy AnswersGive Up Part C ΔH∘rxn=− 117 kJ , ΔS∘rxn=− 263 J/K , T= 291 K. ΔSuniv= J/K SubmitMy AnswersGive Up Part D ΔH∘rxn=− 117 kJ ,...
Given the values of ΔH∘rxn, ΔS∘rxn, and T below, determine ΔSuniv. Part A ΔH∘rxn= 115 kJ...
Given the values of ΔH∘rxn, ΔS∘rxn, and T below, determine ΔSuniv. Part A ΔH∘rxn= 115 kJ , ΔS∘rxn=− 263 J/K , T= 301 K . ΔSuniv= J/K SubmitMy AnswersGive Up Part B ΔH∘rxn=− 115 kJ , ΔS∘rxn= 263 J/K , T= 301 K . ΔSuniv= J/K SubmitMy AnswersGive Up Part C ΔH∘rxn=− 115 kJ , ΔS∘rxn=− 263 J/K , T= 301 K . ΔSuniv= J/K SubmitMy AnswersGive Up Part D ΔH∘rxn=− 115 kJ , ΔS∘rxn=− 263 J/K , T= 557...
Use Hess's law to determine ΔH∘ for the reaction CO(g)+12O2(g)→CO2(g), given that C(graphite)+12O2(g)→CO(g), ΔH∘=−110.54kJ/mol C(graphite)+O2(g)→CO2(g), ΔH∘=−393.51kJ/mol
Use Hess's law to determine ΔH∘ for the reaction CO(g)+12O2(g)→CO2(g), given that C(graphite)+12O2(g)→CO(g), ΔH∘=−110.54kJ/mol C(graphite)+O2(g)→CO2(g), ΔH∘=−393.51kJ/mol
Consider the following reaction: CaCO3(s)→CaO(s)+CO2(g). Estimate ΔG for this reaction at each of the following temperatures....
Consider the following reaction: CaCO3(s)→CaO(s)+CO2(g). Estimate ΔG for this reaction at each of the following temperatures. (Assume that ΔH∘ and ΔS∘ do not change too much within the given temperature range). Also determine whether the reactions in part 1 and 2 are spontaneous or nonspontaneous. 1).1095 K 2).1500K
Part A For which of the following reactions is ΔH∘rxn equal to ΔH∘f of the product(s)?...
Part A For which of the following reactions is ΔH∘rxn equal to ΔH∘f of the product(s)? You do not need to look up any values to answer this question. Check all that apply. Hints Check all that apply. S(s)+O2(g)→SO2(g) Li(s)+12F2(g)→LiF(s) SO(g)+12O2(g)→SO2(g) SO3(g)→12O2(g)+SO2(g) 2Li(s)+F2(g)→2LiF(s) Li(s)+12F2(l)→LiF(s) Part B The combustion of propane, C3H8, occurs via the reaction C3H8(g)+5O2(g)→3CO2(g)+4H2O(g) with heat of formation values given by the following table: Substance ΔH∘f (kJ/mol) C3H8 (g) -104.7 CO2(g) −393.5 H2O(g) −241.8 Calculate the enthalpy for...
Thermochemical Equations 07a (kJ) Consider the following thermochemical equation for the combustion of butane. 2C4H10(g)+15O2(g)→8CO2(g)+10H2O(g)ΔH∘rxn=−5314.6kJ Part...
Thermochemical Equations 07a (kJ) Consider the following thermochemical equation for the combustion of butane. 2C4H10(g)+15O2(g)→8CO2(g)+10H2O(g)ΔH∘rxn=−5314.6kJ Part A Calculate the heat associated with the consumption of 1.158 mol of O2 in this reaction. Use the correct sign for q q = +   kJ   SubmitMy AnswersGive Up Incorrect; Try Again; 6 attempts remaining Part B Calculate the heat associated with combustion of 29.46 g of butane. Use the correct sign for q q =   kJ   SubmitMy AnswersGive Up Part C Calculate the...
Consider the following reaction: CaCO3(s)→CaO(s)+CO2(g). Estimate ΔG∘ for this reaction at each of the following temperatures....
Consider the following reaction: CaCO3(s)→CaO(s)+CO2(g). Estimate ΔG∘ for this reaction at each of the following temperatures. (Assume that ΔH∘ and ΔS∘ do not change too much within the given temperature range.) A. 1090 K B.1405 K C.Predict whether or not the reaction in part A will be spontaneous at 320 K . D. Predict whether or not the reaction in part B will be spontaneous at 1090. E. Predict whether or not the reaction in part C will be spontaneous...
Rate constants for the reaction NO2(g)+CO(g)?NO(g)+CO2(g) are 1.3M?1s?1 at 700 K and 23.0M?1s?1 at 800 K....
Rate constants for the reaction NO2(g)+CO(g)?NO(g)+CO2(g) are 1.3M?1s?1 at 700 K and 23.0M?1s?1 at 800 K. Part A What is the value of the activation energy in kJ/mol? Ea = 134   kJ/mol   SubmitMy AnswersGive Up Correct Part B What is the rate constant at 770K ? Express your answer using two significant figures. k =   /(M?s)
PART 1. Which of the following reactions are spontaneous (favorable). Check all that apply. A. 2Mg(s)+O2(g)--->2MgO(s)...
PART 1. Which of the following reactions are spontaneous (favorable). Check all that apply. A. 2Mg(s)+O2(g)--->2MgO(s) delta G=-1137kj/mol B.NH3(g)+HCl(g)--->NH4Cl(s) delta G=-91.1 kj/mol C.AgCl(s)--->Ag+(aq)+Cl-(aq) delta G=55.6 kj/mol D.2H2(g)+O2(g)--->2H2O(g) delta G=456 kj/mol E.C(s)+H2O(l)--->CO(g)+H2(g) delta G=90.8 kj/mol F.CH4(g)+2O2(g)--->CO2(g)+2H2O(l) delta G=-820 kj/mol PART 2. Calculate the standard entropy, ΔS°rxn, of the following reaction at 25.0 °C using the data in this table. The standard enthalpy of the reaction, ΔH°rxn, is –633.1 kJ·mol–1. 3C2H2(g)--->C6H6(l)   ΔS°rxn=____JxK-1xmol-1 Then calculate Gibbs free energy for ΔG°rxn in kjxmol-1 Finally,...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT