Question

Consider the equilibrium CO2 (g)+4H2(g)⇌ CH4 (g)+ 2H2O(g) for which deltaH° =-252.9 kJ/mol and deltaG° =-130.8...

Consider the equilibrium CO2 (g)+4H2(g)⇌ CH4 (g)+ 2H2O(g) for which deltaH° =-252.9 kJ/mol and deltaG° =-130.8 kJ/mol at 298 K. Estimate the equilibrium constant at 350.0 K.

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
Consider the following system at equilibrium CH4(g) + 2H2O(g) ↔ CO2(g) + 4H2(g). Suppose the concentration...
Consider the following system at equilibrium CH4(g) + 2H2O(g) ↔ CO2(g) + 4H2(g). Suppose the concentration of H2O is increased. (a) In which direction does the reaction shift to reestablish equilibrium? (b) What happens to the concentrations of CH4, CO2, and H2 as the reaction shifts to reestablish equilibrium?
The Combustion of 1 mol of CH4 has a  ?Go = -818 kJ/mol. CH4 + 2O2  ? 2H2O...
The Combustion of 1 mol of CH4 has a  ?Go = -818 kJ/mol. CH4 + 2O2  ? 2H2O + CO2 Calculate the Eocell = ____ V
the combustion of methane, CH4, in oxygen. CH4(g) + 2O2(g) >> CO2(g) + 2H2O (l) the...
the combustion of methane, CH4, in oxygen. CH4(g) + 2O2(g) >> CO2(g) + 2H2O (l) the heat of reaction at 77C and 1.00 atm is -885.5 kJ. what is the change in volume when 1.00 mol CH4 reacts with 2.00 mol O2. what is w for this change? calculate delta U (change in U) for the change indicated by the chemical equation
1) Consider the following system at equilibrium where Kc = 55.6 and deltaH° = -10.4 kJ/mol...
1) Consider the following system at equilibrium where Kc = 55.6 and deltaH° = -10.4 kJ/mol at 698 K. H2(g) + I2(g) ---->2 HI (g) The production of HI (g) is favored by: Indicate True (T) or False (F) for each of the following: ___T/F 1. decreasing the temperature. ___T/F 2. increasing the pressure (by changing the volume). ___T/F 3. increasing the volume. ___T/F 4. removing HI . ___T/F 5. removing I2 2) Consider the following system at equilibrium where...
A) For the reaction CH4(g) + H2O(g) ---> 3H2(g) + CO(g) delta H° = 206.1 kJ...
A) For the reaction CH4(g) + H2O(g) ---> 3H2(g) + CO(g) delta H° = 206.1 kJ and delta S° = 214.7 J/K The equilibrium constant for this reaction at 325.0 K is _____ Assume that delta H° and delta S° are independent of temperature. B) For the reaction N2(g) + 2O2(g)-->2NO2(g) deltaH° = 66.4 kJ and deltaS° = -121.6 J/K The equilibrium constant for this reaction at 327.0 K is _____ Assume that delta H° and delta S° are independent...
What mass of natural gas (CH4) must you burn to emit 275 kJ of heat? CH4(g)+2O2(g)→CO2(g)+2H2O(g)ΔH∘rxn=−802.3kJ...
What mass of natural gas (CH4) must you burn to emit 275 kJ of heat? CH4(g)+2O2(g)→CO2(g)+2H2O(g)ΔH∘rxn=−802.3kJ m = Pentane (C5H12) is a component of gasoline that burns according to the following balanced equation: C5H12(l)+8O2(g)→5CO2(g)+6H2O(g) Part A Calculate ΔH∘rxn for this reaction using standard enthalpies of formation. (The standard enthalpy of formation of liquid pentane is -146.8 kJ/mol.) Express your answer using five significant figures. ΔH∘rxn = kJ
The combustion of methane, CH4, releases 890.4 kj/mol of heat. That is, when one mole of...
The combustion of methane, CH4, releases 890.4 kj/mol of heat. That is, when one mole of methane is burned, 890.4 kj are give off to the surroundings. This means that the products have less energy stored in the bonds than the reactants. Thus, for the reaction: CH4(G) + 2 O (g) -> CO2 (g) + 2 H2O (I) deltaH= -890.4kj/mol. A) what is the enthalpy change when 2.00 mol of CH4 are burned? B)what is the enthalpy change when 22.4g...
1.) Write the equilibrium onstant expression for the reaction below (Keq): CH4(g)+2H2S(g) <--> CS2(g)+4H2(g) A reation...
1.) Write the equilibrium onstant expression for the reaction below (Keq): CH4(g)+2H2S(g) <--> CS2(g)+4H2(g) A reation mixture initially contains 0.50M CH4 ad 0.75M H2S. If the equilibrium concenration of H2 is 0.44M, find the equilibrium constatn (Kc) for the reaction. 2.) Express the equilibrium constant for the following reaction. P4(s)+5O2(g) <--> P4O10(s)
Carbohydrates are metabolized according to: CH2O(aq)+O2(aq)=CO2(aq)+H2O(l) DeltaG= -509 KJ/mol How much energy is available per mole...
Carbohydrates are metabolized according to: CH2O(aq)+O2(aq)=CO2(aq)+H2O(l) DeltaG= -509 KJ/mol How much energy is available per mole of carbohydrate at typical blood levela of the chemicals? Assume 298 K [CH2O]= 5.0*10^-3 M [CO2]= 1.7*10^-3 M [O2]= 2.5*10^-4 M
A sample of gas contains 0.1400 mol of CH4(g) and 0.2800 mol of O2(g) and occupies...
A sample of gas contains 0.1400 mol of CH4(g) and 0.2800 mol of O2(g) and occupies a volume of 14.9 L. The following reaction takes place: CH4(g) + 2O2(g)CO2(g) + 2H2O(g) Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant. ______L
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT