Question

Consider the reaction       CS2(g) + 4 H2(g) --> CH4(g) + 2 H2S(g) Determine the temperature...

Consider the reaction

      CS2(g) + 4 H2(g) --> CH4(g) + 2 H2S(g)

Determine the temperature at which the reaction changes spontaneity.

(DS° for CS2(g) is 237.79 J/molK, DH° for CS2(g) is 117.0 kJ/mol)

Homework Answers

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
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)
Calculate ΔrG° for the reaction below at 25.0 °C CH4(g) + H2O(g) → 3 H2(g) +...
Calculate ΔrG° for the reaction below at 25.0 °C CH4(g) + H2O(g) → 3 H2(g) + CO(g) given ΔfG° [CH4(g)] = –50.8 kJ/mol, ΔfG° [H2O(g)] = –228.6 kJ/mol, ΔfG° [H2(g)] = 0.0 kJ/mol, and ΔfG° [CO(g)] = –137.2 kJ/mol.
Consider the following balanced thermochemical equation, sometimes used for H2S production. 1/8 S8(s) + H2(g) H2S(g)...
Consider the following balanced thermochemical equation, sometimes used for H2S production. 1/8 S8(s) + H2(g) H2S(g) ΔHrxn = -20.2 kJ (a) Is this an exothermic or endothermic reaction? (b) What is ΔHrxn for the reverse reaction? kJ (c) What is ΔHrxn when 1.5 mol S8 reacts? kJ (d) What is ΔHrxn when 22.2 g S8 reacts? kJ
For the reaction:                                 2 C (s) + H2(g) →C2H2(g) a) Calculate the enthalp
For the reaction:                                 2 C (s) + H2(g) →C2H2(g) a) Calculate the enthalpy of reaction (DHrxn) from the following reactions: Reaction                                                             Δ Hrxn(kJ/mol)2 C2H2(g)+ 5 O2(g) → 4 CO2(g) + 2 H2O (l)              -2599.2 C (s) + O2(g) → CO2(g)                                            - 393.5 2 H2(g) + O2(g) → 2H2O (l)                                      -571.8 b) If the DS for the reaction is equal to 652 J/mol, and the reaction proceeds at 25°C, would you expect the reaction to be spontaneous?
Consider the following reaction: 2CH4(g)⇌C2H2(g)+3H2(g) The reaction of CH4 is carried out at some temperature with...
Consider the following reaction: 2CH4(g)⇌C2H2(g)+3H2(g) The reaction of CH4 is carried out at some temperature with an initial concentration of [CH4]=0.083M. At equilibrium, the concentration of H2 is 0.020 M . Find the equilibrium constant at this temperature. Express your answer using two significant figures.
Consider the following reaction: 2CH4(g)⇌C2H2(g)+3H2(g) The reaction of CH4 is carried out at some temperature with...
Consider the following reaction: 2CH4(g)⇌C2H2(g)+3H2(g) The reaction of CH4 is carried out at some temperature with an initial concentration of [CH4]=0.085M. At equilibrium, the concentration of H2 is 0.018 M. Find the equilibrium constant at this temperature. Express your answer using two significant figures.
Consider the following gas-phase reaction: 2 CCl4(g) + H2(g) C2H2(g) + 4 Cl2(g) Using data from...
Consider the following gas-phase reaction: 2 CCl4(g) + H2(g) C2H2(g) + 4 Cl2(g) Using data from Appendix C of your textbook calculate the temperature, To, at which this reaction will be at equilibrium under standard conditions (Go = 0) and choose whether >Go will increase, decrease, or not change with increasing temperature from the pulldown menu. To = K, and Go will with increasing temperature. For each of the temperatures listed below calculate Go for the reaction above, and select...
Consider the following data at 298 K: Compound ∆Hf° (kJ mol−1) H2S (g) -20.5 H2O (g)...
Consider the following data at 298 K: Compound ∆Hf° (kJ mol−1) H2S (g) -20.5 H2O (g) -242 For the reaction   4 Ag(s) + 2 H2S(g) + O2(g) --> 2 Ag2S(s) + 2 H2O(g)    at a temperature of 25 °C, ∆H° = −507 kJ Calculate the ∆Hf° of Ag2S (s) is (in kJ mol−1): -285.5 -32 -64 + 475
Consider the following reaction. CH3OH(g) CO(g) + 2 H2(g) DELTA-H = +90.7 kJ (a) Is the...
Consider the following reaction. CH3OH(g) CO(g) + 2 H2(g) DELTA-H = +90.7 kJ (a) Is the reaction exothermic or endothermic? (b) Calculate the amount of heat transferred when 45.0 g of CH3OH(g) are decomposed by this reaction at constant pressure. DELTA-H =___ kJ (c) If the enthalpy change is 20.0 kJ, how many grams of hydrogen gas are produced? _____g (d) How many kilojoules of heat are released when 11.5 g of CO(g) reacts completely with H2(g) to form CH3OH(g)...
Part 1: You wish to determine ΔH of the following reaction. CS2(ℓ) + 3O2(g) ---> CO2(g)...
Part 1: You wish to determine ΔH of the following reaction. CS2(ℓ) + 3O2(g) ---> CO2(g) + 2SO2(g) Previous research indicates the following ΔH reaction values: C(s) + O2(g) ---> CO2(g) ΔH = -393.5 kJ/mol S(s) + O2(g) ---> SO2(g) ΔH = -296.8 kJ/mol C(s) + 2S(s) ---> CS2(ℓ) ΔH = +87.9 kJ/mol In order to match the coefficients in the desired reaction, which transformation(s) will you do to the reaction forming CO2? And how will ΔH change? A) Flip,...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT