Question

The equation trangleG= -RT in K relates the value of kp, not kc, to triangeG for...

The equation trangleG= -RT in K relates the value of kp, not kc, to triangeG for gas phase reactions. explain why

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
The equilibrium constant, Kc, is calculated using molar concentrations. For gaseous reactions another form of the...
The equilibrium constant, Kc, is calculated using molar concentrations. For gaseous reactions another form of the equilibrium constant, Kp, is calculated from partial pressures instead of concentrations. These two equilibrium constants are related by the equation Kp=Kc(RT)Δn where R=0.08206 L⋅atm/(K⋅mol), T is the absolute temperature, and Δn is the change in the number of moles of gas (sum moles products - sum moles reactants). For example, consider the reaction N2(g)+3H2(g)⇌2NH3(g) for which Δn=2−(1+3)=−2. For the reaction 2A(g)+2B(g)⇌C(g) Kc = 71.6...
The equilibrium constant, Kc, is calculated using molar concentrations. For gaseous reactions another form of the...
The equilibrium constant, Kc, is calculated using molar concentrations. For gaseous reactions another form of the equilibrium constant, Kp, is calculated from partial pressures instead of concentrations. These two equilibrium constants are related by the equation Kp=Kc(RT)Δn where R=0.08206 L⋅atm/(K⋅mol), T is the absolute temperature, and Δn is the change in the number of moles of gas (sum moles products - sum moles reactants). For example, consider the reaction N2(g)+3H2(g)⇌2NH3(g) for which Δn=2−(1+3)=−2. A) For the reaction 3A(g)+2B(g)⇌C(g) Kc =...
The equilibrium constant, Kc, is calculated using molar concentrations. For gaseous reactions another form of the...
The equilibrium constant, Kc, is calculated using molar concentrations. For gaseous reactions another form of the equilibrium constant, Kp, is calculated from partial pressures instead of concentrations. These two equilibrium constants are related by the equation Kp=Kc(RT)Δn where R=0.08206 L⋅atm/(K⋅mol), T is the absolute temperature, and Δn is the change in the number of moles of gas (sum moles products - sum moles reactants). For example, consider the reaction N2(g)+3H2(g)⇌2NH3(g) for which Δn=2−(1+3)=−2. a For the reaction X(g)+3Y(g)⇌2Z(g) Kp =...
A) Calculate Kc for the reaction below. I2(g)⇌2I(g)Kp=6.26×10−22 (at 298 K) B) Calculate Kc for the...
A) Calculate Kc for the reaction below. I2(g)⇌2I(g)Kp=6.26×10−22 (at 298 K) B) Calculate Kc for the reaction below. CH4(g)+H2O(g)⇌CO(g)+3H2(g)Kp=7.7×1024 (at 298 K) C) Calculate Kc for the reaction below. I2(g)+Cl2(g)⇌2ICl(g)Kp=81.9 (at 298 K)
At 1000 K , Kp=1.85 for the reaction SO2(g)+12O2(g)???SO3(g) What is the value of Kp for...
At 1000 K , Kp=1.85 for the reaction SO2(g)+12O2(g)???SO3(g) What is the value of Kp for the reaction SO3(g)???SO2(g)+12O2(g) What is the value of Kp for the reaction 2SO2(g)+O2(g)???2SO3(g)          What is the value of Kc for the reaction in part (b)?        
If Kp=3.13x10-2 at 500 K for the reaction: Br2 (g) + Cl2 (g) <--> 2 BrCl...
If Kp=3.13x10-2 at 500 K for the reaction: Br2 (g) + Cl2 (g) <--> 2 BrCl (g) a) Calculate Kc at 500K b) What is the value of Kc for the reverse reaction at 500 K? c) Calculate the value of Kp for the following reaction at 500 K:    2Br2 (g) + 2Cl2 (g) <--> 4BrCl (g) d) Given the following two reactions and their equilibrium constants:    AgCl (s)<--> Ag+1 (aq) + Cl-1 (aq) Kc=1.8x10-10 M2    Ag+1...
1. In which of the following reactions will Kc = Kp? A) 2 SO2(g) + O2(g)...
1. In which of the following reactions will Kc = Kp? A) 2 SO2(g) + O2(g) ⇌ 2 SO3(g) B) 4 NH3(g) + 3 O2(g) ⇌ 2 N2(g) + 6 H2O(g) C) SO3(g) + NO(g) ⇌ SO2(g) + NO2(g) D) 2 N2(g) + O2(g) ⇌ 2 N2O(g) E) None of the above reactions have Kc = Kp 2. The reaction below has a Kp value of 3.3 × 10-5. What is the value of Kc for this reaction at 700...
Explain the Arrhenius Equation, k = Ae-Ea/RT, in your own words. How does the Arrhenius Equation...
Explain the Arrhenius Equation, k = Ae-Ea/RT, in your own words. How does the Arrhenius Equation relate to the iodine clock reaction? Please explain in one well-developed paragraph.
For chemical reactions where all reactants and products are in the gas phase the amount of...
For chemical reactions where all reactants and products are in the gas phase the amount of each gas in the vessel can be expressed either as partial pressures or as concentrations. As such the equilibrium constant for a gas phase reaction can also be expressed in terms of concentrations or pressures. For the general reaction, aA(g)+bB(g)⇌cC(g)+dD(g) Kp=(PC)c(PD)d(PA)a(PB)b and Kc=[C]c[D]d[A]a[B]b. It is possible to interconvert between Kp and Kcusing Kp=Kc(RT)Δn where R=0.08314 L bar mol−1 K−1 and Δn is the difference...
Find the Kc value for the reaction at 12C when Kp=0.082 3A(s) + 2B(g) + C...
Find the Kc value for the reaction at 12C when Kp=0.082 3A(s) + 2B(g) + C (g) -> 2 D (g)
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT