Question

N2O4 (g) ⇌ 2 NO2 (g) Kc = 5.9×10−3 (at 298 K) Express your answer using...

N2O4 (g) ⇌ 2 NO2 (g) Kc = 5.9×10−3 (at 298 K)

Express your answer using two significant figures.

Kp =

SubmitMy AnswersGive Up

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
Problem 16.45 Part A Calculate [OH−] for 1.0×10−3 M Sr(OH)2. Express your answer using two significant...
Problem 16.45 Part A Calculate [OH−] for 1.0×10−3 M Sr(OH)2. Express your answer using two significant figures. [OH−] = 2.0×10−3   M   SubmitMy AnswersGive Up Correct Part B Calculate pH for 1.0×10−3 M Sr(OH)2. Express your answer using two decimal places. pH = 11.30 SubmitMy AnswersGive Up Correct Part C Calculate [OH−] for 2.500 g of LiOH in 220.0 mL of solution. Express your answer using four significant figures. [OH−] = 0.4745   M   SubmitMy AnswersGive Up Correct Significant Figures Feedback: Your...
Using the data in Appendix C in the textbook and given the pressures listed, calculate ΔG...
Using the data in Appendix C in the textbook and given the pressures listed, calculate ΔG for each of the following reactions at 298 K. Part A N2(g)+3H2(g)→2NH3(g)    Express your answer using two significant figures. If your answer is greater than 10100, express it in terms of the base of the natural logarithm using two decimal places: for example, exp(200.00). Kp = SubmitMy AnswersGive Up Part B N2(g)+3H2(g)→2NH3(g) PN2 = 3.6 atm , PH2 = 5.8 atm , PNH3...
For the following reaction, Kc = 255 at 1000 K. CO (g) + Cl2 (g) ⇌...
For the following reaction, Kc = 255 at 1000 K. CO (g) + Cl2 (g) ⇌ COCl2 (g) A reaction mixture initially contains a CO concentration of 0.1510 M and a Cl2 concentration of 0.179 M at 1000 K. You may want to reference ( pages 667 - 677) section 14.8 while completing this problem. Part A What is the equilibrium concentration of CO at 1000 K? Express your answer in molarity to three significant figures. [CO] = M SubmitMy...
Problem 15.52 For the equilibrium Br2(g)+Cl2(g)⇌2BrCl(g) at 400 K, Kc = 7.0. Part A If 0.25...
Problem 15.52 For the equilibrium Br2(g)+Cl2(g)⇌2BrCl(g) at 400 K, Kc = 7.0. Part A If 0.25 mol of Br2 and 0.55 mol of Cl2 are introduced into a 3.0-L container at 400 K, what will be the equilibrium concentration of Br2? Express your answer to two significant figures and include the appropriate units. SubmitMy AnswersGive Up Part B If 0.25 mol of Br2 and 0.55 mol of Cl2 are introduced into a 3.0-L container at 400 K, what will be...
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)
For the equilibrium 2IBr(g)⇌I2(g)+Br2(g) Kp=8.5×10−3 at 150 ∘C. Part A If 2.1×10−2 atm of IBr is...
For the equilibrium 2IBr(g)⇌I2(g)+Br2(g) Kp=8.5×10−3 at 150 ∘C. Part A If 2.1×10−2 atm of IBr is placed in a 2.0-L container, what is the partial pressure of IBr after equilibrium is reached? Express your answer to two significant figures and include the appropriate units. SubmitMy AnswersGive Up Part B If 2.1×10−2 atm of IBr is placed in a 2.0-L container, what is the partial pressure of I2 after equilibrium is reached? Express your answer to two significant figures and include...
Consider the reaction 2NO2(g)?N2O4(g) Calculate ?G at 298 K if the partial pressures of NO2 and...
Consider the reaction 2NO2(g)?N2O4(g) Calculate ?G at 298 K if the partial pressures of NO2 and N2O4 are 0.38atm and 1.64atm , respectively.
A flask is charged with 1.800 atm of N2O4(g)and 1.00 atm NO2(g) at 25 ∘C, and...
A flask is charged with 1.800 atm of N2O4(g)and 1.00 atm NO2(g) at 25 ∘C, and the following equilibrium is achieved: N2O4(g)⇌2NO2 After equilibrium is reached, the partial pressure of NO2 is 0.517 atm . 1)What is the equilibrium partial pressure of N2O4? Express your answer with the appropriate units. 2)Calculate the value of Kp for the reaction. 3)Calculate Kc for the reaction.
A flask is charged with 1.550 atm of N2O4(g)and 1.00 atm NO2(g) at 25 ∘C, and...
A flask is charged with 1.550 atm of N2O4(g)and 1.00 atm NO2(g) at 25 ∘C, and the following equilibrium is achieved: N2O4(g)⇌2NO2 After equilibrium is reached, the partial pressure of NO2 is 0.519 atm . 1.What is the equilibrium partial pressure of N2O4?Express your answer with the appropriate units. 2. Calculate the value of Kp for the reaction. 3.Calculate the value of Kc for the reaction.
Calculate the pH in 0.23 M HCO2H (Ka=1.8×10−4). Express your answer using two decimal places. pH...
Calculate the pH in 0.23 M HCO2H (Ka=1.8×10−4). Express your answer using two decimal places. pH = 2.20 SubmitMy AnswersGive Up Correct Part B Calculate the concentrations of all species present (HCO2H, HCO−2, H3O+, and OH−) in 0.23M HCO2H . Express your answers using two significant figures. Enter your answers numerically separated by commas. [HCO2H], [HCO−2], [H3O+],[OH−] =   M SubmitMy AnswersGive Up Part C Also calculate the percent dissociation. Express your answer using two significant figures.