Question

The gas-phase decomposition of HI HI (g) → ½ H2 (g) + ½ I2 (g) has...

The gas-phase decomposition of HI HI (g) → ½ H2 (g) + ½ I2 (g) has k = 30. L/mol⋅min at 443°C. What is the concentration after 3.3 minutes if the initial concentration of HI was 0.010 M? Write the rate law for the reaction.

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
a.)For the gas phase decomposition of hydrogen iodide at 700 K 2 HI---->H2 + I2 the...
a.)For the gas phase decomposition of hydrogen iodide at 700 K 2 HI---->H2 + I2 the following data have been obtained: [HI], M 0.530 0.187 0.114 8.16×10-2 time, s 0 48.0 96.0 144 The average rate of disappearance of HI over the time period from t = 48.0 s to t = 96.0 s is M s-1. b.)For the gas phase decomposition of phosphine at 120 °C 4 PH3(g)----->P4(g) + 6 H2(g) the following data have been obtained: [PH3], M...
Hydrogen iodide decomposes according to the following reaction. 2 HI(g) equilibrium reaction arrow H2(g) + I2(g)...
Hydrogen iodide decomposes according to the following reaction. 2 HI(g) equilibrium reaction arrow H2(g) + I2(g) A sealed 1.5 L container initially holds 0.00615 mol H2, 0.00445 mol I2, and 0.0163 mol HI at 703 K. When equilibrium is reached, the equilibrium concentration of H2(g) is 0.00364 M. What are the equilibrium concentrations of HI(g) and I2(g)?
The decomposition of HI (g) into its elements in the gas phase at 800 K is...
The decomposition of HI (g) into its elements in the gas phase at 800 K is found to proceed by a second order process. A) Please write a balanced equation for the reaction (smallest integer ratio of coefficients, please). B) Please write the rate law for the reaction: C) Given that it takes 142 s for the [HI (g)] to change from 6.75 x 10-2 M to 3.50 x 10-2 M, please calculate the value of the rate constant (and...
The decomposition of hydrogen iodide in the gas phase goes as follows at 600 K. 2...
The decomposition of hydrogen iodide in the gas phase goes as follows at 600 K. 2 HI (g)->H2 (g) + I2 (g) Rate = k[HI]2 k = 9.7x10-6 M-1 s -1 a) Starting with an HI concentration of 0.030 M, what is the concentration of HI after 6.00 days? b) What is the concentration of H2 in the flask after 6.00 days? c) How much time would it take to drop the concentration from 0.030 M to 0.025 M? d)...
Hydrogen iodide undergoes decomposition according to the equation 2HI(g) H2(g) + I2(g) The equilibrium constant Kp...
Hydrogen iodide undergoes decomposition according to the equation 2HI(g) H2(g) + I2(g) The equilibrium constant Kp at 500 K for this equilibrium is 0.060. Suppose 0.898 mol of HI is placed in a 1.00-L container at 500 K. What is the equilibrium concentration of H2(g)? (R = 0.0821 L · atm/(K · mol)) A. 7.3 M B. 0.40 M C. 0.15 M D. 0.18 M E. 0.043 M
1.         Write equilibrium (mass action) expressions for each of the following reactions: (a) H2(g) + I2(g)          2 HI...
1.         Write equilibrium (mass action) expressions for each of the following reactions: (a) H2(g) + I2(g)          2 HI (b)2 NO(g) + O2(g)           2 NO2(g) (c)N2(g) + 3 H2(g)           2 NH3(g) (d) CO(g) + NO2(g)           CO2(g) + NO(g) (e) 2 CO(g) + O2(g)             2 CO2(g) 2.    Write equilibrium expressions for each of the following equilibria: (a) 2 C(s) + O2(g)                  CO(g) (b) Zn2+(aq) + H2S(g)               ZnS(s) + 2 H+(aq) (c) HCl(g) + H2O()                  H3O+(aq) + Cl–(aq) (d)H2(g) +  O2(g)                   H2O(g) 3.         Which of the following is more likely to precipitate the hydroxide ion? (a)...
Be sure to answer all parts. The rate constant for the gaseous reaction H2(g) + I2(g)...
Be sure to answer all parts. The rate constant for the gaseous reaction H2(g) + I2(g) →2HI(g) is 2.42 ×10−2/(M·s) at 400°C. Initially an equimolar sample of H2 and I2 is placed in a vessel at 400° C and the total pressure is 1694 mmHg. (a) What is the initial rate (M/min) of formation of HI? _____ (M/min) (b) What are the rate of formation of HI and the concentration of HI (in molarity) after 13.6 min? Rate of formation...
For the exothermic decomposition of HI (g) into H2(g) and I2 (g) at 400 C, Kc=...
For the exothermic decomposition of HI (g) into H2(g) and I2 (g) at 400 C, Kc= 0.0183 a) If 80 g of HI is placed in a 2.5 L chamber at 400 C, what are the conc. of all species when the system comes to equlibrium? b) How much HI (in g) must be added to the reaction to make 0.050 amount of H2 at equilibrium?
1) The gas phase decomposition of dinitrogen pentoxide at 335 K N2O5(g)  2 NO2(g) + ½ O2(g)...
1) The gas phase decomposition of dinitrogen pentoxide at 335 K N2O5(g)  2 NO2(g) + ½ O2(g) is first order in N2O5 with a rate constant of 4.70×10-3 s-1. If the initial concentration of N2O5 is 0.105 M, the concentration of N2O5 will be  Mafter 391 s have passed. 2) The gas phase decomposition of dinitrogen pentoxide at 335 K N2O5(g)2 NO2(g) + ½ O2(g) is first order in N2O5 with a rate constant of 4.70×10-3 s-1. If the initial concentration of...
For the reaction   2HI(g) ⇌H2(g)+I2(g), Kc= 0.290   at 400 K. If the initial concentration of  HI ...
For the reaction   2HI(g) ⇌H2(g)+I2(g), Kc= 0.290   at 400 K. If the initial concentration of  HI  is  4.0×10−3M and the initial concentrations of  H2, and the initial concentrations of  H2, and I2 are both  1.50×10–3M  at  400 K, which one of the following statements is correct? a. The concentrations of HI and I2 will increase as the system is approaching equilibrium. b. The concentrations of H2 and I2 will increase as the system is approaching equilibrium. c. The system is...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT