UTOR Calculate K from Equilibrium Concentrations Some HI is placed in a sealed flask and heated...

Question

Question

science chemistry

Answer 1

Answer #1

arower A er 2 HI(g) + H₂(g) + 12 (g) ki - CH2] [12] 대파 = [3.28 x 162j* [1.23x10272 [0.137]2 = 3-28X123X104 0.017769 Ki= 0.021

Answer 2

Similar Homework Help Questions

A hypothetical weak base has Kg = 5.0 x 108. Calculate the equilibrium concentrations of the...

A hypothetical weak base has Kg = 5.0 x 108. Calculate the equilibrium concentrations of the base, its conjugate acid, and OH in a 0.15 M solution of the base. What is the pH of the solution? [B] = mol/L [HB]= mol/L [OH-] = pH = Submit Show Approach Show Tutor Steps Submit Answer Try Another Version 10 item attempts remaining
im having trouble solving both of these please help, thank you Tutored Practice Problem 16.3.1 Close...

im having trouble solving both of these please help, thank you Tutored Practice Problem 16.3.1 Close Probl Use equilibrium concentrations to calculate K Some SO3 is placed in a flask and heated to 1350 K. When equilibrium is reached, the flask is found to contain SO, (6.58s 103 M), So, (3.ss-102 M), and O (1.53x102 M). What is the value of the equilibrium constant for the following at reaction at 1350 K? (0-(a)ost(afost K Check &Submit Answer Show Approach Tutored...
Calculate the equilibrium concentrations of H2, I2, and HI at 700 K if the initial concentrations...

Calculate the equilibrium concentrations of H2, I2, and HI at 700 K if the initial concentrations are [H2] = 0.200 M and [I2] = 0.400 M. The equilibrium constant Kc for the reaction following reaction is 57.0 at 700 K. (Show Work) H2(g)+I2(g)<--- ---->2HI(g)

11. When 0.941 mol of gaseous HI is sealed in a 1.00-L flask at 225°C, it decomposes until the equilibrium amount o...

11. When 0.941 mol of gaseous HI is sealed in a 1.00-L flask at 225°C, it decomposes until the equilibrium amount of 12 present is 0.171 mol: 2HI() H2(9)+ I2(9) Use these data to calculate Keg for this reaction at 225°C. Submit Answer Tries 0/99
4. A sample of HI is placed in a sealed container and allowed to come to...

4. A sample of HI is placed in a sealed container and allowed to come to equilibrium. The equilibrium reaction and equilibrium constant are HSO4 (aq) + H20(1) = H,O*(aq) +50:(aq) K.-6.6 x 10-4 A sample mixture was found to have the following equilibrium concentrations: (HSO4] -0.056 M [H30 ) - 0.971 M in the equilibrium mixture? Show the steps in your calculation. What is the molar concentration of SO 5. Would HSO4 a strong or weak acid?(make sure you...
At 35°C, K = 1.6 10-5 for the reaction 2 NOCI(g) 52 NO(g) + Cl2(8) If...

At 35°C, K = 1.6 10-5 for the reaction 2 NOCI(g) 52 NO(g) + Cl2(8) If 3.6 mol NO and 1.8 mol Cl2 are placed into a 1.0-L flask, calculate the equilibrium concentrations of all species. [NOCI) - [NO] - м [C12] - Submit Answer Try Another Version 1 item attempt remaining

A stock solution of K S is available to prepare solutions that are more dilute. Calculate...

A stock solution of K S is available to prepare solutions that are more dilute. Calculate the volume, in ml., of a 2.0-M solution of KS required to prepare exactly 100 ml of a 0.130-M solution of Kys ml Submit Show Approach Show Tutor Steps Submit Answer Try Another Version 10 item attempts remaining Click to try another version of this item. "Note that your response(s) and the points you have earned on this item will be cleared. Previous News)...
The equilibrium constant K for the reaction N2 + 3H22NH, is 0.159 at 450°C. Calculate the...

The equilibrium constant K for the reaction N2 + 3H22NH, is 0.159 at 450°C. Calculate the equilibrium composition when 2.50 mol N2 is mixed with 7.50 mol H2 in a 5.00 L vessel. [N] - M [H2] M (NH3) M Submit Answer Try Another Version 6 Item attempts remaining
Lab Exercise #2: Equilibria Problems 1.2S02e) 22S03(e) at 1500 K: If the equilibrium concentrations are [SO2]...

Lab Exercise #2: Equilibria Problems 1.2S02e) 22S03(e) at 1500 K: If the equilibrium concentrations are [SO2] = 0.424 [ 2. We place 10.0 moles of N20 into a 2.00 L flask at 300 K. At equilibrium 2.20 moles remain. O2]-0.212 [SO3] = 0.076, find the Kc Given the following reaction, what is the Kc and the concentrations of N2 and O2? 3. Indicate whether the reaction will proceed right or left, and which concentrations will decrease or increase: 2HI(g) 근...

The equilibrium constant Kp for the reaction CC, (g) 근 C(s) + 2 Cl2 (g) at...

The equilibrium constant Kp for the reaction CC, (g) 근 C(s) + 2 Cl2 (g) at 700°C is 0.73. Determine the initial pressure of carbon tetrachloride that will produce a total equilibrium pressure of 2.60 atm at 700c. Pressure- atm Try Another Version 4 item attempts remaining At a particular temperature, K = 2.0 × 10-6 for the reaction 2 CO (g) + O2 (g) 2 CO2 (g) If 2.5 moles of CO2 is initially placed into a 5.0-L vessel,...