Gaseous hydrogen iodide is placed in a closed container at 425 ∘C, where it partially decomposes to hydrogen and iodine: 2HI(g)←−→H2(g)+I2(g). At equilibrium it is found that [HI]= 3.58×10−3 M , [H2]= 4.86×10−4 M , and [I2]= 4.86×10−4 M .
What is the value of Kc at this temperature?
Gaseous hydrogen iodide is placed in a closed container at 425 ∘C, where it partially decomposes...
What is the final concentration of D at equilibrium if the initial concentrations are [A] = 1.00 M and [B] = 2.00 M ?The reversible chemical reaction A+B⇌C+D has the following equilibrium constant: Kc=[C][D][A][B]=5.3 Gaseous hydrogen iodide is placed in a closed container at 425∘C, where it partially decomposes to hydrogen and iodine: 2HI(g)⇌H2(g)+I2(g) At equilibrium it is found that [HI]= 3.55×10−3M, [H2]= 4.82×10−4M , and [I2]= 4.82×10−4M. What is the value of Kc at this temperature? b The reversible...
Gaseous BrCl is placed in a closed container at 2054 oC, where it partially decomposes to Br2 and Cl2: 2 BrCl(g) 1 Br2(g) + 1 Cl2(g) At equilibrium it is found that p(BrCl) = 0.004430 atm, p(Br2) = 0.008780 atm, and p(Cl2) = 0.002480 atm. What is the value of KP at this temperature? We were unable to transcribe this imageGaseous Brel is placed in a closed container at 2054 °C, where it partially decomposes to Br2 and Cl2: 2...
Gaseous NOBr is placed in a closed container at -171 °C, where it partially decomposes to NO and Br: 2 NOBr(g)# 2 NO(g) + 1 Br2(g) At equilibrium it is found that p(NOBr) 0.007190 atm, p(NO) - 0.009050 atm, and p(Br2) 0.003760 atm. What is the value of Kp at this temperature? Ko
Item 1 Gaseous hydrogen odides placed in a closed container at 25°C where it partially decomposes to hydrogen and lodine 2H (8) H() +1(s) Algulbrum it is found that HT - 351x100 M H, -476-104 Mand (1) - 4.76x10M Part A What is the value of Ke at this temperature? Express the equilibrium constant to three significant digits. You may want to reference coeping this problem 05 040) Section 15 5 while 180 AD OR? K Submit Request Answer Provide...
Gaseous NOBr is placed in a closed container at -165 oC, where it partially decomposes to NO and Br2: 2 NOBr(g) 2 NO(g) + 1 Br2(g) At equilibrium it is found that p(NOBr) = 0.003400 atm, p(NO) = 0.005450 atm, and p(Br2) = 0.007050 atm. What is the value of KP at this temperature? KP = ______
Gaseous BrCl is placed in a closed container at 1099 oC, where it partially decomposes to Br2 and Cl2: 2 BrCl(g) 1 Br2(g) + 1 Cl2(g) At equilibrium it is found that p(BrCl) = 0.002670 atm, p(Br2) = 0.004740 atm, and p(Cl2) = 0.004780 atm. What is the value of KP at this temperature? KP = .
Hydrogen iodide gas decomposes into hydrogen gas and iodine gas at 453°C. If a 2.00 L flask is filled with 0.200 mol of hydrogen iodide gas, 0.156 mol hydrogen iodide remains at equilibrium. What is the equilibrium constant, Kc. for the reaction at this temperature? 2 HI (g) ⇌ H2 (g)+ I2 (8) 0.020 0.0062
Kc for the reaction of hydrogen and iodine to produce hydrogen iodide, H2(g) + I2(g) ⇌ 2HI(g) is 54.3 at 430°C. Determine the initial and equilibrium concentration of HI if initial concentrations of H2 and I2 are both 0.10 M and their equilibrium concentrations are both 0.052 M at 430°C
9. -/0.1 points 0/4 Submissions Used Gaseous NH3 is placed in a closed container at 78 °C, where it partially decomposes to N2 and H2: 2 NH3(9) = 1 N2(g) + 3 H2(g) At equilibrium it is found that p(NH3) = 0.001840 atm, p(N2) = 0.005540 atm, and p(H2) = 0.006350 atm. What is the value of Kp at this temperature? Kp = bit AAC
c for the reaction of hydrogen and iodine to produce hydrogen iodide. H2(g) + I2(g) <-> 2HI(g) is 54.3 at 430 degrees Celsius. Calculate the equilibrium concentrations of H2, I2, and HI at 430 degrees Celsius if the initial concentrations are (H2) = (I2) = 0 M, and (HI)= 0.393 M. (H2) = _______ M (I2) = _________ M (HI) = _________ M (Please explain with an ICE chart if possible.)