(5 pts) The equilibrium constant for dissociation of silver chloride AgCl (s) Atbnshm T tst aStuton...
StUP 7. (5 pts) The equilibrium constant for dissociation of silver chloride AgCl (s) Ag' (aq) + CI (aq) Is 1.8x1010 Find concentration of silver and chloride ions in saturated aqueous solution of silver chloride (10 pts) The equilibrium constant at certain temperature for 8 H2(g) +1:(g) 2 HI(g) is 55.17. If 10mole of hydrogen and 1.0 mole of iodine are placed in 0.5L flask, what is the equilibrium concentration of hydrogen iodide? (10 pts) Solid ammonium carbamate decomposes to...
7. (5 pts) The equilibrium constant for dissociation of silver chloride AgCl (s) + Ag (aq) + Cl(aq) Is 1.8x10. Find concentration of silver and chloride ions in saturated aqueous solution of silver chloride.
8. (10 pts) The equilibrium constant at certain temperature for H2(g) + 1:(g) → 2 HI(g) is 55.17. If 1.0 mole of hydrogen and 1.0 mole of iodine are placed in 0.5 L flask, what is the equilibrium concentration of hydrogen iodide?
Silver chloride, AgCl, is a sparingly soluble solid. Answer the following questions about a saturated solution prepared by placing solid silver chloride in a 1.94 x 10-5 M NaCl(aq) solution. At some temperature, the silver ion concentration, [Ag+], was found to be 6.24 x 10-6 M. (a) What is the concentration of chloride ions, [CI – ], in the resulting solution? XM (b) What is the molar solubility of silver chloride, AgCl, in 1.94 x 10-5 M NaCl? 4.9 6.24e-6...
the equilibrium constant for the dissociation of iodine molecules to iodine atoms I2 (g) arrow 2I(g) is 3.76x10^-3 at 1000 K. suppose 0.170 mol of I2 is placed in a 18.7 L flask at 1000 K. what are the concentrations of I2 and I when the system comes to equilibrium?
1)Consider the following equilibrium at 972 K for the dissociation of molecular iodine into atoms of iodine. I2(g) ----> 2 I(g); Kc = 1.40 ? 10?3 Suppose this reaction is initiated in a 3.4 L container with 0.067 mol I2 at 972 K. Calculate the concentrations of I2 and I at equilibrium. * I got I2= 0.0135M and I= 0.0124 is this right?* 2)Consider the following equilibrium. NH3(aq) + H2O(l) -----> NH4+(aq) + OH ?(aq) What will happen to the...
Please explain them also H2 + I2 = 2HI Write the equilibrium constant expression for the equilibrium: N2(g) +3 H2(g)2 NH,(g) What is the K for the following reaction at 427 °C if the equilibrium concentrations are [H20.20 M, [l2l0.20 M and [HI] = 1.47 M? Identify the direction in which the equilibrium is favored The chloride ion concentration of a saturated solution of silver chloride is 1.3 x 105M. Calculate Ksp for silver chloride A 0.13 M solution of...
9. The equilibrium constant(K.) for the gaseous dissociation of Iodine molecules to lodine atoms (shown below) 12(8) 21(8) is 3.76 x 10-3 at 1000K. If 0.15 mole of 12(g) is placed in a 12.3-L flask at 1000 K, what are the concentrations of 12(g) and I(g) when the reaction comes to equilibrium?
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...
12. If the acetic acid dissociation constant is 1.8 X 10-5 Ka, and its concentration before dissociation (0.15M), the concentration of H+] is equal to the following equilibrium equation. CH,COOH = CH.COO+H* B) 6.41 X 104 C)2.62 X 104 D)1.64 X 10 13. When dissolved (1.93 g) of HNO, acid (MW=47) and dilute the volume to 500 ml the H concentration in the solution was 7.63X10 M, the value of the dissociation constant Ka was equal to : A) 8...