H2 (g) + I, (g)= 2HI (g). When 46 g of I2 and 1.00 g of H2 are heated to equilibrium at 470°C, the equilibrium mixture contains 1.90 g 12. (a) How many moles of each gas are present in the equilibrium mixture? (b) Compute the equilibrium constant. Ans. (a) 0.0075 mol I2, 0.32 mol H2, 0.35 mol HI; (b) K = 50

The reaction N204(g) 2NO2(g) has a K, = 0.140 at 25 °C. In a reaction vessel containing the gases in equilibrium at that temperature, the partial pressure of N204 was 0.127 atm. (a) What was the partial pressure of NO2 in the reaction mixture? pressure of NO2 = i atm (b) What was the total pressure of the mixture of gases? total pressure = i atm

Calculating equilibrium composition from an equilibrium... 0/5 Suppose 500. mL flask is filled with 1.9 mol of H, and o0.50 mol of C1,. The following reaction becomes possible: H, (g) + Cl,(g) – 2HC1(g) The equilibrium constant K for this reaction is 3.61 at the temperature of the flask. Calculate the equilibrium molarity of H,. Round your answer to two decimal places. OM

At a certain temperature, 0.700 mol SO, is placed in a 2.50 L container. 2 SO3 (g) = 2 S0,(g) + 0,(g) At equilibrium, 0.120 mol O, is present. Calculate K.. Ke =

At 400 K, an equilibrium mixture of H2, 12, and HI consists of 0.065 mol H2, 0.079 mol 12, and 0.13 mol HI in a 4.50-L flask. What is the value of K, for the following equilibrium? (R= 0.0821 L atm/(K • mol)) 2HI(g) = H2(g) + 12(8) 0.29 8.2 0.039 O 26 3.4

The equilibrium concentrate of H2: 0.048 M The equilibrium concentrate of N2: 0.304M

References Use the References to access important values if needed for this question. A student ran the following reaction in the laboratory at 688 K: 2HI(g) H2(g) + I½(g) When he introduced HI(g) at a pressure of 4.87 atm into a 1.00 L evacuated container, he found the equilibrium partial pressure of I2(g) to be 0.510 atm. Calculate the equilibrium constant, K,, he obtained for this reaction. %3D Submit Answer

1) Given the following reaction what is the expression for K? 2SO2 (g) + 02 (g) = 2S03 (g)

At a certain temperature, 0.760 mol SO, is placed in a 2.50 L container. 2 SO,(g) = 2 SO2(g) + O,(g) At equilibrium, 0.120 mol O, is present. Calculate K.. Ke

Consider the reaction N₂(g) + O₂(g) = 2 NO(g) that has an equilibrium constant, Kc, fof 4.10 × 10−4 at 1700 °C. What percentage of O₂ will react to form NO if 0.635 mol N₂ and 0.635 mol O₂ are added to a 0.617 L container and allowed to come to equilbrium at 1700 °C? 2 percentage of 0₂: %