Since Kp = (PO2)^3 ---------(1)
If pressure of oxygen is double then
Kp' = (2* PO2)^3 = 2^3 * (PO2)^3 = 8 *(PO2)^3 ----(2)
From (1) & (2)
Equilibrium constant will increase by 8 times if pressure of oxygen doubles.
Write Kp for the reaction 2KCIO3 (s) 2KCI (s) 302 (g) If the pressure of the...
8. Please consider the following reaction at 21.0°C and 744 mm Hg: 2KCIO3(8) 2KCI(S) + 302(g) If 78.0 g of KClO3 react, how many liters of O2 will be produced? A3.00-L plastic container is filled with NH, gas with a pressure of 856 torr at 45°C. Calculate me mass of NH3 in the container. 20
24. Potassium chlorate (KCIO3) was heated to give oxygen. 2KCIO3 (s) - 2KCI (s) + 202 (g) A volume of 550mL of gas was collected over water at 21°C and an atmospheric pressure of 743 Torr. The vapor pressure of water at 21°C is 19 Torr. How many moles of oxygen were collected?
When 5.00 g of KClO3 is heated it decomposes according to the equation: 2KCIO3 ---> 2KCI + 302 a) Calculate the theoretical yield of oxygen b) Give the % yield if 1.78 g of O2 is produced. c) How much Oz would be produced if the percentage yield was 78. 1 i.FT BIO E Eng
The thermal decomposition of potassium chlorate can be used to produce oxygen in the laboratory 2KCIO3 (8) ► 2KCI (s) + 302 (9) What volume (L) of O2 gas at 25°C and 1.00 atm pressure is produced by the decomposition of 7.5 g of KClO3 (s)? Select one: a. 11 b.4.5 CO d. 3.7 e. 2.3
Calculate the entropy of the surroundings at 25°C for the reaction below 2KCI (s) + 302 (g) 2KCLO3(s) AHrxn=-89.4kJ O 300 J/K 2.4x106J/K O 6.86x103 J/K
(1). The equilibrium constant, Kp, for the following reaction is 1.80×10-2 at 698K. 2HI(g) =H2(g) + I2(g) If an equilibrium mixture of the three gases in a 15.5 L container at 698K contains HI at a pressure of 0.399 atm and H2 at a pressure of 0.562 atm, the equilibrium partial pressure of I2 is atm. (2). Consider the following reaction: PCl5(g) =PCl3(g) + Cl2(g) If 1.17×10-3 moles of PCl5, 0.217 moles of PCl3, and 0.351 moles of Cl2 are at...
For the reaction H2 S(g) + I2 (s) ⇌ S(s) + 2 HI(g) Kp = 1.33×10–5 at 333 K. What will be the total pressure of the gases above an equilibrium mixture if, at equilibrium, PHI = 0.010 × PH2 S? The answer is 0.134 atm. Please include work and explanation! Thank you :-)
For the reaction 2A(g) ⇌ B(g) + 2C(s) the equilibrium constant is Kp = 3.6 at a particular temperature. The reaction mixture initially contains 2.0 atm of each gas, A and B, and 10.2 g of C. Choose the statement that is true of the reaction mixture as equilibrium is established at that temperature. A) The reaction will proceed to form more A. B) The outcome cannot be predicted since more data are needed. C) The reaction will proceed to...
Consider the reaction: SO2Cl2(g)⇌SO2(g)+Cl2(g) Kp=2.91×103 at 298 K In a reaction at equilibrium, the partial pressure of SO2 is 0.156 atm and that of Cl2 is 0.365 atm . What is the partial pressure of SO2Cl2 in this mixture?
The equilibrium constant, Kp , for the following reaction is 1.04×10-2 at 548 K. NH4Cl(s) NH3(g) + HCl(g) If an equilibrium mixture of the three compounds in a 4.51 L container at 548 K contains 1.31 mol of NH4Cl(s) and 0.103 mol of NH3(g), the partial pressure of HCl(g) is __ atm.