In a study of the reaction below at 1199 K, it was observed that when the equilibrium partial pressure of water vapor is 55.4 torr, the total pressure at equilibrium is 70.7 torr. Calculate Kp for this reaction at 1199 K.
3 Fe(s) + 4 H2O(g) <==> Fe3O4(s) + 4 H2(g)
Can I get this written out? How do you know which part of the equation goes on top for finding Kp?
To solve this problem you have to first calculate partial pressure of remaining gaseous species and then calculate Kp by keeping partial pressures of product on the top or in numerator and of reactants in denominator.
Keep one more thing in mind species present in their solid state are not involved in Kp calculation.
In a study of the reaction below at 1199 K, it was observed that when the...
In a study of the reaction below at 1199 K, it was observed that when the equilibrium partial pressure of water vapor is 53.4 torr, the total pressure at equilibrium is 68.2 torr. Calculate Kp for this reaction at 1199 K. 3 Fe(s) + 4 H2O(g) equilibrium reaction arrow Fe3O4(s) + 4 H2(g)
2. In a study of the reaction 3Fe (1) + 4H20) Fe3O4 (0) + 4H2O at 1200 K it was observed that when the equilibrium partial pressure of water vapor is 15.0 torr, that the total pressure at equilibrium is 36.3 torr. Calculate the value of K, for this reaction. (Hint: Apply Dalton's Law of Partial Pressures)
Consider the reaction: CO(g) + H2O(g) -><- CO2(g) + H2(g) Kp = 0.0871 at 1000 K A reaction mixture originally contains a CO partial pressure of 1744 torr and a H2O partial pressure of 766 torr at 1000 K. Caluculate the equilibrium partial pressures of each of the products 6) (10 points) Consider the reaction: CO(g) + H2O(g) = CO2(g) + H2(g) Kp = 0.0871 at 1000 K A reaction mixture initially contains a CO partial pressure of 1 744...
Consider the following reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kp=0.0611 at 2000 K A reaction mixture initially contains a CO partial pressure of 1346 torr and a H2O partial pressure of 1762 torr at 2000 K. A.) Calculate the equilibrium partial pressure of CO2. B.) Calculate the equilibrium partial pressure of H2.
Consider the following reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kp=0.0611 at 2000 K A reaction mixture initially contains a CO partial pressure of 1390 torr and a H2O partial pressure of 1750 torr at 2000 K. Calculate the equilibrium partial pressure of CO2 and H2. Express the pressure in torr to three significant figures.
Consider the following reaction: CO(g) + H2O(g)CO2(g) + H2 (9) Kp-0.0611 at 2000 K A reaction mixture initially contains a CO partial pressure of 1342 torr and a H2 O partial pressure of 1778 torr at 2000 K. Calculate the equilibrium partial pressure of CO2
Consider the following reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kp=0.0611 at 2000 K A reaction mixture initially contains a CO partial pressure of 1380 torr and a H2O partial pressure of 1770 torr at 2000 K. Calculate the equilibrium partial pressure of CO2.
Consider the following reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kp=0.0611 at 2000 K -A reaction mixture initially contains a CO partial pressure of 1310 torr and a H2O partial pressure of 1790 torr at 2000 K. - Calculate the equilibrium partial pressure of CO2. (Express the pressure in torr to three significant figures.)
The reaction of iron and water vapor results in an equilibrium 3 Fe(s) + 4 H2O (g) ⇋ Fe3O4 (s) + 4 H2 (g) Kc = 5.0 at 800.°C. What is the concentration of water present (in M) at equilibrium if the reaction is initiated with 7.5 g of H2 and excess Fe3O4 in a 15.0 liter container?
The equilibrium constant Kp for the reaction C(s)+H2O(g)⇌CO(g)+H2(g) is 2.44 at 1000 K. What are the equilibrium partial pressures of H2O, CO, and H2 if the initial partial pressures are PCO= 1.30 atm, and PH2= 1.40 atm? Part A What is the equilibrium partial pressure of H2O? What is the equilibrium partial pressure of CO? What is the equilibrium partial pressure of CO?