Consider the following reaction:
CO2(g) + C(graphite) ⇌ 2 CO(g)
A reaction mixture initially contains 0.56 atm CO2 and 0.32 atm CO. Determine the equilibrium pressure of CO if Kp for the reaction at this temperature is 2.25.
Consider the following reaction: CO2(g) + C(graphite) ⇌ 2 CO(g) A reaction mixture initially contains 0.56...
Consider the following reaction: NO2(g) + N(graphite) ⇌ 2 NO(g) A reaction mixture initially contains 0.86 atm NO2 and 0.42 atm NO. Determine the equilibrium pressure of NO if Kp for the reaction is 3.25
1) The following reaction is an equilibrium reaction. CO2(g) + C(graphite) = 2 CO(g) A reactor initially contained only 0.20 atm CO2 gas in the presence of graphite at 25 °C and later the reaction reached an equilibrium. Answer the following questions. A) If Kis 2.25 at the given temperature above, calculate the equilibrium pressures of CO, and CO, respectively. [6 pts) B) Determine the Ke of the reaction above. [4 pts]
3. At 850°C, Kp is 14.1 for the reaction C(graphite) + CO2(g) t 2CO(g) A reaction vessel at 850°C initially contains CO2 at 0.500 atm, CO at 1.00 atm, and graphite. Determine a. The direction in which the reaction moves b. The equilibrium partial pressure of each gas
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 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 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.)
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(g)CO(g)+H2O(g)⇌CO2(g)+H2(g) Kp=0.0611Kp=0.0611 at 2000 KK A reaction mixture initially contains a COCO partial pressure of 1354 torrtorr and a H2OH2O partial pressure of 1756 torrtorr at 2000 KK. A) Calculate the equilibrium partial pressure of CO2CO2 . B) Calculate the equilibrium partial pressure of H2H2.
Consider the following reaction: I2(g)+Cl2(g)⇌2ICl(g), Kp=81.9 (at 25∘C) A reaction mixture at 25∘C initially contains PI2 = 0.110 atm , PCl2 = 0.110 atm , and PICl = 0.00 atm. Find the equilibrium partial pressure of I2 at this temperature. Find the equilibrium partial pressure of Cl2 at this temperature. Find the equilibrium partial pressure of ICl at this temperature.
13. Calculate equilibrium concentrations: [CO2] 0.56 CO2(8)+ C(graphite) 2 CO(g) M K=2.25