When heated with graphite CO2(g) forms CO(g)
CO2(g) + C(s) 2CO(g)
mass of CO2 = 4.62 g
Molar mass of CO2 = 44 g/mol
Number of moles of CO2 = 4.62 g/44 g/mol = 0.105 mol
mass of C(s) = 3.73 g
molar mass of C(s) = 12 g/mol
number of moles of C(s) = 3.73 g/12 g/mol = 0.311 mol
therefore, C(s) is an excessive reactant.
Initial volume of CO2(g), V = 10 L
Initial temperature of CO2(g), T = 1200 K
R = 0.0821 L atm mol-1 K-1
Applying Ideal gas equation, PV = nRT
or, P = nRT/V = 0.105 mol 0.0821 L atm mol-1 K-1 1200 K / 10 L = 1.035 atm
CO2(g) + C(s) 2CO(g)
Initial pressure 1.035 0
Equilibrium pressure (1.035-x) 2x
Kp = (Pressure of CO)2/(Pressure of CO2) = 5.78 (given)
or, (2x)2/(1.035-x) = 5.78
or, 4x2 + 5.78x - 5.9823 = 0
Solving the above quadratic equation, x = 0.7
Hence, at equilibrium PCO2 = 1.035-x = 1.035 - 0.7 = 0.335 atm and PCO = 2x = 2 X 0.7 = 1.4 atm
Hence, total preessure, Ptotal = PCO2 + PCO = 0.335 atm + 1.4 atm = 1.735 atm
The reaction CO_2(g) +C(s) doubleheadarrow 2CO(g) has K_p = 5.78 at 1200 K. Calculate the total...
The reaction CO2(g) + C(s)<-->2CO(g) has Kp=5.78 at 1200 K. 1) Calculate the total pressure at equilibrium when 4.73g of CO2 is introduced into a 10.0-L container and heated to 1200 K in the presence of 3.75g of graphite. (I have the answer to this half 1.77 atm) 2) Repeat the calculation of part A in the presence of 0.49g of graphite.
Calculate the value of K_p for the equation C(s) + CO_2(g) 2CO(g) K_p = ? given that at a certain temperature C(s) + 2H_2O(g) CO_2(g) + 2H_2(g) K_p^1 = 3.75 H_2(g) + CO_2(g) H_2O(g) + CO(g) K_p^2 = 0.701 K_p =
Carbon monoxide gas may be formed as follows. C0_2(g) + C(s) 2 CO(g) K_p = 5.78 at 1200 K 3.46 g of C0_2,1.98 g of C(s) and 7.22 g of CO(g) are placed in a 12.2 L container and heated to 1200 K. Calculate the total pressure (in bar) at equilibrium. All mathematical steps must be shown. If the volume of the vessel is allowed to expand to 40.0 L when the system is already at equilibrium, would you predict...
For the equilibrium Br2(g)+Cl2(g)⇌2BrCl(g) at 400 K, Kc = 7.0. Part A If 0.25 mol of Br2 and 0.55 mol of Cl2 are introduced into a 3.0-L container at 400 K, what will be the equilibrium concentration of Br2? Express your answer to two significant figures and include the appropriate units. Part B If 0.25 mol of Br2 and 0.55 mol of Cl2 are introduced into a 3.0-L container at 400 K, what will be the equilibrium concentration of Cl2?...
For the equilibrium Br2(g)+Cl2(g)⇌2BrCl(g) at 400 K, Kc = 7.0. Part A If 0.25 mol of Br2 and 0.55 mol of Cl2 are introduced into a 3.0-L container at 400 K, what will be the equilibrium concentration of Br2? Express your answer to two significant figures and include the appropriate units. Part B If 0.25 mol of Br2 and 0.55 mol of Cl2 are introduced into a 3.0-L container at 400 K, what will be the equilibrium concentration of Cl2?...
Methane, CH4, reacts with I2 according to the reaction CH4(g)+I2(g)⇌CH3I(g)+HI(g) At 630 K, Kp for this reaction is 2.26×10−4. A reaction was set up at 630 K with initial partial pressures of methane of 105.1 torr and of 7.96 torr for I2. Part A Calculate the pressure, in torr, of CH4. Express your answer to four significant figures and include the appropriate units. SubmitMy AnswersGive Up Part B Calculate the pressure, in torr, of I2. Express your answer to three...
A 10.0 g sample of krypton has a temperature of 25°C at 560 mmHg Part A What is the volume, in milliliters, of the krypton gas? Express your answer to three significant figures and include the appropriate units.
Consider this reaction: standard conditions CO(g) +2 H2(9)CH,OH(g) K-2.18 x 102 at 340 K Express your answer using three significant figures and include the appropriate units Calculate Δ,G for the reaction at 340 K under each of the following conditions A,G-1 Value Units
A. For the reaction 2KClO3(s) ? 2KCl(s) + 3O2(g) calculate how many grams of oxygen form when 83.6 kg KClO3 completely reacts. Express your answers, separated by commas, in grams to three significant figures. B. For the reaction 2KClO3(s) ? 2KCl(s) + 3O2(g)calculate how many grams of oxygen form when 22.5 mg KClO3 completely reacts. Express your answers, separated by commas, in grams to three significant figures. A. What is the molar mass of butane, C4H10? Express your answer to...
For the reaction H2(g)+I2(g)⇌2HI(g), Kc= 55.3 at 700 K. In a 2.00-L flask containing an equilibrium mixture of the three gases, there are 0.053 g H2 and 4.38 g I2. What is the mass of HI in the flask? Express your answer to two significant figures and include the appropriate units.