Question

In: Chemistry

2.00 moles of CO2 and 1.50 moles of H2 are placed into a rigid 5.00-L container...

2.00 moles of CO2 and 1.50 moles of H2 are placed into a rigid 5.00-L container and they react according to the equation ? ? CO2(g) + H2(g) ? CO(g) + H2O(g) ? ? K = 2.50 What will be the concentration of carbon monoxide when equilibrium is reached?

Solutions

Expert Solution

2.00 moles of CO2 and 1.50 moles of H2 are placed into a rigid 5.00-L container and they react according to the equation ? ? CO2(g) + H2(g) ? CO(g) + H2O(g) ? ? K = 2.50 What will be the concentration of carbon monoxide when equilibrium is reached?

Initial concentration of CO2 = moles / volume = 2 / 5 = 0.4 M

Initial concentraiton of H2 = moles / volume = 1.5 /5 = 0.3 M

The equation is

                          CO2(g) +       H2(g) ===> CO(g) + H2O(g)

Initial            0.4 0.3 0 0

Change -x -x +x    +x

Equilibrium    0.4-x 0.3-x    x x

Kc = 2.50 = [CO] [ H2O] / [CO2][H2] = x2 / (0.4-x)(0.3-x)     = 2.50

x2 = 2.50 [(0.4-x)(0.3-x)]

x2 = 2.50x2 + 0.3 - 0.6x

1.50 x2 + 0.3 - 1.75x = 0

On solving

x = 0.209

[CO] = x = 0.209

queen_honey_blossom answered 2 years ago
Next > < Previous

Related Solutions

5.00 moles of N2 and 8.00 moles of H2 are placed in an empty container, the...
5.00 moles of N2 and 8.00 moles of H2 are placed in an empty container, the container is heated to 887 degrees Celsius, and a catalyst is added that catalyzes the rxn. of these gases to form NH3 as the only product. At equilibrium 1.00 mole of NH3 is found to be present. Find number of moles N2 and moles H2 present at equilibrium. * I think that the concentrations of the reactants changes by 1 mole but I'm not...
A mixture of H2(g) and O2 (g) at 1.50 atm in a rigid container at temperature...
A mixture of H2(g) and O2 (g) at 1.50 atm in a rigid container at temperature T is ignited. The remaining gas, which is entirely H2 (g) exerts a pressure of 0.30 atm at tempertaure T. Assume that the gases are ideal and the H2O(l) formed in the combustion reaction takes up negligible volue in the container. Determine the mole fraction of O2(g) in the original mixture.
A mixture of H2(g) and O2 (g) at 1.50 atm in a rigid container at temperature...
A mixture of H2(g) and O2 (g) at 1.50 atm in a rigid container at temperature T is ignited. The remaining gas, which is entirely H2 (g) exerts a pressure of 0.30 atm at tempertaure T. Assume that the gases are ideal and the H2O(l) formed in the combustion reaction takes up negligible volue in the container. Determine the mole fraction of O2(g) in the original mixture.
a 2.00 l container holds 4.00 moles of o2 and 2.70 moles of he at 293...
a 2.00 l container holds 4.00 moles of o2 and 2.70 moles of he at 293 k. What is the partial pressure of o2? He? what is the total pressure?
4.00 moles of HI are placed in an evacuated 5.00 L flask and then heated to...
4.00 moles of HI are placed in an evacuated 5.00 L flask and then heated to 800 K. The system is allowed to reach equilibrium. What will be the equilibrium concentration of each species
A 0.831 gram sample of SO3 is placed in a 1.00 L rigid container and heated...
A 0.831 gram sample of SO3 is placed in a 1.00 L rigid container and heated to 1100 K. The SO3 decomposes to SO2 and O2 :                                     2SO3(g) ↔ 2SO2(g) + O2(g) At equilibrium, the total pressure in the container is 1.300 atm. Calculate the value of Kp at 1100 K Extra Credit: Consider two containers A and B where A is a rigid container and B is a container with a massless, frictionless piston that maintains constant pressure....
At a certain temperature, 0.860 mol of SO3 is placed in a 1.50-L container. At equilibrium,...
At a certain temperature, 0.860 mol of SO3 is placed in a 1.50-L container. At equilibrium, 0.100 mol of O2 is present. Calculate Kc.
0.924 moles of A (g) is placed in a 1.00 L container at 700 degrees Celsiusand...
0.924 moles of A (g) is placed in a 1.00 L container at 700 degrees Celsiusand a reaction occured. 38.8% of the gas A dissociated when equilibrium was established. 3 A (g) ⇌ 5 B (g) + 2 C (g). What is the value of the equilibrium constant, K, at this temperature? (Answer: K = 0.0241) **PLEASE SHOW WORK. THANKS**
A sample consisting of 2.0 mol CO2 occupies a rigid container (constant volume) of 15.0 L...
A sample consisting of 2.0 mol CO2 occupies a rigid container (constant volume) of 15.0 L at 300 K. When it is supplied with 2.35 kJ of energy as heat its temperature increases to 341 K. Assume that CO2 is described by the van der Waals equation, and calculate w, U, and H.
A 2.00 L reaction container at 25.0 °C contains CO2 (g) and O2 (g). The total...
A 2.00 L reaction container at 25.0 °C contains CO2 (g) and O2 (g). The total pressure of the gases in the container was 656 torr and the mole fraction of CO2 is 0.245. Calculate the partial pressure of oxygen gas in the mixture Calculate the mass of oxygen gas in the mixture (in g). Which gas will rise to the top of the container? Explain your answer. Calculate the total volume of the container if 15.0 g of helium...
ADVERTISEMENT
Subjects
ADVERTISEMENT
Latest Questions
ADVERTISEMENT