for the reaction 2CO + O2 = 2CO2 it is found that at a certain temperature the concentration are [CO] = 7.2 x 10^-4 M, [O2] = 8.1 x 10^-3 M, and [CO2] = 2.3 x 10-2 M. write out the equilibrium expression and calculate K for the reaction at this temperature?
How would the equilibrium position change if CO2 was added?
2 CO (g) + O2 (g) 2 CO2 (g)
equilibrium constant, K = [CO2]2 / ([CO]2[O2])
K = (2.3 x 10-2 M)2 / [(7.2 x 10-4 M)2 * (8.1 x 10-3 M)]
K = 1.26 x 105
If CO2 is added then the reaction would shift backwards so that the added CO2 is consumed and equilibrium can be achieved again
for the reaction 2CO + O2 = 2CO2 it is found that at a certain temperature...
For the reaction 2CO(g)+O2(g)⇌2CO2(g), the value of K at a certain temperature is 1300. Calculate [CO2] at equilibrium when [CO] = 9.0×10−2 mol/L and [O2] = 0.527 mol/L
Consider the following reaction at equilibrium. 2CO2 (g) 2CO (g) + O2 (g) ΔH° = -514 kJ Le Châtelier's principle predicts that the equilibrium partial pressure of CO (g) can be maximized by carrying out the reaction ________. A.) at low temperature and low pressure B.) at low temperature and high pressure C.) at high temperature and low pressure D.) in the presence of solid carbon E.) at high temperature and high pressure
Assuming that Ac is independent of temperature, calculate AH1200 for the reaction: 2CO(g) + O2(g) → 2CO2(g) AH co Chemical KkJ mol-?) U moll) -398.029 39.277 CO2(g) o2g) CO(g) n/a 28.34 -111.42 27.247 -577078.56
13. Given the following reaction: 2CO(g) + O2(g) & CO2(g) with K. = 4000. Ar equilibrium, the concentrations of O, and Co, are 0.10 M and 0.75 M, respectively. Calculate the concentration of CO at equilibrium.
Given the following reaction: 2CO (?) + O2 (?) → 2CO2 (?) ∆? = −566 kJ/mol Calculate the change in internal energy when ?∆? at constant pressure is -102 kJ/mol.
An equilibrium mixture of Co, O2 and CO2 at a certain temperature contains 0.0010 M CO2 and 0.0100 M 02. At this temperature, Kc equals 1.4 x 10^2 for the reaction: 2 CO(g) + O2(g) = 2 CO2(g). What is the equilibrium concentration of CO? O a. 7.1 x 10-7 Ob.1.4 x 10-2 M O c. 8.4 x 10-4 M d. 1.2 * 10-1 M
An equilibrium mixture of CO O2 and CO2 at a certain temperature contains 0.00 10 2 CO(g) + Oda) _ 2 CO2(g). What is the equilibrium concentration of CO? CC and 0.0 100 O2 Athis temperature k equals 1.4·10. r e eaction: 0 1.4x 10-2 M O 1.2 x 10-1 M O 8.4 x 10 M O 7.1 x 10 M
4. Calculate AG°(375 K) for the reaction 2CO(g) + O2(g) → 2CO2(g) from the values of AG°(298 K) and AH°(298 K) (found in tables) and the Gibbs-Helmholtz equation.
An equilibrium mixture of CO, O2 and CO2 at a certain temperature initially contains 0.0010 M CO2 and 0.0015 M O2. At this temperature, Kc, equals 1.4 × 102 for the reaction: 2 CO(g) + O2(g) <=> 2 CO2(g). What is the equilibrium concentration of CO?
11. For the given reaction at a certain temperature, the equilibrium concentrations were found to be 2] 5.7x 10- M, [o2)- 1.o x from these data (delete units). O x 10 2M, and [NO] - 2.0 x 10 M. Calculate the value of the equilibrium constant and 2NO(g) + Olg)-2NO2(g) a. 8.1 x 102 b. 14.3 x 104 C. 2.9% 102 d. 1.2 x 103 e. None of these