Question

In: Chemistry

The following reaction reaches equilibrium at 350 degree C and 2 bar, with an equilibrium constant...

The following reaction reaches equilibrium at 350 degree C and 2 bar, with an equilibrium constant K = 3.7064 at these conditions: C H subscript 3 C H O space left parenthesis g right parenthesis space plus space H subscript 2 space left parenthesis g right parenthesis space rightwards arrow space C subscript 2 H subscript 5 O H space left parenthesis g right parenthesis If the system initially contains 1 mol of H2 and 1 mol of acetaldehyde, what is the extent of reaction? Assume ideal gases. Give your answer to 2 decimal places.

Solutions

Expert Solution

For the reaction given:

Keq = 3.7064

                            CH3CHO(g)     +      H2(g)            C2H5OH(g)
Initial                         1                            1                            0
Change                    -x                           -x                           +x
Equilibrium             1 - x                      1 - x                           x

Keq = [C2H5OH] / [CH3CHO][H2]

3.7064 = x / (1-x)(1-x)

x = 0.598

At equilibrium:

CH3CHO = 1 - 0.598 = 0.402

H2 = 1 - 0.598 = 0.402

C2H5OH = 0.508

Extent of reaction,

= ni / vi  

where, ni is the moles of the i-th reactant and νi is the stoichiometric number of the i-th reactant.

= (0.402 - 1) / (-1)

= 0.59


Related Solutions

The equilibrium constant, K, for the following reaction is 10.5 at 350 K. 2CH2Cl2(g) CH4(g) +...
The equilibrium constant, K, for the following reaction is 10.5 at 350 K. 2CH2Cl2(g) CH4(g) + CCl4(g) An equilibrium mixture of the three gases in a 1.00 L flask at 350 K contains 5.47×10-2 M CH2Cl2, 0.177 M CH4 and 0.177 M CCl4. What will be the concentrations of the three gases once equilibrium has been reestablished, if 3.44×10-2 mol of CH2Cl2(g) is added to the flask? [CH2Cl2] =_____ M [CH4] = ________M [CCl4] =________ M
The equilibrium constant, Kc, for the following reaction is 10.5 at 350 K. 2CH2Cl2(g) ------CH4(g) +...
The equilibrium constant, Kc, for the following reaction is 10.5 at 350 K. 2CH2Cl2(g) ------CH4(g) + CCl4(g) Calculate the equilibrium concentrations of reactant and products when 0.321 moles of CH2Cl2 are introduced into a 1.00 L vessel at 350 K. [CH2Cl2] = ------------M [CH4] = ------- M [CCl4] = ------ M
The equilibrium constant, K, for the following reaction is 10.5 at 350 K. 2CH2Cl2(g) =CH4(g) +...
The equilibrium constant, K, for the following reaction is 10.5 at 350 K. 2CH2Cl2(g) =CH4(g) + CCl4(g) An equilibrium mixture of the three gases in a 1.00 L flask at 350 K contains 5.12×10-2 M CH2Cl2, 0.166 M CH4 and 0.166 M CCl4. What will be the concentrations of the three gases once equilibrium has been reestablished, if 0.121 mol of CH4(g) is added to the flask? [CH2Cl2] = _________M [CH4] = _________ M [CCl4] = _________ M
(a) For the reaction 2 A(aq) ⇋ 2 B(g) + C(g), the equilibrium constant is 4.59...
(a) For the reaction 2 A(aq) ⇋ 2 B(g) + C(g), the equilibrium constant is 4.59 at 25.0oC. If the concentrations of B(aq) and C(aq) are each 0.311 M, what concentration of A(aq) is required to have a ΔG value of -6.66 kJ/mol? The temperature is 25.0oC. (b) We have a buffer solution that was produced by adding 11.9 g of NaOH to 2.000 L of a 0.666 M solution of HA(aq). The pH of the buffer solution is 3.25...
The equilibrium constant Kc for the reaction N2O4 <—> 2 NO2 at 25degrees C is 170....
The equilibrium constant Kc for the reaction N2O4 <—> 2 NO2 at 25degrees C is 170. Suppose 13.3g of N2O4 is placed in a 4.000-L flask at 25 C. Calculate the percentage of the original N2O4 that is dissociated?
1. The equilibrium constant, Kp, for the following reaction is 10.5 at 350 K: 2CH2Cl2(g) <--->CH4(g)...
1. The equilibrium constant, Kp, for the following reaction is 10.5 at 350 K: 2CH2Cl2(g) <--->CH4(g) + CCl4(g) Calculate the equilibrium partial pressures of all species when CH2Cl2(g) is introduced into an evacuated flask at a pressure of 0.865 atm at 350 K. PCH2Cl2 =____ atm PCH4 =____ atm PCCl4 =____ atm 2. The equilibrium constant, Kp, for the following reaction is 0.215 at 673 K: NH4I(s) <----> NH3(g) + HI(g) Calculate the equilibrium partial pressure of HI when 0.413...
Using the Equilibrium Constant The reversible chemical reaction A+B⇌C+D has the following equilibrium constant: Kc=[C][D]/[A][B]=4.6 Part...
Using the Equilibrium Constant The reversible chemical reaction A+B⇌C+D has the following equilibrium constant: Kc=[C][D]/[A][B]=4.6 Part A Initially, only A and B are present, each at 2.00 M. What is the final concentration of A once equilibrium is reached? Express your answer to two significant figures and include the appropriate units. Part B What is the final concentration of D at equilibrium if the initial concentrations are [A] = 1.00 M and [B] = 2.00 M ? Express your answer...
At 1700 °C, the equilibrium constant, Kc, for the following reaction is 4.10 × 10–4. N2...
At 1700 °C, the equilibrium constant, Kc, for the following reaction is 4.10 × 10–4. N2 (g) +O2 (g) <---> 2NO (g) What percentage of O2 will react to form NO if 0.737 mol of N2 and 0.737 mol of O2 are added to a 0.645-L container and allowed to come to equilbrium at 1700 °C?
At 1700 °C, the equilibrium constant, Kc, for the following reaction is 4.10 × 10–4. N2...
At 1700 °C, the equilibrium constant, Kc, for the following reaction is 4.10 × 10–4. N2 (g) +O2 (g) <---> 2NO (g) What percentage of O2 will react to form NO if 0.737 mol of N2 and 0.737 mol of O2 are added to a 0.645-L container and allowed to come to equilbrium at 1700 °C?
At 1700 degrees C, the equilibrium constant, Kc, for the following reaction is 4.10 × 10^-4....
At 1700 degrees C, the equilibrium constant, Kc, for the following reaction is 4.10 × 10^-4. N2 (g) +O2 (g) <---> 2NO (g) What percentage of O2 will react to form NO if 0.713 mol of N2 and 0.713 mol of O2 are added to a 0.521-L container and allowed to come to equilbrium at 1700 degrees C?
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT