The reversible chemical reaction A+B?C+D has the following equilibrium constant:

Question

The reversible chemical reaction

A+B?C+D has the following equilibrium constant: Kc=[C][D]/[A][B]=3.7

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] = 1.00M and [B] = 2.00M? Express your answer to two significant figures and include the appropriate units.

2) Consider the reaction for the decomposition of hydrogen disulfide 2H2s(g)<-> 2H2(g) + S2 Kc= 1.67x10^4 at 800 degrees celsius. A 0.500 L reaction vessel iitially contains 0.0125 mol of H2s at 800 degrees celsius .  Find the equilibrium concentration of [S2]. [H2S] = 0.100 M, [H2] = 0.100 M, and [S2] = 0.00 M. Find the equilibrium concentration of [S2]. Temp is 800 degrees celsius.

3) The reaction CO2(g)+C(s)?2CO(g) has Kp=5.78 at 1200 K. Part A: Calculate the total pressure at equilibrium when 4.56g of CO2 is introduced into a 10.0-L container and heated to 1200 K in the presence of 2.19g of graphite. Part B: Repeat the calculation of part A in the presence of 0.31g of graphite.

Explanation / Answer

part1) final conc. A=x=B; of D and C it will be 2-x;

so, 3.5=(2-x)^2/x^2; so, x=0.6969M final conc of A

part 2) let conc of D and C be x each so, conc of A=1-x; and B=2-x;

so, 3.5=x^2/(1-x)/(2-x) so, x=0.8311 M is conc of D

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