  A researcher is studying the decomposition of A as shown by the general reaction below:2 A(g) 2 B(g) + 2 C(g)Initially, the scientist fills an evacuated 4.956 L flask with 9.570 x 10-1 moles of species A. Upon equilibrium, it is determined that the concentration of A is 1.724 x 10-1 M. Calculate Kc.

Question

A researcher is studying the decomposition of A as shown by the general reaction below:

2 A(g) 2 B(g) + 2 C(g)

Initially, the scientist fills an evacuated 4.956 L flask with 9.570 x 10-1 moles of species A. Upon equilibrium, it is determined that the concentration of A is 1.724 x 10-1 M. Calculate Kc.

Step 1

Kc of the reaction is calculted using ICE table. help_outlineImage TranscriptioncloseAn equilibrium constant (K) is the ratio of concentration of products and reactants raised to appropriate stoichiometric coefficient at equlibrium For the general reaction aА + bв — сС+dD The relative strength of reaction can be also expressed quantitatively with an equilibrium constant as follows: (aC) (aD) К. (aA) (1) aB An equilibrium constant is (K ). fullscreen
Step 2

concentration of A is calculated. help_outlineImage TranscriptioncloseThe reaction is shown below 2A (g)2B (g) 2C (g) K of the reaction is calculated as follows, Moles Concentration Volume = Concentration ofA = Moles Volume Concentration of A = 9.570 x10 4.956 Concentration of A=0.193 fullscreen
Step 3

At equilibrium the concentration of... help_outlineImage TranscriptioncloseICE table 2C (g) 2B (g 2A(g) 0.193 M Initial 0 0 concentration +2x Change -2x +2x At equilibrium 0.193-2x 2x 2x According to the equation, 0.193-2x-1.724 x1 0 2x 0.0206 x0.0103 fullscreen

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