On analysis, an equilibrium mixture for the reaction 2H2S(g) 2H2(g) S2(g) was found to contain 1.0 mol H2S, 4.0 mol H2, and 0.80 mol S2 in a 4.0 L vessel. Calculate the equilibrium constant, Kc, for this reaction.

The equilibrium constant for this reaction is 3.2

Explanation:

Step 1: Data given

Number of moles H2S = 1.0 moles

Number of moles H2 = 4.0 moles

Number of moles S2 = 0.80 moles

Volume = 4.0 L

Step 2: The balanced equation

2H2S(g) ⇆ 2H2(g) S2(g)

Step 3: Calculate molarity

[H2] = 4.0 moles / 4.0 L = 1.0 M

[S2]= 0.80 moles / 4.0 L = 0.20 M

[H2S] = 1.0 moles / 4.0 L = 0.25 M

Step 4: Calculate Kc

Kc = [H2]²[S2] / [H2S]²

Kc  = (1.0²*0.20)/0.25²

Kc = 0.2 / 0.0625

kC = 3.2

The equilibrium constant for this reaction is 3.2

a. they are both space stations

happy to

pls mark as brainliest.

in scientific notation, the value of the  speed of light in a vacuum

  will be written as 2.995 * 10^8. when this value is represented in the form of

  a * 10^b, then, a = 2.995 and b = 8.

the value of the speed of light in a vacuum given above can also be rounded up to approximately 300000000. in this case, the scientific notation will be written as 3 *10^8.