A5.60 mol sample of solid a was placed in a sealed 1.00 l container and allowed to decompose into gaseous b and c. the concentration of b steadily increased until it reaches 1.40 m, where it remained constant. a(s)↽−−⇀b(g)+c(g) then, the container volume was doubled and equilibrium was re‑established. how many moles of a remain?

The number of moles of A that remain is; 2.8 moles

We are given the decomposition reaction as;

A(s) ⇆ B(g) + C(g)

Also;

Number of moles of solid A; n_a = 5.6 mol

Volume of the container; V = 1 L

Concentration of gas B = 1.4 M

Formula for concentration is;

Concentration = number of Moles/Volume

Thus, concentration of solid A is;

Cₐ = 5.6 moles/1 L

Cₐ = 5.6 M

Similarly;

No of moles = Concentration × volume

Thus, number of moles of gas B is;

n_b = 1.4 × 1

n_b = 1.4 mol

We are told that the volume gets doubled. Thus, V' = 2 L

n'b = 1.4 × 2

n'b = 2.8 moles

Now, the Initial concentration of B and C is 0 M.

Thus;

Cₐ at equilibrium = 5.60 - 2.80

Cₐ at equilibrium = 2.8 M

Thus, number of moles of A at equilibrium is 2.8 moles

∴ Remaining moles of A =  5.6 moles - 2.8 moles

Remaining moles of A = 2.8 moles

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The number of remaining moles of A = 2.80 moles

Explanation:

Step 1: Data given

A(s) ⇆ B(g)+C(g)

Number of moles of solid A = 5.60 mol

Volume of the container = 1.00 L

The concentration of B steadily increased until it reaches 1.40 M

The container volume was doubled and equilibrium was re‑established.

Step 2: Calculate concentration of solid A

Concentration = Moles / Volume

Concentration = 5.6 moles / 1.00 L

Concentration = 5.6 M

Step 3: Calculate moles of B

Moles = Concentration * volume

Moles = 1.40 M *1.00 L = 1.40 moles

Step 4: The volume gets doubled

Moles B = 1.40M * 2.00 L = 2.80 moles

Step 5: The balanced equation

A(s) ⇆ B(g)+C(g)

Initial concentration of A = 5.6M

Initial concentration of B and C = 0 M

Concentration of A at the equilibrium = 5.60 - 2.80 = 2.80

Remaining moles of A = 2.80 moles

The number of remaining moles of A = 2.80 moles

the temperature of the gas, in k, not celsius.