Question

write a balanced chemical equation depicting the formation of one mole of pocl3(l) from its elements in their standard states.

Answer 1

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At 25 C and 1 atm pressure (the standard state): P is a solid, O2 is a gas, and Cl2 is a gas. 

P(s) + O2(g) + Cl2(g) ==> POCl3(l) 

To make 1 mole of POCl3, we need to start with 1 mole of P, 1/2 mole of O2, and 3/2 mole of Cl2. 

P(s) + 1/2O2(g) + 3/2Cl2(g) ==> POCl3(l) 

NOTE: Some people write P as P4(s), in which case you would need 1/4 mole P4.

Answer 2

Answer:

Explanation:

First off, it's important to identify the constituent elements of the Compound.

From the compound, we can identify the following elements;

Phosphorus (P), Oxygen (O) and Chlorine (Cl)

So we have;

P + O + Cl --> POCl3

The standard states of elements are the phases that they adopt at a Temperature of 25°C and Pressure of 1 atm.

For POCl3, the standard form of P is P4 (s) while O2 (g) for O and Cl2 (g) for Cl. With this, we now have;

P4 + O2 + Cl2 --> POCl3

Upon balancing, we have;

P4 + 2O2 + 6Cl2 --> 4POCl3

The above equation shows 4 moles of POCl3, since the question stated one mole, we now have;

1/4 P₄ (s) +  1/2 O₂(g) +  3/2 Cl₂ (g) -----> POCl₃ (l)