[wraene]

Consider the reaction 4PH3 (g) → P4 (g) + H2 (g)
If in a certain experiment, over a specific amount of time, 0.048 mol PH3 is consumed in a 2.0 L container each second of reaction, what are the rates of production of P4 and H2 in this experiment?

I haven't taken chemistry for a long time. I don't understand a bunch of this. Can someone please help?

[DevaDevil]

well, first of all, start by balancing the reaction equation.

[wraene]

The balanced equation is
4PH₃ (g) -> P₄(g) + 6H₂ (g)

[rabolisk]

This tells us that 4 molecules of PH₃ are converted to 1 molecule of P₄ and 6 molecules of H₂. Put another way, every time 4 molecules of PH₃ are used up, 1 molecule of P₄ and 6 molecules of H₂ are formed. See if this helps you.