IN THE REACTION P4 +5 O2= 2P 2 O5. HOW MANY MOLES OF O2 ARE CONSUMED EACH TIME 0.5 MOLES OF P2 O5 ARE FORMED?
0.5 mol P2O5 x (1 mol P4/2 mols P2O5),.
Actually I think it forms P4O10.
how many grams of oxygen must be provided to completely burn 6.75 moles of C2H6? and how do you set up a problem like this?
In the reaction 2P4 + 5O2 → 2P2O5, the stoichiometric ratio between P4 and O2 is 2:5, meaning that for every 2 moles of P4 consumed, 5 moles of O2 are consumed.
To find out how many moles of O2 are consumed each time 0.5 moles of P2O5 are formed, we need to use the stoichiometry of the reaction.
Given that the reaction is:
2P4 + 5O2 → 2P2O5
The moles of P4 consumed is twice the moles of P2O5 formed, so if 0.5 moles of P2O5 are formed, the moles of P4 consumed is:
0.5 moles P2O5 x (2 moles P4 / 2 moles P2O5) = 0.5 moles P4
Using the stoichiometric ratio, we can calculate the moles of O2 consumed as follows:
0.5 moles P4 x (5 moles O2 / 2 moles P4) = 1.25 moles O2
Therefore, each time 0.5 moles of P2O5 are formed, 1.25 moles of O2 are consumed.
To determine the number of moles of O2 consumed each time 0.5 moles of P2O5 are formed, we need to use the balanced chemical equation.
The balanced equation is:
P4 + 5O2 → 2P2O5
From the equation, we can see that the molar ratio between P2O5 and O2 is 5:5, implying that for every 5 moles of O2, 2 moles of P2O5 are formed.
To find the number of moles of O2 consumed, we can set up a proportion based on the ratio:
5 moles O2 / 2 moles P2O5 = x moles O2 / 0.5 moles P2O5
Cross-multiplying the equation gives us:
(5 moles O2)(0.5 moles P2O5) = (2 moles P2O5)(x moles O2)
Simplifying the equation yields:
2.5 moles O2 = 2 moles P2O5
Therefore, each time 0.5 moles of P2O5 are formed, 2.5 moles of O2 are consumed.