If 3.40 mole is theoritical yield. what is the percent yield if the actual yield from this reaction is 405g ?

The formula actual yield / theoretical yield is used to calculate the percent yield of a reaction. This value is a measure of how much product is produced relative to the what is supposed to be produced. It can be associated with efficiency. The percent yield for this problem cant be solved because of lack of information. The molar mass of the substance should be known to convert the units in order to obtain homogeneity in the units.

Consider a situation in which 235g of P4 are exposed to 272g of O2.

In Part A, you found the amount of product (3.80mol P2O5 ) formed from the given amount of phosphorus and excess oxygen. In Part B, you found the amount of product (3.40mol P2O5 ) formed from the given amount of oxygen and excess phosphorus.

Now, determine how many moles of P2O5 are produced from the given amounts of phosphorus and oxygen

What is the maximum amount in moles of P2O5 that can theoretically be made from 235g of P4 and excess oxygen?

that i got 3.80 as answer

What is the maximum amount in moles of P2O5 that can theoretically be made from 272g of O2 and excess phosphorus?

answer is 3.40

C) ideal gas law the ideal gas law. the volume (v) occupied by n moles of any gas has a pressure (p) at temperature (t) in kelvin. the relationship for these variables, p v = n r t, where r is known as the gas constant, is called the ideal gas law or equation of state.