P4 +502 — P4010 What is the limiting reactant if you are using 25.0 grams of phosphorus and 50.0 grams of oxygen?

A.) O2

B.) P4

C.) P4O10

D.) P4O2

B.) P4

Explanation:

Step 1: Convert 25.0 grams of phosphorus into moles of phosphorous:

25 g P4 x 1 mol P4/123.90 g P4 = 0.202 mol P4

Step 2: Convert 0.202 mol P4 into moles of O2 using their stoichiometric ratios:

0.202 mol P4 x 5 mol O2/1 mol P4 = 1.01 mol O2

Step 3: Convert 1.01 mol O2 into grams of O2:

1.01 mol O2 x 31.98 g O2/1 mol O2 = 32.3 g O2

Because 25.0 grams of phosphorous only needs 32.3 grams of oxygen to react, phosphorous will be the limiting reactant, as after the 25.0 grams of phosphorous is used up, there will still be 17.7 grams of oxygen leftover (excess reactant).

Because the reaction cannot occur without more phosphorous to react with the 17.7 grams of oxygen remaining, P4 is the limiting reactant.

the equation that correctly represent the reaction for formation of ammonia is

n2+ 3h2 → 2nh3 (answer d)

1 mole of nitrogen gas (n2) react with 3 moles of hydrogen gas (h2) to form 2 moles of ammonia ( nh3). this is in a process known as haber process were iron is used as a catalyst and reaction take place that a higher temperature and pressure. the process is exothermic hence energy is released.

explanation: it gains negative electrons, therefore becoming negatively charged. as charge cannot be created, nor destroyed, only transferred, this leaves the wool positive. now that they have opposite charges, the two items attract.