2H2 (1) + O2(g) → 2H20 (g) 1. Find the limiting reactant if you start with 30.0 grams of hydrogen and 5.29 grams of oxygen.

2. The actual yield for H2O in the above reaction is 6.72 g, Determine the percent yield for the reaction

when 9.93 grams of hydrogen and excess oxygen react?

1. Oxygen is the the limiting reactant.

2. 7.52%

Explanation:

The balanced chemical equation is:

To calculate the moles :

According to stoichiometry :

1 mole of require  = 2 moles of

Thus 0.165 moles of will require=  of

Thus is the limiting reagent as it limits the formation of product and is the excess reagent.

2.  

As 2 moles of give = 2 moles of

Thus 4.96 moles of give =  of

percentage yield =

Thus the percent yield for the reaction is 7.52%

water at room temperature is flowing through a pipe with pressure taps located 10 ft apart along one section of the pipe, which are connected to a mercury (s=13.6) manometer.