For the reaction shown, 38.25 grams of silicon is combined with 14.33 grams of nitrogen gas. how many grams of silicon nitride can be formed if nitrogen is the limiting reactant? 3si + 2n2 yields si3n4 17.94 g 21.23 g 35.88 g 63.69 g

From the periodic table:
molar mass of silicon = 28 grams
molar mass of nitrogen = 14 grams

From the balanced chemical equation, 
3 x 28 = 84 grams of silicon react with 2 x 2 x 14 = 56 grams of nitrogen to produce 3(28) + 4(14) = 140 grams of silicon nitride.

Since it is mentioned that nitrogen is the limiting reagent, therefore, the reaction will stop once the amount of reacting nitrogen is consumed.
Now we know that 56 grams of nitrogen produce 140 grams of silicon nitride. Thus, we can use cross multiplication to calculate the amount of silicon nitride produced when using 14.33 grams of nitrogen as follows:

amount of produced silicon nitride = (14.33 x 140) / 56 = 35.8 grams

This is what i found on google “when one phosphate group is removed by breaking a phosphoanhydride bond in a process called hydrolysis, energy is released, and atp is converted to adenosine diphosphate (adp). likewise, energy is also released when a phosphate is removed from adp to form adenosine monophosphate (amp).” i hope this you .