Question

PLEASE HELP FAST! How many grams of NO are formed if 8.3 g of ammonia react with 11.8 g of oxygen? The reaction is 4NH3 + 5O2 --> 4NO + 6H2O.

Options:
A. 8.85 g NO
B. 12.6 g NO
C. 14.6 g NO
D. 9.3 g NO

Answer 1

To find the grams of NO formed, calculate the moles of ammonia and oxygen used, use the mole ratio to convert to moles of NO, and then convert the moles of NO to grams using its molar mass. The correct answer is option C. 14.6 g NO.

Step-by-step explanation:

To determine the grams of NO formed, we need to calculate the moles of ammonia and oxygen used in the reaction, and then use the mole ratio from the balanced equation to convert to moles of NO. Finally, we can convert the moles of NO to grams using its molar mass.

First, calculate the moles of ammonia and oxygen:

moles of NH3 = 8.3 g / molar mass of NH3 = 8.3 g / 17.03 g/mol = 0.487 mol

moles of O2 = 11.8 g / molar mass of O2 = 11.8 g / 32.00 g/mol = 0.369 mol

Next, use the mole ratio from the balanced equation to calculate the moles of NO:

moles of NO = 0.487 mol NH3 * (4 mol NO / 4 mol NH3) = 0.487 mol

Finally, convert the moles of NO to grams using its molar mass:

grams of NO = 0.487 mol * molar mass of NO = 0.487 mol * 30.01 g/mol = 14.6 g

Therefore, option C. 14.6 g NO is the correct answer.