Ammonia nh3 chemically reacts with oxygen gas o2 to produce nitric oxide no and water h2o . what mass of water is produced by the reaction of 8.45g of oxygen gas? round your answer to 3 significant digits.

1) Balanced chemical reaction

4NH3 + 5O2 ---> 4NO + 6H2O

2) Molar ratios

4 mol NH3 : 5 mol O2 : 4 mol NO : 6 mol H2O

3) Convert 8.45 g of O2 to moles

moles = mass in grams / molar mass = 8.45 g / 32.0 g/mol = 0.264 mol O2

4) Proportion

5 mol O2 / 6 mol H2O = 0.264 mol O2 / x

=> x = 0.264 mol O2 * 6 mol H2O / 5 mol O2 = 0.3168 mol H2O

5) Convert 0.3168 mol H2O in grams

mass = molar mass * number of moles

molar mass H2O = 18.0 g/mol

mass = 18.0 g/mol * 0.3168 mol = 5.7024 g ≈ 5.70 g

5.70 g

Answerit curves up and levels out.explanationwe assume that the container contains absolutely no ammonia to begin with as it states that "nitrogen gas and hydrogen gas" react to "produce ammonia."at dynamic equilibrium, the product and reactant concentrations are equal.this means that, starting from a concentration of zero, [nh₃] must curve "up" from zero and then level out to a constant concentration.

B. nuclear reactions could first occur.