Nitric acid is a key industrial chemical, largely used to make fertilizers and explosives. the first step in its synthesis is the oxidation of ammonia. in this reaction, gaseous ammonia reacts with dioxygen gas to produce nitrogen monoxide gas and water.
suppose a chemical engineer studying a new catalyst for the oxidation of ammonia reaction finds that 645. liters per second of dioxygen are consumed when the reaction is run at 195.oc and 0.88 atm. calculate the rate at which nitrogen monoxide is being produced. give your answer in kilograms per second. be sure your answer has the correct number of significant digits.

Rate at which nitrogen monoxide is being produced 0.355Kg /s

Explanation:

4NH3(g) + 5O2(g) ⟶4 NO(g) +6 H2O(l)  

O2 Volume Rate = 645 L /s

Pressure = 0.88 atm

Temperature = 195°C + 273 = 468K

NO molecular weight = 30.01 g/mol

Let´s keep in mind that using this equation our constant R is

PV =n RT

n= PV / RT

n= [ 0.88atm x 645L/s] / [ (0.08205 Lxatm/Kxmol) x 468K]

n= 14.781 moles /s of O2

the leaf is an organ of a typical plant, and the main functions are to complete photosynthesis and allow the plant to exchange gas, just like how we have the respiratory system. leaves have the stomata, which collects maintains co2 and o2 levels. this is necessary for cell metabolism. the leaf also collects sunlight using chloroplasts. succinctly, leaves own a pivotal role in sustaining plant life.