The given question is incomplete. The complete question is as follows.
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.
Explanation:
Chemical equation for the oxidation of ammonia is as follows.
Then volume of per second consumed is as follows.
V =
As this reaction is taking place at a temperature of (468.15 K) and pressure 0.88 atm. Hence, moles of consumption of are calculated as follows.
n =
=
= 14.77 mol /sec
When 5 moles of produces 4 moles of NO then the amount of NO produced from 14.77 mol
= 354.60 g/s
Therefore, NO formed per second is as follows.
= 0.35 kg/s
Thus, we can conclude that the rate at which nitrogen monoxide is being produced is 0.35 kg/s.
Answer:
7g/cm³
Explanation:
Given parameters:
Mass of the mineral = 21g
Volume = 3cm³
Unknown:
Density of the mineral = ?
Solution:
Density of a substance is the mass per unit volume of the substance.
Density =
Now insert the given parameters and solve;
Density = = 7g/cm³
The mineral with a density of 7g/cm³ is Galena, an ore of lead.
Answer:
C. This is because weathering is when a rock is broken down to smaller bits and destroyed. Hope this helps!