In the manufacturing process of sulfuric acid, sulfur dioxide is reacted with oxygen to produce sulfur trioxide. using the equation, 2so2 (g) + o2 imported asset 2so3 (g), if 192 g of sulfur dioxide is given the opportunity to react with an excess of oxygen to produce 225 g of sulfur trioxide, what is the percent yield of this reaction?

The percent yield of this reaction 93.75%.

Explanation:

if 192 g of sulfur dioxide reacts with excessive of oxygen gas.

Moles of Sulfur dioxide =

According to reaction 2 moles of sulfur dioxide gives 2 moles of sulfur trioxide.

Then 3 mol of sulfur dioxide will give:

of sulfur trioxide

Mass of 3 mole of sulfur trioxide = 3 mol × 80 g/mol = 240 g

Experimental yield of sulfur tiroxide = 240 g

Theoretical yield of sulfur trioxide = 225 g

Percentage yield;

The percent yield of this reaction:

the ozone layer acts as a filter for the shorter wavelength and highly hazardous ultraviolet radiation (uvr) from the sun, protecting life on earth from its potentially harmful effects. when the sky is clear, there is an inverse relationship between stratospheric ozone and solar uvr measured at the earth's surface.