Calculate the mass of butane needed to produce 61.9 g of carbon dioxide

20.4g

Explanation:

First, we need to write a balanced equation for the reaction of butane to produce carbon dioxide.

When butane undergo Combustion, it will produce carbon dioxide and water as shown below:

2C4H10 + 13O2 —> 8CO2 + 10H2O

Molar Mass of C4H10 = (12x4) + (10x1) = 48 + 10 = 58g/mol

Mass of C4H10 from the balanced equation = 2 x 58 = 116g

Molar Mass of CO2 = 12 + (2x16) = 12 + 32 = 44g/mol

Mass of CO2 from the balanced equation = 8 x 44 = 352g

From the equation,

116g of C4H10 produced 352g of CO2.

Therefore, Xg of C4H10 will produce 61.9g of CO2 i.e

Xg of C4H10 = (61.9 x 116)/352 = 20.4g

Therefore, 20.4g of butane(C4H10) is needed to produce 61.9g of CO2

b) mutualism

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in chemistry, adhesion and cohesion are attractive forces that exist between molecules. they hold the molecules together from each other. they are different in that adhesive force exists between molecules of different substance while cohesive force happens between molecules of same substance.

adhesion between water and glass causes water molecules at the edge of water and glass interface to climb up the wall in a narrow glass tube. this is called capillary action. cohesion is what gives glass its shape and causes water to form a droplet.