(5 points) In the lab you find four bags; each contains 5.00 g of a different gas at STP. The gases are O2, C2H6, CO2, and Ne. Which bag has the largest volume? a O2 b C2H6 c CO2 d Ne

Option D. Ne

Explanation:

Step 1

Data obtained from the question:

Mass of O2 = 5g

Mass of C2H6 = 5g

Mass of CO2 = 5g

Mass of Ne = 5g

Step 2:

At this stage we'll determine the mole of each gas. This is illustrated below:

For O2:

Mass of O2 = 5g

Molar Mass of O2 = 16x2 = 32g/mol

Number of mole = Mass/Molar Mass

Number of mole of O2 = 5/32

Number of mole of O2 = 0.156 mole

For C2H6

Mass of C2H6 = 5g

Molar Mass of C2H6 = (12x2) + (6x1) = 24 + 6 = 30g/mol

Number of mole = Mass/Molar Mass

Number of mole of C2H6 = 5/30

Number of mole of C2H6 = 0.167 mole

For CO2:

Mass of CO2 = 5g

Molar Mass of CO2 = 12 + (16x2) = 12 + 32 = 44g/mol

Number of mole = Mass/Molar Mass

Number of mole of CO2 = 5/44

Number of mole of CO2 = 0.114 mole

For Ne:

Mass of Ne = 5g

Molar Mass of Ne = 20g/mol

Number of mole = Mass/Molar Mass

Number of mole of Ne = 5/20

Number of mole of Ne = 0.25 mole

Step 3:

Determination of the volume occupied by each gas.

This is illustrated below:

1 mole of a gas occupy 22.4L at stp.

For O2:

0.156 mole will occupy = 0.156 x 22.4 = 3.49 L

For C2H6:

0.167 mole will occupy = 0.167 x 22.4 = 3.74L

For CO2:

0.114 mole will occupy = 0.114 x 22.4 = 2.55L

For Ne:

0.25 mole will occupy = 0.25 x 22.4 = 5.6L

Considering the calculations made above, it is evident that Ne has the largest volume

the potential energy of the reactants is 200j.

from the energy diagram, the energy of the product formed is 350j; this means that, this reaction is an endothermic reaction, because it absorbs energy from its environment.