Chemistry: 26 grams of 2,2 dimethyl hexane( C8H16) under goes combustion. How much space would the CO2 gas occupy at 26 Celsius and 101.75 kPa?

Breakdown of rocks is the right answer...

26 grams of 2,2 dimethyl hexane( C8H16) under goes - id262281613212664, sierrabuckner397

yonna74

12.06.2021

The $CO_{2}$ gas occupies a space of 5.57 L at 26 Celsius and 101.75 kPa.

Explanation:

Given: Mass = 26 g

Pressure = 101.75 kPa

Convert kPa into atm as follows.

$1 kPa = 0.00986923 atm\\101.75 kPa = 101.75 kPa \times \frac{0.00986923 atm}{1 kPa}\\= 1 atm$

Temperature = $26^{o}C = (26 + 273) K = 299 K$

Now, moles of a substance is defined as mass of substance divided by its molar mass.

As molar mass of 2,2 dimethyl hexane is 114.23 g/mol. So, its number of moles are calculated as follows.

$No. of moles = \frac{mass}{molar mass}\\= \frac{26}{114.23 g/mol}\\= 0.227 mol$

Formula used to calculate the volume is as follows.

PV = nRT

where,

P = pressure

V = volume

n = no. of moles

R = gas constant = 0.0821 L atm/mol K

T = temperature

Substitute the values into above formula as follows.

$PV = nRT\\1 atm \times V = 0.227 mol \times 0.0821 L atm/mol K \times 299 K\\V = 5.57 L$

Thus, we can conclude that the $CO_{2}$ gas occupies a space of 5.57 L at 26 Celsius and 101.75 kPa.

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