Question

b) Assuming a reaction starts with 1 mole of octane, which burns at 220°C, and is at a pressure of 1 atm, what volume will the products occupy upon reaction completion?

Answer 1

40.48 liters

Step-by-step explanation

Given: that:

n = mole = 1 mol

P = Pressure = 1 atm

T = Temperature = 220 °C = (220 + 273K) = 493 K

What to find:

The volume of the product.

Step-by-step solution:

The volume, V of the product can be calculated using the ideal gas equation:

PV = nRT

Putting the values of the parameters and molar gas constant, R = 0.0821 liter·atm/mol·K into the formula, we have:

`\begin{gathered} V=(nRT)/(P)=\frac{1\text{ }mol*0.0821\text{ }L.atm\text{/}mol.K*493\text{ }K}{1\text{ }atm}=40.48\text{ }L \\ \end{gathered}`

Thus, the volume of the product, upon reaction completion, will occupy 40.48 liters.