You're asking for the volume of carbon monoxide (CO) given its mass. To do this, you need to know the temperature and pressure of the gas. Here's why and how to solve this:

Why Temperature and Pressure Matter

The volume of a gas is directly related to its temperature and pressure. Here's how:

* Temperature: As the temperature of a gas increases, the molecules move faster and spread out, increasing the volume.

* Pressure: As the pressure on a gas increases, the molecules are squeezed closer together, decreasing the volume.

Using the Ideal Gas Law

The ideal gas law is the most common way to relate the volume, pressure, temperature, and amount of a gas. It's expressed as:

PV = nRT

Where:

* P = Pressure (in atmospheres, atm)

* V = Volume (in liters, L)

* n = Number of moles (mol)

* R = Ideal gas constant (0.0821 L·atm/mol·K)

* T = Temperature (in Kelvin, K)

Here's how to solve the problem:

1. Calculate the number of moles (n) of CO:

* Find the molar mass of CO (12.01 g/mol for C + 16.00 g/mol for O = 28.01 g/mol)

* Divide the mass of CO by the molar mass:

* n = 85.5 g / 28.01 g/mol = 3.05 mol

2. You'll need to provide the temperature (T) and pressure (P) of the carbon monoxide gas.

3. Solve for volume (V):

* Rearrange the ideal gas law: V = (nRT) / P

* Plug in the values for n, R, T, and P.

Example:

Let's say the temperature is 25°C (298 K) and the pressure is 1 atm.

* V = (3.05 mol * 0.0821 L·atm/mol·K * 298 K) / 1 atm

* V ≈ 75.2 L

Therefore, the volume of 85.5 grams of carbon monoxide at 25°C and 1 atm is approximately 75.2 liters.

Important Note: Remember to always include the temperature and pressure when asking about the volume of a gas.