Question

How many grams of CO are present in a 500 ml sample of CO (g) collected at 50°C and 1.50 atm?

Answer 1

0.792 g.

Step-by-step explanation:

What is given?

Volume (V) = 500 mL = 0.5 L.

Pressure (P) = 1.50 atm.

Temperature (T) = 50 °C = 50 °C + 273 = 323 K.

Molar mass of CO = 28 g/mol.

What do we need? Grams of CO.

Step-by-step solution:

To solve this type of problem, we have to use the ideal gas law: the ideal gas law is a single equation that relates the pressure, volume, temperature, and the number of moles of an ideal gas. The formula of ideal gas law is given by the following:

`PV=nRT,`

where P is pressure, V is volume, n is the number of moles, R is the constant of ideal gas which, in this case, is 0.082 atm * L/mol *K.

We want to find the number of moles of CO and then we will find its mass in grams, so let's solve for 'n' and replace the given data in the new formula:

`n=(PV)/(RT)=\frac{1.50\text{ atm}\cdot0.5L}{0.082(atm\cdot L)/(mol\cdot K)\cdot323K}=0.0283\text{ moles CO.}`

And the final step is to convert 0.0283 moles of CO to grams using its given molar mass (you can calculate the molar mass using the periodic table). The conversion will look like this:

`0.0283\text{ moles CO}\cdot\frac{28\text{ g CO}}{1\text{ mol CO}}=0.792\text{ g CO.}`

The mass of CO would be 0.792 g.