Question

If, at 25°C and standard pressure, 2.47 ml of dry air are injected into a graduated cylinder, how many moles of dry air are in the sample space?

Answer 1

To find the number of moles of dry air in a 2.47 ml sample at 25°C and standard pressure, you need to use the ideal gas law equation and convert the volume from milliliters to liters. The calculation yields approximately 0.000101 moles of dry air in the sample.

Step-by-step explanation:

To find the number of moles of dry air in a 2.47 ml sample at 25°C and standard pressure, we can use the ideal gas law equation:

V = nRT, where V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.

First, we need to convert the volume from milliliters to liters by dividing by 1000: 2.47 ml ÷ 1000 = 0.00247 L.

Using the ideal gas law equation and plugging in the values, we have:

0.00247 L = n(0.0821 L·atm/mol·K)(298K)

Solving for n, we get:

n = 0.00247 L / (0.0821 L·atm/mol·K)(298K)

n ≈ 0.000101 mol

Therefore, there are approximately 0.000101 moles of dry air in the sample.