A sample of CO₂ gas at 100.°C has a volume of 250.mL at 760.mm Hg.How many moles of CO₂ are present?

Question

Quizplus · Accepted Answer

To solve the problem, we can use the Ideal Gas Law:

PV = nRT

where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature.

First, we need to convert the temperature to Kelvin:

T = 100°C + 273.15 = 373.15 K

Next, we can rearrange the equation to solve for n:

n = PV/RT

We are given P = 760 mm Hg and V = 250 mL. The gas constant R is 0.08206 L·atm/mol·K. Substituting these values and solving for n, we get:

n = (760 mm Hg)(0.250 L)/(0.08206 L·atm/mol·K)(373.15 K) = 0.00816 mol

Therefore, the answer is A) 0.00816 mol.

A Sample of CO2 Gas at 100