What is the volume in milliliters of 5.00 moles of helium gas held at a pressure of 1.50 atm and 27 ° C?

Question

Quizplus · Accepted Answer

We can use the ideal gas law, which states:

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 in Kelvin.

First, we need to convert the temperature from Celsius to Kelvin:
27 °C + 273 = 300 K

Next, we can rearrange the ideal gas law to solve for V:

V = (nRT)/P

Plugging in the given values:

V = (5.00 mol)(0.0821 L·atm/(mol·K))(300 K)/(1.50 atm)
V = 8.21 L

However, the question asks for the volume in milliliters, so we need to convert 8.21 L to mL:

8.21 L x 1000 mL/L = 8210 mL

Rounding to three significant figures, we get:

V = 8.21 × 10^3 mL

Therefore, the answer is D) 8.21 × 10^3 mL, which is equivalent to 8.21 × 10^1 mL (to one significant figure).

What Is the Volume in Milliliters of 5