Question

What is the pressure in millimeters of mercury of 0.0135 mol of helium gas with a volume of 222 ml at 35 ∘c ? (hint: you must convert each quantity into the correct units ( l , atm , mol , and k ) before substituting into the ideal gas law.) express your answer with the appropriate units.

Answer 1

The question asks for the pressure of a helium gas sample given in moles, volume, and temperature, using the ideal gas law. After unit conversions, the ideal gas law is applied to find the pressure, which can then be converted to millimeters of mercury if necessary.

Step-by-step explanation:

To find the pressure of 0.0135 mol of helium gas with a volume of 222 ml at 35 °C, we will employ the ideal gas law, PV = nRT, where P is the pressure, V the volume, n the number of moles, R the gas constant, and T the temperature. Before substituting into the ideal gas law, ensure that all units are converted correctly:

V should be in liters (0.222 L), T in kelvin (308.15 K), and either use R = 62.36 L·mmHg/(mol·K) or convert the final pressure to atmospheres. The calculation would thus be P = (nRT)/V, where P is the unknown pressure we are finding. After performing the calculation, if desired, we can convert the pressure from atmospheres to millimeters of mercury using the conversion factor of 760 mmHg = 1 atm.