12 liters of Ammonia (NH3) at a room temperature and pressure (293K and 100kpa) weigh 8.4g.
<h3>Given: </h3>
V(volume) = 12 liters
T(Temperature) = 293K
P(Pressure) = 100kpa
m(Mass) = ?
<h3>Formula applied:</h3>
PV = nRT (Ideal gas equation )
<h3>Universal Constants used : </h3>
R = 8.3145 liter-kpa/ mol-K
<h3>Solution : </h3>
Converting moles to grams :
Molar mass of NH3 = 14.007 g/mol + 1.008 x 3 g/mol = 17.03 g/mol
Calculated mass = 17.03g/mol x 0.4925 mol = 8.4g(approx.)
<h3>What is ideal gas law?</h3>
An ideal gas is one in which there are no intermolecular attraction forces and all collisions between atoms or molecules are entirely elastic. It can be seen as a group of perfectly hard spheres that collide but do not otherwise interact with one another. All of the internal energy in such a gas is kinetic energy, and any variation in internal energy causes a variation in temperature.
PV = nRT ( Ideal Gas Equation)
Learn more about Ideal gas law and ideal gas equations :
brainly.com/question/4147359
#SPJ4