If 0.500 liter of gas X weighs .0750 what is the molecular weight of X? (Volume measured at STP)
THANKYOU
22.4 L at STP is the volume occupied by ONE MOLE of a gas.
what exactly do you do? i have no idea wat to do.
The definition of the molar mass of an ideal gas is that mass of gas that occupies 22.4 L at STP. You know the mass that occupies 0.500 L. So if 0.5 L has a mass of 0.0750 g, then 1 L would weigh what? If that mass occupies 1 L, then how much mass would occupy 22.4 L?
o i get it thankyou
To find the molecular weight of gas X, we can use the ideal gas law equation, which relates the pressure (P), volume (V), temperature (T), and the number of moles of gas (n):
PV = nRT
In this case, we are given the volume of gas X as 0.500 liters, but no information is provided about the pressure or temperature. However, we are told that the volume is measured at STP (Standard Temperature and Pressure).
At STP, the temperature is 273.15 Kelvin (0 degrees Celsius) and the pressure is 1 atmosphere (atm).
We also need to convert the given weight of gas X from grams to moles. The molecular weight (MW) can be calculated using the formula:
MW = weight / (moles * Avogadro's number)
First, we need to convert the given weight of gas X from grams to moles. We know that the weight is 0.0750 g.
To convert grams to moles, we need to divide by the molar mass (M). However, we do not have the molar mass of gas X. So, we cannot directly convert the weight to moles.
To find the molar mass, we need additional information about the composition of gas X (e.g., the elements present and their respective atomic masses).