Use equation pv = nrt]
a 300 ml sample of gas was collected at stp weighs .90g. what is the molar mass of this gas?

Molar mass of the gas:

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How many moles of gas molecules in that 300 ml of gas sample at STP?

The gas is under Standard Temperature and Pressure, STP. Each mole of an ideal gas will occupy a volume of around 22.4 L or 22,400 ml.

By Arrhenius's Law, the volume of an ideal gas is proportional to the number of gas particles in that gas.

Assuming that the gas in question here is ideal.

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What's the molar mass of this gas?

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hope this

explanation:

covalent bonds

consist of pairs of electrons shared by two atoms, and bind the atoms to fixed orientation and requre high energies to break them

ionic bonds

when two atoms differ considerably in their electronegativity, then one of the atoms will lose its electron to the other atom. this results in a positively charged ion(cation) and a negatively charged ion (anion)

output?

explanation: