If you are given 7.34moles of a gas at 540K and a pressure of 2.3atm, what is the volume of the gas?

140 L (141.409 without rounding)

Explanation:

Assuming ideal behavior (so that we can use the ideal gas law), we can plug into the equation PV=nRT.  P=2.3 atm, n=7.34 mol, and T=540 K.  (If converting from Celsius to Kelvin, add 273.15.) For R, we'll use 0.082057 L*atm/(mol*K) so that the units cancel out.  2.3 atm*V=7.34 mol*.082057 Latm/(molK)*540 K.  Divide both sides by 2.3 to get the Volume in liters.  That will give you a volume of 140 L (with sig figs.  If you don't round it, you'd get 141.409 L).

108

explanation:

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ca has a crystalline lattice with positive ions (since it is a metal, metals are positively charged) and electrons flow freely in its structure since the ca atoms have a large nuclear radius so the electrons are not tightly held, therefore the electrons can flow freely since they are not being highly attracted by the nucleus. moreover, one of the properties of metals are that they are conductors of electricity, thus proving ca is the element.