Calculate the volume of each of the following gas samples at STP.

1. 8.7 mol C2H6

2. 0.250 mol CO

3. 0.465 mol CO2

4. 24.1 mol N2O

All of these should be in liters (L). Can someone help me please?

All of these can be answered with the Ideal Gas Law: PV=nRT. STP means at Standard Temperature and Pressure, which happens to be 1 atm and 273 Kelvin. We are given moles, STP covers Pressure and Temperature, and the Ideal Gas constant (R) [.0821].

1. (1 atm)(V L)=(8.7 mol C2H6)(.0821 [L*atm/(mol*K)])(273 K)

V=(8.7 mol C2H6)(.0821 [L*atm/(mol*K)])(273 K)/((1 atm))

V=195 L C2H6

2. (1 atm)(V L)=(.25 mol CO)(.0821 [L*atm/(mol*K)])(273 K)

V=5.6 L CO

3. (1)(V)=(.465)(.0821)(273)

V= (.465)(.0821)(273)/1

V= 10.4 L CO2

4. (1)(V)=(24.1)(.0821)(273)

V= 540 L N20

Since 1 mole of a gas occupies 22.4 L at STP, just multiply each mole of the given gas by 22.4 to obtain its volume at STP.