An empty water bottle is full of air at 15° c and standard pressure . the volume of the bottle is 0.500 liter . how many moles of air are in a bottle ?

There are 0.0211 moles of air in the bottle

Explanation:

Step 1: Data given

Temperature of air = 15°C = 273.15 + 15 = 288.15 Kelvin

Standard pressure = 1 atm

Volume of the bottle = 0.500 L

Step 2: ideal gas law

p*V = n*R*T

with p = the pressure of the gas = 1 atm

with V = the volume of the bottle = 0.500 L

with n = the number of moles

with R = the gas constant = 0.08206 L*atm/ mol*K

with T = the temperature of the gas = 15 °C = 288.15 Kelvin

In this case we have:

1atm * 0.500L = n * 0.08206  L*atm/ mol*K * 288.15 K

Number of moles n = (1 atm * 0.500 L)/(0.08206  L*atm/ mol*K * 288.15 K)

Number of moles = 0.0211 moles

There are 0.0211 moles of air in the bottle

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d: the voltage of the secondary coil is less than that of the primary coil.

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