Cyclists sometimes use pressurized carbon dioxide inflators to inflate a bicycle tire in the event of a flat. these inflators use metal cartridges that contain 16.0 g of carbon dioxide.
at 301 k , to what pressure (in psi) can the carbon dioxide in the cartridge inflate a 3.08 l mountain bike tire?
(note: the gauge pressure is the difference between the total pressure and atmospheric pressure. in this case, assume that atmospheric pressure is 14.7 psi.)
express your answer to three significant figures with the appropriate units.

Pressure of the carbon dioxide gas in the bicycle tire is 28.2 psi.

Explanation:

Using ideal gas equation:

PV = nRT

where,

P = Total Pressure of gas =?

V = Volume of gas = 3.08 L

n = number of moles of gas =

R = Gas constant = 0.0821 L.atm/mol.K

T = Temperature of gas = 301 K

Putting values in above equation, we get:

P = 2.92 atm =   42.91 psi(1 atm =14.6959 psi)

Gauge pressure = Total pressure - Atmospheric pressure

    = P - 14.7 psi = 42.91 psi - 14.7 psi = 28.21 psi ≈ 28.2 psi

Pressure of the carbon dioxide gas in the bicycle tire is 28.2 psi.

explanation:

i think option no d is the correct answer

answer: the value of enthalpy change will be -152.80 kj.

solution:

pressure = 1atm , temperature = = 298 k

given that pressure and temperature are same in both gases , the number of moles of both gases can be determined by the ideal gas equation.

according to reaction 3 moles no are reacting with 1 mol of ,then 0.49 mol of no will react with moles of ozone that is 0.16 moles of ozone. since, no is limiting reagent and is an excessive reagent.

enthalpy change for the reaction between the given volumes of the gases is :