a) calculate the number of moles of He that you shoulf add to each balloon so th

Question

a) calculate the number of moles of He that you shoulf add to each balloon so that the volume at the party will bw 10 L

b) what will be the volume of each balloon in the laboratory ?

c) suppoused the overnight low tempeture after the party was 15 c with the pressure still at 1 atm. what is the new volume of the balloons, assuming no gas loss?

You plan to fill balloons with helium in a 25°C laboratory for an outdoor party where the expected temperature will be 36°C and pressure will be 1 atm. R 0.08206 L-atm/mole-K

Explanation / Answer

a) According to ideal gas equation: PV = nRT

T = 36 oC = (36+273.15) K = 309.15 K, V = 10 L

P = 1 atm, R = 0.08206 L atm mol-1 K-1

i.e. 1 atm*10 L = n*0.08206 L atm mol-1 K-1*309.15 K

i.e. n = 0.3942 mol of He

b) PV = nRT

i.e. 1 atm * V = 0.3942 mol*0.08206 L atm mol-1 K-1*298.15 K

i.e. V = 9.644 L

c) PV = nRT

i.e. 1 atm*V = 0.3942 mol*0.08206 L atm mol-1 K-1*288.15 K

i.e. V = 9.32 L

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