10.34 10.33 Complete the following table for an ideal 104 2.00 atm 0.300 atm 025

Question

10.34 10.33 Complete the following table for an ideal 104 2.00 atm 0.300 atm 0250L 7mol 650 torr 7 atm 100 L 0500 mol K 7L 585 ml 27 C 0.333 mol 3S0K 0250 mol 295 K 10.34 Calculate each of the following quantities for an ideal gas kax 104 (a) thevolume of the gas, in liters, Iif 1.50 mol has a pressure of 125 atmat a temperature of-6,(b) the absolute tempera- ture of the gas at which 3.33 × 10 mol occupies 478 ml. at 750 torr; (c) the pressure, in atmospheres, if 0.00245 mol occupies 413 mL at 138°C; (d) the quantity of gas, in moles, if126.SL at 54·C has a pressure of 1 1.25 kPa. 10.35 The Goodyear blimps, which frequently fly over sporting events, hold approx imately 175,000 ft of helium. If the gas is at 23 °C and 1.0 atm, what mass of helium is in a blimp?

Explanation / Answer

From PV=nRT equation we have

1):v=net/p

1.5*0.083*267/1.25=26.6 litre

2):T=PV/nR=

P=0.98 ATM

=0.98*478/3.33*.083=1.7k Kelvin

3):p=net/v

0.00245*0.083*411/413*0.001=0.202 ATM

4):n=PV/rt=126.5*0.11/0.083*327=0.512 moles

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