4. The volume of a sample of gas at 23°C and 1.2atm is V. Calculate its volume i

Question

4. The volume of a sample of gas at 23°C and 1.2atm is V. Calculate its volume in terms of V at 90°C and 1.10atm. 5. The pressure if a sample of gas when its volume is 1.20 L. What will be its pressure if this sample of gas place in a 1.30L container at the same temperature? 6. How many liters of oxygen will be produced at STP when 1.03g of KClO3 is decomposed? 2KClO3(s)---->2KClO(s)+3O2(g). 7. A sample of hydrogen was collected over water at 25°C when the atmospheric pressure is 758.0 Torr. If the volume of gas is 250mL, calculate (a) the partial pressure of hydrogen, and (b) mol of hydrogen. 8. The mass fraction of oxygen in the atmosphere is 0.233 and that nitrogen is 0.767. What is the partial pressure of each gas when the total pressure is 754 Torr.

Explanation / Answer

4. PV = nRT

p = 1.2atm V = ? n = 1 mole

R = 0.0821 L.atm.k-1.mol-1. T = 296 k

V = nRT/P = (1*0.0821*296)/1.2 = 20.25 L

V = (1*0.0821*363)/1.1 = 27.093 L

5. P = nRT/v = (1*0.0821*296)/1.2 = 20.25 atm

p = (1*0.0821*296)/1.3 = 18.69 atm

6. 2KClO3(s)---->2KClO(s)+3O2(g)

at STP

No of mooles of KClO3 = 1030/122.55 = 8.4 mole

No of moles of O2 liberated = 8.4*(3/2) = 12.6 mole

V = nRT/P = (12.6*0.0821*298)/1 = 308.27 L

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