Question

Name Section 6. A sample of gas occupies 500 mL at STP. What volume will the gas occupy at 85.00 and 525 torr 7. A gas canister can tolerate internal pressures up to 210 atmospheres. If a 2.0L canister holding 3.5 moles of gas is heated to 1350°C, will the canister explode? 8. Calculate the density of 0.625 g of carbon dioxide at 26.32C and 1.03 atm. 9. Calculate the number of grams of hydrogen sulfide gas, HS, in a 3.6 L container at 32.6°C and 712 mmHg. 10. Consider the following equation for the production of NO and NO: 2 NO + O2(g) → 2 NO a. If 84.8 L of O, gas measured at 35.0°C and 632 mmHg, is allowed to react with 158.2 R of NO, find the limiting reactant. b. 97.3 g of NO, forms, measured at 35.0°C and 632 mm Hg, what is the percent yield? Gas Laws Page 180

Answer 1

STP 6) Divi P2V2 P = 760 torr V = 500mL 760 x 500 525 x V2 Ti = 2935 2.73 358 760 x 500x 358 525 * 273 = 949 mL External conditions P F 525 torr = ? T2 = 85+273 358k 7) DV=nRT 3.5x0.0821% (1350+273 ) 20 » 233 atm observed pressure is 233 atm whee pressure is 233 atm which is more than 210 atm, so, Canister explodes: 8) According to gas laos: p= dRT (m= molarman of con a kede glomal ) M d= .pm : d = RT 1:03x44 0.08 24x299.32 = 1.84 g/L 1. a) PV = nRT n=pre 0.9368* 3.6 70.1344 moles 10821x30516 mars of MyS = moles x molormar E 0.1344 x 34 Actrealyield = 4156969 (Ayield - All 10) 2100) + 02 (9) —> 2 NO3(9) al PVE ORT = no se ha = n = 0.831%84:8 → 2.19 moles of on 00821*308 moles of No = 158.2 35.24 moles of No limiting reagent in No, on it control the product formation. b) Theoretical yield & 24.2.429 mans of Ng= 5:27 x 26 17. yield = 11:3x100 + $0.14% = 242429 Theoretical yield loo) 30