1. A GAS EXERTS A P=4.00 ATM AND OCCUPIES A 10.0L VESSEL. IT IS ALLOWED TO EXPAND INTO A 20.0L VESSEL AT CONSTANT n AND T.
WHAT IS THE NEW P IN torr?
A) 6.00 torr B) 1.52X103 torr C) 3.04X103 torr D) 190 torr
2. A GAS HAS T=27.00C IN A 10.0L VESSEL. IT IS FORCED, AT CONSTANT n AND P, INTO A 2.00X103 mL VESSEL. WHAT IS THE NEW T IN 0C?
A) -193.0 B) 8.92X104 C) 5.4 D) -213.2
3. WHAT VOLUME DOES 22.0g CO2 OCCUPY AT STP?
A) 6.72L B) 5.6L C) 29.1L D) 11.2L
4. A GAS OCCUPIES A 2.00L VESSEL AND HAS P=5.00ATM AT T=127.00C. THE GAS IS ALLOWED TO EXPAND, AT CONSTANT n, INTO A 10.0L VESSEL AT 27.00C. CALCULATE THE NEW P IN ATM.
A) .750 B) .213
C) 570 D) 1.33
5. A GAS OCCUPIES 30.0L AT 57.20C UNDER 380.0 torr. WHAT IS n ?
A) 3.19 B) 1.81
C) 9490 D) .553
6. DETERMINE THE MOLAR MASS OF A GAS IF 1.60g OCCUPIES
100.0mL AT 37.00C UNDER 5.00 ATM.
A) 50.9 g/mol B) 40.7 g/mol C) 6.08 g/mol D) 81.4 g/mol
7. CONSIDER A MIXTURE OF 4.4 g CO2 AND 5.6 g N2 WITH PTOTAL=9.0 ATM. DETERMINE PARTIAL P FOR CO2 AND N2.
A) .33, .67 B) 3.0, 6.0 C) .76, .24 D) 3.3, 6.7
8. CONSIDER THE REACTION : N2 + 3H2 ßà 2NH3 IF THE REACTANTS AND PRODUCTS ARE AT STP DETERMINE THE VOLUME OF NH3 PRODUCED WHEN 9.00 L N2 IS REACTED WITH EXCESS H2.
A) 14.0 L B) 27.0 L C) 42.0 L D) 18.0 L
9. CALCULATE THE urms FOR N2 GAS AT 1270C
A) 10.6 m/s B) 597 m/s C) 336 m/s D) 59.3 m/s
10. CONSIDER THE REACTION: N2 + 3H2 ßà 2NH3 IF 2.00L N2 UNDER 3.00 ATM AT 27.00C REACTS WITH EXCESS H2 AT THE SAME T,P HOW MANY LITERS OF NH3 CAN BE PRODUCED UNDER 5.00 ATM AT 52.00C.
A) 4.00L B) 2.OOL C) 2.63L D) 68.3L
FOR THE NEXT 3 PROBLEMS CONSIDER THE FOLLOWING. A SOLID SAMPLE OF KClO3 IS DECOMPOSED ACCORDING TO:
2KClO3(s) à 2KCl(s) + 3O2(g)
THE O2 PRODUCED IS COLLECTED OVER WATER AND THE FOLLOWING DATA IS COLLECTED: T=250C, PBAR=762 torr, VPWATER AT 250C=23 torr V OF O2 COLLECTED=0.40 L
11. DETERMINE PARTIAL P OF O2 IN ATM
A) 0.972 ATM B) 1.03 ATM C) 1.00 ATM D) .400 ATM
12. DETERMINE THE MOLES OF O2 COLLECTED
A) 0.017 mol B) 0.016 mol C) 0.19 mol D) 12 mol
13. DETERMINE THE GRAMS OF KClO3 USED
A) 1.3 g B) 2.0 g C) 15.5 g D) .011 g
14. A (L) HAS NBP=58.00C AND HEAT OF VAP.=77.0 kJ/mol
WHAT IS ITS VP AT 98.00C ?
A) 762 TORR B) 2.29 X 103 TORR C) 1.56 X 104 TORR D) 3.01 TORR
15. A SOLUTION CONSISTS OF 40.0 g OF SOLUTE( MOLAR MASS=250.0 g/mol)
IN 200.0 mL H2O (D=1.000 g/mL). CALCULATE ITS MOLALITY(m) AND
MOLE FRACTION (XSOLUTE).
A) m=.800 mol/kg X=.0142 B) m=.800 mol/kg X=.00889
C) m=1.25 mol/kg X=.0144 D) m=.160 mol/kg X=.016
16. A PURE SOLVENT HAS VP=124 torr AND MOLAR MASS=86.0 g/mol IF 5.00g SOLUTE(NON-ELECTROLYTE M=50.0 g/mol) ARE DISSOLVED IN 43.0g OF SOLVENT. WHAT IS VPSOLN AND VPL IN torr ?
A) 103, 21 B) 117, 7.0 C) 78, 36 D) 121, 4.0
17. WHAT IS THE NEW TB AND TF OF A SOLUTION CONSISTING OF
20.8 g KI IN 500.0 g WATER. FOR WATER KB=.51kgC/mol, KF=-1.86kgC/mol
A) 100.50C, -1.860C B) 101.00C, -3.720C
C) 98.00C, -7.440C D) 100.250C, -.930C
18. WHAT IS THE OSMOTIC PRESSURE OF A SOLUTION CONSISTING OF 10.0 g OF A NON-ELECTROLYTE SOLUTE WITH MOLAR MASS OF 50.0 g DISSOLVED IN SUFFICIENT WATER TO MAKE 400.0 mL OF SOLUTION AT 270C?
A) 12.3 torr B) 12.3 atm C) 24.6 atm D) 2.22 atm
19. A SOLUTION CONSISTS OF 5.00g OF A NON-ELECTROLYTE SOLUTE DISSOLVED IN 100.0g OF SOLVENT WITH KF=-8.00kgC/mol AND TF, SOLVENT=72.00C, TF, SOLUTION=62.00C. WHAT IS THE MOLAR MASS OF THE SOLUTE IN G/MOL
A) 80.0 B) 40.0 C) 1.60X102 D) 2.00X102
20. A SOLUTION CONSISTS OF 10.0mg OF A NON-ELECTROLYTE SOLUTE DISSOLVED IN SUFFICIENT WATER TO MAKE 2.00mL OF SOLUTION. THE OSMOTIC P OF THE SOLUTION=25.3 torr AT 270C. WHAT IS THE MOLAR MASS OF THE SOLUTE IN G/MOL?
A) 3.70X103 B) 424 C) 3.7x102 D) 741