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************************************************************************* BSAC General Chemistry I QUIZ 1 Name__________________ID__________ *************************************************************************.

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  1. ************************************************************************************************************************************************** • BSAC General Chemistry I QUIZ 1 Name__________________ID__________ • ************************************************************************* Q1: 50g of an unknown fluorocarbon gas at 75 ºC and 180 Torr pressure was found to occupy 60.27 L volume. Calculate the molar mass of the gas and hence decide on its formula. What is the unknown? A) C3F6 B) C2F4 C) CF4D) C2F6 E) C6F6 B Q2: By referring to the solubility table (attached), decide which of the following solution mixings would NOT produce a precipitate: A) KOH(aq) + Al(NO3)3 (aq)  B)Ag2SO4 (aq) + HF (aq)  C) (NH4)2S (aq) + Ba(OH)2 (aq)  D) CaCl2 (aq) + K2CO3 (aq)  * * * * * Q3: When 25 mL of HCl (2.00 mol/L) is added to 30 mL AgNO3(1.50 mol/L) a white precipitate instantly formed. What was the precipitate? Q4: What is the maximum possible mass (theoretical yield) of precipitate salt that is recoverable by filtration? * * * * * Q5: Glycine (H2N-CH2-COOH) (13.5 g) was dissolved in 250 mL water (molal freezing point depression constant = 1.86 Kkg/mol). What was the freezing point of the solution? Q6: In the space below, write the full equation (including all ions) for the mixing of lead (II) perchlorate and iron(III) chloride: ____________________________________ ______________________________________ (4 + 2 + 2 + 4 + 4 + 4 marks) TOTAL: 20 marks C A) HNO3 B) AgClC) AgOH D) AgCl2E) Ag2(SO4)2 B A) 8.93 gB) 8.04 gC) 7.17 g D) 4.56 gE) 6.45 g E A) +0.72 ºC B) -0.72 ºCC) -1.34 ºC D) -1.68 ºC E) -0.33 ºC C 3Pb(ClO4)2 + 2FeCl3 3PbCl2(s) + 2Fe(ClO4)3

  2. ************************************************************************************************************************************************** • BSAC General Chemistry I QUIZ 2 Name__________________ID__________ • ************************************************************************* Q1: 30g of an unknown fluorocarbon gas at 65 ºC and 270 Torr pressure was found to occupy 26.61 L volume. Calculate the molar mass of the gas and hence decide on its formula. What is the unknown? A) C5F10 B) C2F2 C) CF4D) C7F14E) C2F6 C Q2: By referring to the solubility table (attached), decide which of the following solution mixings would NOT produce a precipitate: A) NaOH (aq) + (NH4)2S (aq)  B)K2CO3 (aq) + BaCl2 (aq)  C) KOH(aq) + Cu(NO3)2 (aq)  D) Ag2SO4 (aq) + HBr (aq)  * * * * * Q3: When 25 mL of HCl (1.60 mol/L) is added to 40 mL AgNO3(1.40 mol/L) a white precipitate instantly formed. What was the precipitate? Q4: What is the maximum possible mass (theoretical yield) of precipitate salt that is recoverable by filtration? * * * * * Q5: Urea (H2N-CO-NH2) (13.5 g) was dissolved in 250 mL water (molal freezing point depression constant = 1.86 Kkg/mol). What was the freezing point of the solution? Q6: In the space below, write the full equation (including all ions) for the mixing of ammonium phosphate and copper (II) chloride: ____________________________________ ______________________________________ (4 + 2 + 2 + 4 + 4 + 4 marks) TOTAL: 20 marks A A) HNO3 B) AgCl2 C) AgOH D) AgCl E) Ag2(SO4)2 D A) 8.02 gB) 5.73 gC) 3.75 g D) 2.56 gE) 11.45 g B A) -1.67 ºC B) -1.76 ºCC) -0.42 ºC D) -0.24 ºC E) +2.40 ºC A 2(NH4)3PO4 + 3CuCl2 6NH4Cl + Cu3(PO4)2(s)

  3. ************************************************************************************************************************************************** • BSAC General Chemistry I QUIZ 3 Name__________________ID__________ • ************************************************************************* Q1: 86g of an unknown fluorocarbon gas at -25 ºC and 980 Torr pressure was found to occupy 9.046 L volume. Calculate the molar mass of the gas and hence decide on its formula. What is the unknown? A) C3F6 B) C2F6 C) C4F6D) CF4E) C6F10 A Q2: By referring to the solubility table (attached), decide which of the following solution mixings would NOT produce a precipitate: A) HI (aq) + Ag3PO4 (aq)  B) LiClO3(aq) + Sb(NO3)3 (aq)  C) K2S (aq) + CuSO4 (aq)  D) (NH4)2CO3 (aq) + Sr(OH)2 (aq)  * * * * * Q3: When 60 mL of HCl (2.00 mol/L) is added to 50 mL AgNO3(3.00 mol/L) a white precipitate instantly formed. What was the precipitate? Q4: What is the maximum possible mass (theoretical yield) of precipitate salt that is recoverable by filtration? * * * * * Q5: Glucose(C6H12O6) (3.5 g) was dissolved in 200 mL water (molal freezing point depression constant = 1.86 Kkg/mol). What was the freezing point of the solution? Q6: In the space below, write the full equation (including all ions) for the mixing of caesium carbonate and tin (II) chloride: ____________________________________ ______________________________________ (4 + 2 + 2 + 4 + 4 + 4 marks) TOTAL: 20 marks B A) Ag2(SO4)2 B) Ag2ClC) AgCl D) Ag2O E) HNO3 C A) 17.2 gB) 21.5 gC) 11.7 g D) 24.6 gE) 6.1 g A A) -0.04 ºC B) +0.12 ºCC) -1.12 ºC D) -0.81 ºC E) -0.18 ºC E Cs2(CO3)2 + 2SnCl2 2CsCl + 2SnCO3 (s)

  4. ************************************************************************************************************************************************** • BSAC General Chemistry I QUIZ 4 Name__________________ID__________ • ************************************************************************* Q1: 250g of an unknown fluorocarbon vapour at 175 ºC and 50 Torr pressure was found to occupy 750.8 L volume. Calculate the molar mass of the gas and hence decide on its formula. What is the unknown? A) C2F4B) CF4C) C4F8D) C6F12 E) C6F6 E Q2: By referring to the solubility table (attached), decide which of the following solution mixings would NOT produce a precipitate: A) Li2CO3 (aq) + MgCl2 (aq)  B)AgClO3 (aq) + HBr (aq)  C) CsOH(aq) + Fe2(NO3)3 (aq)  D) BaS (aq) + CrBr2 (aq)  * * * * * Q3: When 105 mL of HCl (0.10 mol/L) is added to 125 mL AgNO3(0.05 mol/L) a white precipitate instantly formed. What was the precipitate? Q4: What is the maximum possible mass (theoretical yield) of precipitate salt that is recoverable by filtration? * * * * * Q5: Sucrose (C12H22O11) (10.00 g) was dissolved in 150 mL water (molal freezing point depression constant = 1.86 Kkg/mol). What was the freezing point of the solution? Q6: In the space below, write the full equation (including all ions) for the mixing of barium chloride and iron(III) sulphate: ____________________________________ ______________________________________ (4 + 2 + 2 + 4 + 4 + 4 marks) TOTAL: 20 marks C A) HNO3 B) AgClC) AgOH D) AgCl2E) Ag2(SO4)2 B A) 0.06 gB) 0.90 gC) 1.10 g D) 1.50 gE) 6.25 g B A) +0.10 ºC B) -0.36 ºCC) -0.10 ºC D) -0.02 ºC E) -1.33 ºC B Fe2(SO4)3 + 3BaCl2 2FeCl3(s) + 3BaSO4(s)

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