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What is the mass ratio of fluorine to boron in a boron trifluoride molecule? 1.8 to 1 3.0 to 1 3.5 to 1 5.3 to 1 6.0 t

What is the mass ratio of fluorine to boron in a boron trifluoride molecule? 1.8 to 1 3.0 to 1 3.5 to 1 5.3 to 1 6.0 to 1. D. A hydrocarbon sample with a mass of 6 grams underwent c ombustion, producing 11 grams of carbon dioxide. If all

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What is the mass ratio of fluorine to boron in a boron trifluoride molecule? 1.8 to 1 3.0 to 1 3.5 to 1 5.3 to 1 6.0 t

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  1. What is the mass ratio of fluorine to boron in a boron trifluoride molecule? 1.8 to 1 3.0 to 1 3.5 to 1 5.3 to 1 6.0 to 1 D

  2. A hydrocarbon sample with a mass of 6 grams underwent combustion, producing 11 grams of carbon dioxide. If all of the carbon initially present in the compound was converted to carbon dioxide, what was the percent of carbon, by mass, in the hydrocarbon sample? 25 % 33 % 50 % 66 % 75 % C

  3. What is the mass of oxygen in 148 grams of calcium Hydroxide (Ca(OH)2)? 16 grams 24 grams 32 grams 48 grams 64 grams E

  4. An ion containing only oxygen and chlorine is 31 % oxygen By mass. What is the empirical formula? ClO – ClO2 – ClO3 – ClO4 – Cl2O- A

  5. A sample of propane, C3H8, was completely burned in air at STP. The reaction occurred as shown below C3H8 + O2 3O2 + 4 H2O If 67.2 liters of CO2 were produced and all of the carbon in the CO2 came from the propane, what was the mass of propane sample? 11 grams 22 grams 33 grams 44 grams 55 grams D

  6. What is the percent composition by mass of the elements in the Compound NaNO3? 20 % Na, 20 % N, 60 % O 23 % Na, 14 % N, 48 % O 23 % Na, 14 % N, 63 % O 27 % Na, 16 % N, 57 % O 36 % Na, 28 % N, 36 % O D

  7. CaCO3 (s)  CaO (s) + CO2 (g) A sample of pure CaCO3 was heated and decomposed according to The reaction given above. If 28 grams of CaO were produced by the Reaction, what was the initial mass of CaCO3? 14 grams 25 grams 42 grams 50 grams 84 grams D

  8. A sample of a hydrate of CuSO4 with a mass of 250 grams was heated until all of the water was removed. The sample was then weighed and found to have a mass of 160 grams. What is the formula for the hydrate? CuSO4 . 10 H2O CuSO4 . 7 H2O CuSO4 . 5 H2O CuSO4 . 2 H2O CuSO4 . H2O C

  9. A compound containing only sulfur and oxygen is 50 % sulfur by weight. What is the empirical formula of the compound? SO SO2 SO3 S2O S3O B

  10. 2Na(s) + 2H2O (l)  2NaOH (aq) + H2 (g) Elemental sodium reacts with water to form hydrogen gas as shown above. If a sample of sodium reacts completely to form 20 liters of hydrogen gas, Measured at standard temperature and pressure, what was the mass of Sodium? 5 grams 10 grams 20 grams 30 grams 40 grams E

  11. ZnSO3 (s)  ZnO (s) + SO2 (g) What is the STP volume of SO2 gas produced by the above reaction When 145 grams of ZnSO3 are consumed? 23 liters 36 liters 45 liters 56 liters 90 liters A

  12. A hydrocarbon contains 75 % carbon by mass. What is the empirical Formula for the compound? CH2 CH3 CH4 C2H5 C3H8 C

  13. CaCO3 (s) + 2H+ (aq)  Ca 2+ (aq) + H2O (l) + CO2 (g) If the reaction above took place at STP and 150 grams of CaCO3 (s) were consumed, what was the volume of CO2 (g) At STP? 11L 22 L 34 L 45 L 56 L B

  14. A sample of a hydrate of BaCl2 with a mass of 61 grams was heated Until all the water was removed. The sample was then weighed and Found to have a mass of 52 grams. What is the formula for the Hydrate? BaCl2 . 5H2O BaCl2 4 H2O BaCl2 3 H2O BaCl2 2H2O BaCl2 H2O D

  15. When chlorine gas is combined with fluorine gas, a compound Is formed that is 38 % chlorine and 62 % fluorine. What is the Empirical formula of the compound? ClF ClF2 ClF3 ClF5 ClF7 c

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