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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 to 1 PowerPoint PPT Presentation


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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 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 to 1

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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 to 1

D


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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


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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


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An ion containing only oxygen and chlorine is 31 % oxygen

By mass. What is the empirical formula?

ClO –

ClO2 –

ClO3 –

ClO4 –

Cl2O-

A


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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


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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


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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


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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


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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


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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


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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


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A hydrocarbon contains 75 % carbon by mass. What is the empirical

Formula for the compound?

CH2

CH3

CH4

C2H5

C3H8

C


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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


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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


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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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