Free Printable 1234

Worksheets

1234

Total questions: 39

Worksheet time: 1hrs 15mins

Name

Class

Date

When baking soda is added to vinegar, the solution produces a gas (carbon dioxide). A student is trying to see if there is a relationship between the amount of vinegar added and the amount of gas produced. He added one gram of baking soda to different amounts of vinegar in a test tube, and collected the gas in a balloon. The data is graphed.

What would be a valid conclusion if the student had added vinegar in the range of 0 - 10 ml only?

The amount of gas produced continues to increase as the amount of vinegar increases

Adding more than 10 ml of vinegar does not lead to additional gas production

The amount of gas produced depends only on the amount of baking soda in the test tube

There is no relationship between the amount of gas produced and the amount of vinegar added

If brass is 25% (by weight) copper, how many grams of copper are in 12 grams of brass?

3 g

37 g

48 g

300 g

Which of the following is a unit of volume?

$\frac{lb}{in^2}$

$cm^3$

miles

If a variable X is directly proportional to variable Y, it means…

as Y increases, X increases.

as Y increases, X decreases

there is no relationship between X and Y

none of these answers are correct

Density is defined as mass per unit volume or

d=\frac{m}{v}

Solve the density equation for variable v.

$v=d+m$

$v=\frac{d}{m}$

$v=dm$

$v=\frac{m}{d}$

$\frac{9cm^3}{3cm^2}$

$3cm^5$

$3cm^1$

$3cm^{-1}$

$3cm^{-5}$

If 2a = 3b, and a = 6, what does b equal?

0.000786 in scientific notation is

$7.86\ \times10^{-3}$

$7.86\times10^{-4}$

$7.86\times10^4$

$7.86\ \times10^3$

The part labelled W in the elemental information represents the

Atomic Mass

Symbol

Element Name

Atomic Number

10.

What is the Relative molecular mass (Mr) of ammonia (NH₃)?

17 g/mol

16.0 g/mol

15 g/mol

14.0 g/mol

11.

What is the mass unit commonly used in chemistry?

grams

pounds

kilograms

meter

12.

The ______________ yield is the maximum amount of product possible in a reaction. This determines the amount of product that should be produced in a perfect setting

Percent

actual

stoichiometry

theoretical

13.

When reacting Na with Cl₂, we calculated that the theoretical yield should be 13 grams. Our actual yield was 12.5 grams. What is the percent yield?

90.4%

104%

96.15%

1.04%

14.

Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.

1.16%

116%

85%

76%

15.

Using the following equation:
Fe₂O₃(s) + 3H₂(g) → 2Fe(s) + 3H₂O(l)
How many moles of iron can be made from 6 moles H₂?

4 moles Fe

6 moles Fe

9 moles Fe

2 moles Fe

16.

2H₂ + O₂ → 2H₂O
How many moles of water can be produced if 8 moles H₂ are used?

4 moles

8 moles

16 moles

2 moles

17.

N₂ + 3H₂ → 2NH₃
How many moles of hydrogen are needed to react with 2 moles of nitrogen?

18.

9. Complete the equation for the percent yield of a chemical reaction:
Percent yield=(________)÷(________)×100%

actual yield; theoretical yield

theoretical yield; actual yield

19.

How many moles is 4 grams of Calcium?

0.10 moles

10 moles

44 moles

160 moles

20.

What is Avogadro's Number?

602,000

23 x 10⁶

10 x 10²³

6.02 x 10²³

21.

If a chemist calculates the maximum amount of product that could be obtained in a chemical reaction, he or she is calculating the

theoretical yield

mole ratio

actual yield

percentage yield

22.

Using the following equation:
Fe₂O₃(s) + 3H₂(g) → 2Fe(s) + 3H₂O(l)
How many moles of iron can be made from 9 moles H₂?

4 moles Fe

6 moles Fe

9 moles Fe

2 moles Fe

23.

The limiting reactant is the reactant that __________ .

slows down the reaction

used up first

left over at the end of reaction

controls the speed of the reaction

24.

4NH₃+ 5O₂→ 4NO + 6H₂O

Based on reaction above, oxygen is a limiting reactant. Calculate the mass of NO formed if the mass of oxygen reacted is 1.80g.

0.37g

0.045g

1.35g

11.1g

25.

2NaClO₃ (s) → 2NaCl (s) + 3O₂ (g)

12.00 moles of NaClO₃ will produce how many grams of O₂?

96g

576g

288g

384g

26.

This is what you call a reactant that you have enough of. The one that DOES NOT run out.

Limiting Reactant

Excess Reactant

Highly Reactant

Super Reactant

27.

In a balanced equation, the ratio between the coefficient of any two substances is called the _______.

mole ratio

stoichiometry

limiting reactant

excess reactant

28.

Calculate the theoretical yield if given the actual yield and percent yield are 51.4g and 77.0% respectively.

25.6g

1.5g

15g

66.8g

29.

CuCl₂ + 2NaNO₃--> Cu(NO₃)₂ +2NaCl

In the reaction above, 15 grams of copper (II) chloride react with 20 grams of sodium nitrate. The expected mass of NaCl formed should be 13.104 g, but only 7.000 g of NaCl obtained. How many grams is the actual yield in the experiment?

13.104 g

7.000 g

15.00 g

20.00

30.

CuCl₂ + 2NaNO₃--> Cu(NO₃)₂ +2NaCl

In the reaction above, 15 grams of copper (II) chloride react with 20 grams of sodium nitrate. The expected mass of NaCl formed should be 13.104 g, but only 7.000 g of NaCl obtained. Calculate the percentage yield of the experiment.

90.00 %

53.42%

100%

7.00%

31.

An impure sample of Na₂SO₄ has a mass of 1.56 grams. This sample is dissolved and allowed to react with BaCl₂ solution. The reaction produced of 2.15 grams BaSO₄. Calculate the percentage of Na₂SO₄ in the original sample.

83.89

85.0

90.0

45.6

32.

CH₄ + 2O₂ → CO₂ + 2H₂O

32 grams of CH₄ was added to the above reaction. Calculate the theoretical yield of CO₂.

44 g

88 g

32 g

36 g

33.

If the percent yield in a reaction is 75% and the actual amount of product obtained was 12 g, what was the theoretical yield?

10 g

16 g

20 g

18 g

34.

2Fe₂O₃ + C → Fe + 3CO₂

You add 28 grams of carbon. You find the actual yield to be 181.2 grams of CO₂. What is the percent yield of CO₂? (Hint: calculate theoretical yield of CO₂ first)

58.83%

308%

6435%

15.5

35.

If you burn 2.5 moles of methane (CH4) according to the following reaction,

CH₄ (g) + 2 O₂ (g) → CO₂ (g) + 2 H₂O (g)

How many grams of carbon dioxide are produced?

(a)

36.

Aspirin (C₉H₈O₄) can be made from salicylic acid (C₇H₆O₃) and acetic anhydride (C₄H₆O₃). Suppose you mix 13.2 g of salicylic acid with an excess of acetic anhydride and obtain 5.9 g of aspirin and some water. Calculate the percent yield of aspirin in this reaction. The balanced equation has been provided for you.

2 C₇H₆O₃ (s) + C₄H₆O₃ (l) → 2 C₉H₈O₄ (s) + H₂O (l)

Calculate the Theoretical Yield of Aspirin?

(a)

37.

Iron metal (Fe) can be obtained from iron ore (Fe₂O₃) by the following reaction, Fe₂O₃ (s) + 3CO (g) → 2Fe (s) + 3CO₂ (g)

How many grams of iron ore are needed to obtain 92.8 g of iron metal?

(a)

38.

In an experiment, 10.0 g of magnesium reacted with excess hydrochloric acid forming magnesium chloride.

Mg(s) + 2HCl(aq) → MgCl₂ + H₂(g)

At the completion of the reaction, 29.5 g of magnesium chloride was produced. Calculate the theoretical yield?

(a)

39.

A piece of magnesium burns in the presence of oxygen, forming magnesium oxide. Write the equation and balance it.

2 Mg + O₂ -----> 2 MgO

how many moles of oxygen are needed to completely react with 12 moles of magnesium?

(a)

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Total questions: 39

Worksheet time: 1hrs 15mins

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