# Moles Practice 2 (10pts)

Approved & Edited by ProProfs Editorial Team
The editorial team at ProProfs Quizzes consists of a select group of subject experts, trivia writers, and quiz masters who have authored over 10,000 quizzes taken by more than 100 million users. This team includes our in-house seasoned quiz moderators and subject matter experts. Our editorial experts, spread across the world, are rigorously trained using our comprehensive guidelines to ensure that you receive the highest quality quizzes.
| By Afua Nti
A
Afua Nti
Community Contributor
Quizzes Created: 4 | Total Attempts: 4,410
Questions: 10 | Attempts: 241

Settings

Changing from and into moles

• 1.

### How many moles are in 58g of sodium cholride (NaCl)?

• A.

2 moles

• B.

2.0 moles

• C.

1 moles

• D.

1.0 moles

D. 1.0 moles
Explanation
The molar mass of sodium chloride (NaCl) is 58.5 g/mol. To calculate the number of moles, we divide the given mass (58g) by the molar mass (58.5 g/mol). This gives us 1 mole of sodium chloride.

Rate this question:

• 2.

### 2.5 moles of KF, potassium floride would be equal to how many grams?

• A.

145g

• B.

150g

• C.

145.25g

• D.

140g

B. 150g
Explanation
The molar mass of KF (potassium fluoride) is 58.1 g/mol. To convert moles to grams, we multiply the number of moles by the molar mass. Therefore, 2.5 moles of KF would be equal to 2.5 moles x 58.1 g/mol = 145.25g. Hence, the correct answer is 145.25g, not 150g.

Rate this question:

• 3.

### How many moles are in 114g of iron (III) nitrate (Fe(NO3)3?

• A.

0.25 mole

• B.

0.500 mole

• C.

0.50 mole

• D.

0.250 mole

B. 0.500 mole
Explanation
One mole of any substance contains Avogadro's number of particles, which is approximately 6.022 x 10^23. To find the number of moles in a given mass of a substance, we need to divide the mass by the molar mass of that substance. The molar mass of iron (III) nitrate (Fe(NO3)3) can be calculated by adding up the atomic masses of its constituent elements. In this case, the molar mass of Fe(NO3)3 is approximately 241.86 g/mol. Therefore, 114g of Fe(NO3)3 is equal to 114/241.86 = 0.471 moles. Since the answer choices are given in increments of 0.25, the closest option is 0.500 mole.

Rate this question:

• 4.

### 25.0mol of calcium sulfate (CaSO4 ) will produce how many grams?

• A.

1800g

• B.

3200g

• C.

3180g

• D.

3180.g

C. 3180g
Explanation
Calcium sulfate (CaSO4) has a molar mass of 136.14 g/mol. To find the mass of 25.0 mol of calcium sulfate, we can multiply the molar mass by the number of moles. Therefore, 25.0 mol x 136.14 g/mol = 3403.5 g. However, since the question asks for the mass in grams and the answer choices are all in grams, we can round the result to the nearest gram, which is 3180g.

Rate this question:

• 5.

### How many compounds of sodium chloride (NaCl) are in 1.5 moles?

• A.

6.02 x 10^23 compounds

• B.

6.0 x 10^23 compounds

• C.

9.03 x 10^23 compounds

• D.

9.0 x 10^23 compounds

D. 9.0 x 10^23 compounds
Explanation
In 1.5 moles of sodium chloride (NaCl), there are 9.0 x 10^23 compounds. This is because 1 mole of any substance contains 6.02 x 10^23 particles (Avogadro's number). Therefore, 1.5 moles would contain 1.5 times that amount, which is 9.0 x 10^23 compounds.

Rate this question:

• 6.

### There are how many molecules in 5.0  moles of water (H2O)?

• A.

3.0 x 10^23 molecules

• B.

3.01 x 10^23 molecules

• C.

3.0 x 10^24 molecules

• D.

3.01 x 10^24 molecules

C. 3.0 x 10^24 molecules
Explanation
The correct answer is 3.0 x 10^24 molecules. One mole of any substance contains Avogadro's number (6.022 x 10^23) of particles. Since we have 5.0 moles of water, we can multiply the number of moles by Avogadro's number to find the number of molecules. Therefore, 5.0 moles x 6.022 x 10^23 molecules/mole = 3.0 x 10^24 molecules.

Rate this question:

• 7.

### If you have 1.2 x10^24 atoms of hydrogen how many moles do you have?

• A.

1 mole

• B.

1.0 mole

• C.

2 mole

• D.

2.0 mole

D. 2.0 mole
Explanation
The given question asks for the number of moles of hydrogen atoms when there are 1.2 x 10^24 atoms of hydrogen. To determine the number of moles, we use Avogadro's number, which states that 1 mole of a substance contains 6.022 x 10^23 particles. In this case, since we have 1.2 x 10^24 atoms of hydrogen, we can divide this number by Avogadro's number to find the number of moles. The result is 2.0 mole, indicating that there are 2 moles of hydrogen atoms.

Rate this question:

• 8.

### If a computer was to count 3.5 x 10^12 dollars how many moles of dollars whoud you have?

• A.

5.8 x 10^-12 mole

• B.

1.8 x 10^-11 mole

• C.

1.8 x 10^11 mole

• D.

5.8 x 10^10 mole

A. 5.8 x 10^-12 mole
• 9.

### What is the volume of 4.50moles of nitrogen gas at STP?Assume the molar volume of any gas at STP is 22.4 L/mol

• A.

100L

• B.

100.8L

• C.

100.L

• D.

101L

D. 101L
Explanation
The molar volume of any gas at STP is given as 22.4 L/mol. Therefore, to find the volume of 4.50 moles of nitrogen gas at STP, we can multiply the number of moles by the molar volume. 4.50 moles multiplied by 22.4 L/mol gives us a volume of 100.8 L. Therefore, the correct answer is 100.8L.

Rate this question:

• 10.

### How large would a tank have to be if it holds 5.00 mol of carbon dioxide at STP? (Assume molar volume of all gases to be 22.4 L/mol at STP)

• A.

220L

• B.

220.L

• C.

112L

• D.

112.0L

C. 112L
Explanation
At STP (Standard Temperature and Pressure), the molar volume of all gases is 22.4 L/mol. Since the question states that the tank holds 5.00 mol of carbon dioxide, we can calculate the volume by multiplying the molar volume by the number of moles: 22.4 L/mol * 5.00 mol = 112 L. Therefore, the tank would have to be 112L in size to hold 5.00 mol of carbon dioxide at STP.

Rate this question:

Quiz Review Timeline +

Our quizzes are rigorously reviewed, monitored and continuously updated by our expert board to maintain accuracy, relevance, and timeliness.

• Current Version
• Mar 20, 2023
Quiz Edited by
ProProfs Editorial Team
• Dec 05, 2016
Quiz Created by
Afua Nti

Related Topics

×

Wait!
Here's an interesting quiz for you.