Grams To Atoms And Atoms To Grams Practice Quiz
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How many grams are there in 1.3846 x 1024 atom of Silicon?
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64.607 g
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33.51 g
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61.025 g
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361.25
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Get ready to unleash your inner chemist and go on a journey through the zany universe of atoms and grams with our uproariously entertaining "Atoms to Grams" quiz! Brace yourself for a wild ride as you navigate through a maze of molecular madness, where the only thing heavier than the elements is the laughter echoing through the laboratory.
Ever wondered See morehow many moles of avocado toast you'd need to reach critical mass? Or perhaps pondered the existential question of whether a burrito can truly achieve stoichiometric perfection? Fear not, intrepid quiz-taker, for we've got the answers you never knew you needed!
From deciphering the cryptic hieroglyphics of chemical equations to mastering the art of balancing atoms like a seasoned tightrope walker, this quiz will put your chemistry chops to the test. But fear not, even if your knowledge of Avogadro's number is a bit fuzzy, we promise there'll be plenty of laughs along the way. So gather your fellow science enthusiasts, or perhaps just your pet rock named Bunsen, and prepare to embark on the chemistry adventure of a lifetime.
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- 2.
How many grams are there in 2.0468 x 1025 atoms of NaCl? (The molar mass of NaCl is 58.44g)
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19.96 g
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116 x 10^25 g
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1988.59 g
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1256.99 g
Correct Answer
A. 1988.59 g -
- 3.
How many atoms are there in 25.0 g of magnesium (Mg)? (Molar mass of magnesium is 24.31 g/mol)
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6.02 x 10^23 atoms
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1.45 x 10^24 atoms
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1.03 x 10^24 atoms
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1.00 x 10^24 atoms
Correct Answer
A. 6.02 x 10^23 atomsExplanation
The process begins by determining the number of atoms present in 25.0 g of magnesium. We employ the molar mass of magnesium, which is 24.31 g/mol. Utilizing Avogadro's number, we ascertain that one mole of magnesium contains 6.022 x 10^23 atoms. Employing the formula Number of atoms = (Mass (g) ÷ Molar mass (g/mol)) × Avogadro's number, we substitute the given values to derive the number of atoms. This yields 6.02 x 10^23 atoms, aligning with option a) 6.02 x 10^23 atoms.Rate this question:
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- 4.
How many atoms are there in 70.554 g of Sulfur?
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140 atoms
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6.02 x 10^23atoms
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1.32 x 10^25 atoms
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1.32 x 10^24 atoms
Correct Answer
A. 1.32 x 10^24 atomsExplanation
To change from grams to atoms requires TWO steps:
1st: change to moles: Take your grams and divide by molar mass.
70.554 g divided by 32.07 g = 2.2 moles
2nd: Change to atoms: Take your moles and multiply by Avogadro’s number:
2.2 x 6.02 x 10^23 = 1.32 x 10^24Rate this question:
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- 5.
How many grams are in 2.2274 x 1025 atoms of CO2?
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1,629 g
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162.84 g
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120.45 g
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198.5 g
Correct Answer
A. 1,629 gExplanation
Firstly, we recognize that CO2 consists of one carbon (C) atom and two oxygen (O) atoms. Carbon has a molar mass of around 12.01 grams per mole, and oxygen has a molar mass of about 16.00 grams per mole.
To find the total molar mass of CO2, we add the molar masses of carbon and two oxygen atoms together. This gives us approximately 44.01 grams per mole.
Next, we convert the number of atoms given to moles. This conversion utilizes Avogadro's number, which is about 6.022 x 10^23 atoms per mole. By dividing the given number of atoms by Avogadro's number, we find the number of moles, approximately 37 moles.
Finally, to find the mass in grams, we multiply the number of moles by the molar mass. This yields a result of approximately 1.63 x 10^3 grams which is approximately 1629 g.
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- 6.
How many atoms are there in 118.082 g of Potassium?
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118.082 atoms
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6.02 x 10^23 atoms
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1.818 x 10^24 atoms
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1.18 x 10^23 atoms
Correct Answer
A. 1.818 x 10^24 atomsExplanation
To change from grams to atoms requires TWO steps:
1st: change to moles: Take your grams and divide by molar mass.
118.082 g divided by 39.1 g = 3.02 moles
2nd: Change to atoms: Take your moles and multiply by Avogadro’s number:
3.02 x 6.02 x 10^23 = 1.818 x 10^24Rate this question:
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- 7.
What is the correct conversion factor to use when converting grams of a substance to atoms?
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Avogadro's number
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Molar mass
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Density
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Both Avogadro's number and molar mass
Correct Answer
A. Molar massExplanation
To convert grams to atoms, you need to use both Avogadro's number and the molar mass of the substance. First, convert grams to moles using the molar mass. Then, convert moles to atoms using Avogadro's number.Rate this question:
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- 8.
How many grams are in 2.1672 x 1025 atoms of Glucose C6H12O6? (The molar mass of glucose is: 180 g/mol)
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568 g
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1,230 g
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540 g
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6498 g
Correct Answer
A. 6498 g -
- 9.
How many atoms are there in 80.223 g of Magnesium?
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1.99 x 10^24 atoms
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6.02 x 10^24 atoms
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2.4 x 10^24 atoms
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3.3 x 10^23 atoms
Correct Answer
A. 1.99 x 10^24 atomsExplanation
To change from grams to atoms requires TWO steps: 1st: change to moles: Take your grams and divide by molar mass. 80.223 g divided by 24.31 g = 3.3 moles 2nd: Change to atoms: Take your moles and multiply by Avogadro’s number: 3.3 x 6.02 x 10^23 = 1.99 x 10^24 atomsRate this question:
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- 10.
How many atoms are there in 148.375 g of LiCl? (Hint: How many atoms are found in each LiCl?) (Use molar mass for LiCl = 42.394)
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6.02 x 10^23 atoms
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3.4 x 10^23 atoms
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2.107 x 10^24 atoms
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4.26 x 10^24 atoms
Correct Answer
A. 4.26 x 10^24 atoms -
- 11.
How many atoms are there in 18.02 g of H2O? (Hint: How many atoms are the in each molecule of H2O?)
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1.8 x 10^23 atoms
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6.02 x 10^24 atoms
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1.8 x 10^24 atoms
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6.02 x 10^23 atoms
Correct Answer
A. 1.8 x 10^24 atoms -
- 12.
What is the mass in grams of 4.50 x 10^22 atoms of oxygen (O)? (Molar mass of oxygen is 16.00 g/mol)
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2.16 x 10^-22 grams
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4.50 x 10^-22 grams
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3.20 x 10^-21 grams
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1.44 x 10^-21 grams
Correct Answer
A. 1.44 x 10^-21 gramsExplanation
To ascertain the mass in grams of 4.50 x 10^22 atoms of oxygen, we integrate the molar mass of oxygen (16.00 g/mol) and Avogadro's number (6.022 x 10^23 atoms/mol). Employing the formula Mass (g) = Number of atoms × (Molar mass (g/mol) ÷ Avogadro's number), we substitute the provided values to compute the mass. This yields 1.44 x 10^-21 grams, corresponding to option d) 1.44 x 10^-21 grams.Rate this question:
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- 13.
What is the mass in grams of 4.20 x 10^23 atoms of sulfur (S)? (Molar mass of sulfur is 32.07 g/mol)
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5.55 x 10^-21 grams
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2.62 x 10^-20 grams
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4.77 x 10^-21 grams
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2.54 x 10^-20 grams
Correct Answer
A. 2.62 x 10^-20 gramsExplanation
To determine the mass in grams of 4.20 x 10^23 atoms of sulfur, we integrate the molar mass of sulfur (32.07 g/mol) and Avogadro's number (6.022 x 10^23 atoms/mol). Applying the formula Mass (g) = Number of atoms × (Molar mass (g/mol) ÷ Avogadro's number), we substitute the provided values to compute the mass. This yields 2.62 x 10^-20 grams, corresponding to option b) 2.62 x 10^-20 grams.Rate this question:
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- 14.
How many atoms are there in 2.00 g of chlorine (Cl)? (Molar mass of chlorine is 35.45 g/mol)
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3.38 x 10^22 atoms
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1.13 x 10^23 atoms
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1.14 x 10^22 atoms
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6.02 x 10^23 atoms
Correct Answer
A. 1.13 x 10^23 atomsExplanation
Determining the number of atoms in 2.00 g of chlorine initiates by incorporating the molar mass of chlorine (35.45 g/mol) and Avogadro's number (6.022 x 10^23 atoms/mol). Utilizing the formula Number of atoms = (Mass (g) ÷ Molar mass (g/mol)) × Avogadro's number, we input the given values to calculate the number of atoms. Consequently, the result is 1.13 x 10^23 atoms, which aligns with option b) 1.13 x 10^23 atoms.Rate this question:
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- 15.
What is the mass in grams of 3.01 x 10^24 atoms of carbon (C)? (Molar mass of carbon is 12.01 g/mol)
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2.50 x 10^-24 grams
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5.02 x 10^-23 grams
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5.02 x 10^-22 grams
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3.01 x 10^24 grams
Correct Answer
A. 5.02 x 10^-22 gramsExplanation
To determine the mass in grams of 3.01 x 10^24 atoms of carbon, we first utilize the concept of molar mass, representing the mass of one mole of a substance. Carbon's molar mass is 12.01 g/mol. We then employ Avogadro's number, which states that one mole of any substance contains 6.022 x 10^23 atoms. Using the formula Mass (g) = Number of atoms × (Molar mass (g/mol) ÷ Avogadro's number), we substitute the given values to calculate the mass. Consequently, the result is 5.02 x 10^-22 grams, corresponding to option c) 5.02 x 10^-22 grams.Rate this question:
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Oct 30, 2024Quiz Edited by
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Jul 30, 2010Quiz Created by
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