I don’t know how to do this because I was sick when this was thought. If someone could please explain how to do or set up the first problem.
A. Measure out 0.130 moles of salt (NaCl) into a blue, dry cup. You need to convert to mass in grams. Show work:
B. Put 4.03x10^23 molecules of water into a clear cup. You need to convert to mass in grams. Show work:
C. Obtain a small sample of metal from your teacher. Determine how many atoms it contains. Show work: the metal sample weighs 142g
a. mass=moles*formulaMassNaCl
b. mass=moles*molmass=numbermolecules*molmass/avagNumber
c. you have to know what kind of metal.
atoms=mass*avagnumber/molmassmetal
A. To convert the number of moles of NaCl to mass in grams, you need to use the molar mass of NaCl. The molar mass of NaCl is the sum of the atomic masses of sodium (Na) and chlorine (Cl). The atomic mass of sodium is 22.99 g/mol, and the atomic mass of chlorine is 35.45 g/mol.
To calculate the molar mass of NaCl, you add the atomic masses of sodium and chlorine:
Molar mass of NaCl = atomic mass of Na + atomic mass of Cl
Molar mass of NaCl = 22.99 g/mol + 35.45 g/mol
Molar mass of NaCl = 58.44 g/mol
Now, to convert moles of NaCl to grams, you can use the following equation:
Mass (in grams) = Number of moles * Molar mass
In this case, since you have 0.130 moles of NaCl, you can calculate the mass in grams as follows:
Mass (in grams) = 0.130 moles * 58.44 g/mol
Mass (in grams) = 7.5892 grams (rounding to four decimal places)
Therefore, 0.130 moles of salt (NaCl) is equivalent to approximately 7.5892 grams.
B. To convert the number of water molecules to mass in grams, you need to use the concept of molar mass for water (H2O). The molar mass of water is the sum of the atomic masses of hydrogen (H) and oxygen (O). The atomic mass of hydrogen is 1.008 g/mol, and the atomic mass of oxygen is 16.00 g/mol.
To calculate the molar mass of water, you add the atomic masses of hydrogen and oxygen:
Molar mass of H2O = (2 * atomic mass of H) + atomic mass of O
Molar mass of H2O = (2 * 1.008 g/mol) + 16.00 g/mol
Molar mass of H2O = 18.02 g/mol
Now, to convert the number of molecules of water (4.03x10^23) to grams, you can use the following equation:
Mass (in grams) = Number of molecules * (1 mole / Avogadro's number) * Molar mass
Note: Avogadro's number is approximately 6.022 x 10^23 molecules/mol.
In this case, using the given Avogadro's number and the molar mass of water, you can calculate the mass in grams as follows:
Mass (in grams) = 4.03x10^23 molecules * (1 mol / 6.022x10^23 molecules) * 18.02 g/mol
Mass (in grams) = 1.3381 grams (rounding to four decimal places)
Therefore, 4.03x10^23 molecules of water is equivalent to approximately 1.3381 grams.
C. To determine the number of atoms in the metal sample, you need to use the concept of moles and Avogadro's number. Avogadro's number is approximately 6.022 x 10^23 atoms/mol.
Given that the metal sample weighs 142 grams, you can calculate the number of moles using the equation:
Number of moles = Mass (in grams) / Molar mass
Since the mass of the metal sample is provided as 142 grams, we need to know the molar mass of the metal to proceed with the calculation. The molar mass of the metal will depend on the specific metal, which is not provided in the question.