To solve this problem, we need to use Avogadro's number, which states that one mole of any substance contains 6.022 x 10^23 entities (atoms, molecules, etc.).

Step 1: Determine the molar mass of nitrogen gas (N2). Nitrogen has an atomic mass of approximately 14.01 g/mol. Since nitrogen gas is diatomic (N2), we multiply this by 2 to get 28.02 g/mol.

Step 2: Convert the mass of nitrogen gas in the balloon to moles. We do this by dividing the given mass by the molar mass.

12.88 g / 28.02 g/mol = 0.46 moles

Step 3: Use Avogadro's number to find the number of molecules.

0.46 moles * 6.022 x 10^23 molecules/mole = 2.77 x 10^23 molecules

So, the answer is D. 2.77 x 10^23 molecules.

Question

To solve this problem, we need to use Avogadro's number, which states that one mole of any substance contains 6.022 x 10^23 entities (atoms, molecules, etc.).

Step 1: Determine the molar mass of nitrogen gas (N2). Nitrogen has an atomic mass of approximately 14.01 g/mol. Since nitrogen gas is diatomic (N2), we multiply this by 2 to get 28.02 g/mol.

Step 2: Convert the mass of nitrogen gas in the balloon to moles. We do this by dividing the given mass by the molar mass.

12.88 g / 28.02 g/mol = 0.46 moles

Step 3: Use Avogadro's number to find the number of molecules.

0.46 moles * 6.022 x 10^23 molecules/mole = 2.77 x 10^23 molecules

So, the answer is D. 2.77 x 10^23 molecules.

Knowee AI · Accepted Answer

To solve this problem, we need to use Avogadro's number, which states that one mole of any substance contains 6.022 x 10^23 entities (atoms, molecules, etc.).

Step 1: Determine the molar mass of nitrogen gas (N2). Nitrogen has an atomic mass of approximately 14.01 g/mol. Since nitrogen gas is diatomic (N2), we multiply this by 2 to get 28.02 g/mol.

Step 2: Convert the mass of nitrogen gas in the balloon to moles. We do this by dividing the given mass by the molar mass.

12.88 g / 28.02 g/mol = 0.46 moles

Step 3: Use Avogadro's number to find the number of molecules.

0.46 moles * 6.022 x 10^23 molecules/mole = 2.77 x 10^23 molecules

So, the answer is D. 2.77 x 10^23 molecules.

A balloon contains 12.88 g of nitrogen gas (N2). How many nitrogen molecules are in the balloon?The Periodic TableA.26 moleculesB.361 moleculesC.7.75 × 1024 moleculesD.2.77 × 1023 moleculesSUBMITarrow_backPREVIOUS

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