If you have a 37.34g sample of ammonium chromate , how many protons do you have?\
To determine the number of protons in a sample of ammonium chromate, we need to find the molar mass of ammonium chromate and then calculate the number of moles of the compound. From there, we can use Avogadro's number to find the number of protons in the sample.
1. Find the molar mass of ammonium chromate (NH4)2CrO4:
- Ammonium (NH4) has a molar mass of:
- Nitrogen (N) (14.01 g/mol) x 1 = 14.01 g/mol
- Hydrogen (H) (1.01 g/mol) x 4 = 4.04 g/mol
- Chromate (CrO4) has a molar mass of:
- Chromium (Cr) (52.00 g/mol) x 1 = 52.00 g/mol
- Oxygen (O) (16.00 g/mol) x 4 = 64.00 g/mol
- Total molar mass of (NH4)2CrO4:
- (14.01 g/mol + 1.01 g/mol x 4) x 2 + 52.00 g/mol + 16.00 g/mol x 4 = 152.07 g/mol
2. Calculate the number of moles of ammonium chromate:
- Moles = Mass / Molar mass
- Mass = 37.34 g (given)
- Moles of ammonium chromate = 37.34 g / 152.07 g/mol = 0.2457 mol
3. Use Avogadro's number to find the number of protons:
- Avogadro's number (NA) = 6.022 x 10^23 mol^-1
- Number of protons = Number of moles x Avogadro's number
- Number of protons = 0.2457 mol x 6.022 x 10^23 mol^-1 = 1.478 x10^23 protons
Therefore, if you have a 37.34g sample of ammonium chromate, you would have approximately 1.478 x 10^23 protons.