The mass of hydrogen in 1.52 grams of acetic acid (CH3CO2H) can be calculated by determining the percentage of hydrogen in the compound and then multiplying this by the total mass, resulting in approximately 0.102 grams of hydrogen.
To calculate the number of grams of hydrogen in 1.52 grams of acetic acid (CH3CO2H), you first need to find the molar mass of acetic acid. The molar mass of acetic acid is the sum of the molar masses of its constituent atoms: 2(12.01 g/mol C) + 4(1.01 g/mol H) + 2(16.00 g/mol O) = 60.05 g/mol.
Then we calculate the percentage of hydrogen in the compound by adding the molar mass contributions of the hydrogen atoms and dividing by the total molar mass: (4(1.01 g/mol H)/60.05 g/mol) × 100 = 6.722%. To find the mass of hydrogen in 1.52 grams of acetic acid, multiply this percentage by the total mass: (6.722/100) × 1.52 g = 0.102 grams H.