In trial one the mass of silver oxide is .5g. The mass of silver metal product is .431 grams.
In trial two the silver oxide=.498 and silver metal=.388.
How do you use this information and the conservation of mass to calculate the mass of oxygen that combined with the silver?
same problem
To calculate the mass of oxygen that combined with the silver in each trial, we will use the conservation of mass principle. According to this principle, mass cannot be created or destroyed during a chemical reaction. Therefore, the total mass of the reactants should be equal to the total mass of the products.
In both trials, the reactant is silver oxide (Ag2O), and the product is silver (Ag) and oxygen (O2).
Trial 1:
Mass of silver oxide = 0.5g
Mass of silver metal product = 0.431g
To calculate the mass of oxygen, we can subtract the mass of silver produced from the initial mass of silver oxide:
Mass of oxygen = Mass of silver oxide - Mass of silver metal
= 0.5g - 0.431g
= 0.069g
Therefore, in trial 1, the mass of oxygen that combined with the silver is 0.069 grams.
Trial 2:
Mass of silver oxide = 0.498g
Mass of silver metal product = 0.388g
Using the same approach, we can calculate the mass of oxygen in trial 2:
Mass of oxygen = Mass of silver oxide - Mass of silver metal
= 0.498g - 0.388g
= 0.11g
Therefore, in trial 2, the mass of oxygen that combined with the silver is 0.11 grams.
By applying the conservation of mass principle, we can determine the mass of oxygen that combined with the silver in each trial.