Answer:
Mass = 473.2 g
Explanation:
Given data:
Mass of cobalt(III) nitrate = 206 g
Mass of silver bromide produced = ?
Solution:
Chemical equation:
CoBr₃ + 3AgNO₃ → 3AgBr + Co(NO₃)₃
Number of moles of cobalt(III) nitrate:
Number of moles = mass/ molar mass
Number of moles = 206 g/ 245 g/mol
Number of moles = 0.84 mol
Now we will compare the moles of cobalt(III) nitrate with silver bromide.
Co(NO₃)₃ : AgBr
1 : 3
0.84 : 3/1 × 0.84 = 2.52 mol
Mass of silver bromide:
Mass = number of moles × molar mass
Mass = 2.52 mol × 187.77 g/mol
Mass = 473.2 g
Answer:
Jose is right
Explanation:
As the book is sitting still on the table, it is being acted upon by two forces of equal magnitude and opposite direction. Theses are;
i) The weight of the book
ii) The normal reaction on the book
The weight of the book acts downwards while the normal reaction acts upwards. These two forces exactly counterbalance each other hence the book sits still on the table.
TLDR: 6.53x10^5 g NH4ClO4
The stoichiometric coefficients (the numbers in front of the reactants and products) show that Aluminum and Ammonium Perchlorate are consumed at the exact same rate throughout the reaction: 3 parts of one to 3 parts of another.
1.5x10^5 grams of Aluminum, considering that the formula weight of Aluminum is 26.98 g/mol, is equal to 5,559.7 moles of Aluminum. This means that 5,559.7 moles of Ammonium Perchlorate are required to run the reaction to completion.
The formula weight of Ammonium Perchlorate is 117.49 grams a mole, and multiplying it by 5,559.7 moles to react to completion means that 6.53x10^5 grams of Ammonium Perchlorate is required for the reaction.
I’m pretty one of the answers is water, but I don’t know if there is more