1. From grams -> mole:
=grams given x 1 mol/molar mass
So 150 g Cu x 1 mol Cu/63.546 g Cu = 2.4 mol Cu
2. From mole -> atoms
=number of mol x 6.022x10^22 atoms/1 mol
So 2.4 mol Cu x 6.022x10^22 atoms Cu/1 mol Cu = 1.4 x 10^24 atoms Cu
False, Atoms are the smallest units of matter that display both the chemical and physical properties of it, based on the structure of the atom.
Answer:
Molecules in liquids are held to other molecules by intermolecular interactions, which are weaker than the intramolecular interactions that hold the atoms together within molecules and polyatomic ions.
So calculate the H for the other two reactions a room temperature and combine the reactions to calculate the H of the decomposition of calcium carbonate using the Hess's Law
Answer:
Explanation:
This is a direct application of the equation for ideal gases.
Where:
- P = pressure = 1.25 atm
- V = volume = 25.2 liter
- R = Universal constant of gases = 0.08206 atm-liter/K-mol
- T = absolute temperature = 25.0ºC = 25 + 273.15 K = 298.15 K
- n = number of moles
Solving for n:
Substituting:
