The molecular weight of H2O is 18g/mol.
Therefore, 27.9 g H2O / (1mol/18g) = 0.155 mol H2O
Calculating only for the latent heat, the heat required to be released for this amount of H2O to condense is:
40.7 kJ/mol (0.155 mol) = 6.3 kJ or -6.3 kJ since it is to be released
TRUE. (Lorenzo Romano Amadeo Carlo Avogadro) Ideal Gas Law that defined as one in which all collisions between atoms or molecules are perfectly elastic in which there are no intermolecular attractive forces. In such a gas, all the internal energy is the form of kinetic energy and any change in internal energy is accompanied by a change in temperature. That characterized by three state variables: absolute pressure (P) = 1 atm, volume (V) = 22.4 L and absolute temperature (T) = 273 K.
Answer:
I'll do #1
Explanation:
Solids:They are molecules packed together and contain the least amount of kinetic energy
Liquids:Flows frequently in space, of constant volume
Gasses:Gas is made up of atoms,mostly made up of a mixture of air
Plasma:Largest part of your blood
Hope This Helppps!!Good Luck!!!
Answer:
Number of moles = 0.04 mol
Explanation:
Given data:
Mass of water lost = 0.7 g
Number of moles = ?
Solution:
Number of moles = mass/molar mass
Molar mass of water = 18 g/mol
Now we will put the values in formula:
Number of moles = mass/molar mass
Number of moles = 0.7 g/ 18 g/mol
Number of moles = 0.04 mol
