Answer:
v = 37.9 ml
Explanation:
Given data:
Mass of compound = 1.56 kg
Density = 41.2 g/ml
Volume of compound = ?
Solution:
First of all we will convert the mass into g.
1.56 ×1000 = 1560 g
Formula:
D=m/v
D= density
m=mass
V=volume
v = m/d
v = 1560 g / 41.2 g/ml
v = 37.9 ml
D.10.0 mol is the correct
<u>Answer:</u> The moles of water produced are 1.54 moles.
<u>Explanation:</u>
To calculate the number of moles, we use the equation:
Given mass of ethane = 15.42 g
Molar mass of ethane = 30.07 g/mol
Putting values in above equation, we get:
The chemical equation for the combustion of ethane follows:
By Stoichiometry of the reaction:
2 moles of ethane produces 6 moles of water
So, 0.513 moles of ethane will produce = 
of water
Hence, the moles of water produced are 1.54 moles.
Answer:
i think it's 3 because there aren't any indexes so that leaves us with one atom of Ca, one atom of O, and one atom of H
The bonds found between water molecules are called:
Hydrogen bonds
which contribute to water having a high number of Van Der Waals forces.
Explanation:
A hydrogen bond is an electromagnetic attraction within polar molecules in which hydrogen is joined to a larger atom, such as oxygen or nitrogen. This is not a dividing of electrons, as in a covalent bond. Preferably, this is an attraction among the positive and negative poles of charged atoms.
