B) Cu(OH) 2 Is the resulting answer when H20 is decomposed.
Answer:
Molecule
Explanation:
Molecule is defined as the discrete group of atoms that are held together by sharing valence electrons.
This is because two or more atoms is known as a molecule and for electron sharing to occur then there must be a minimum of two atoms which is also known as a molecule present in the sharing process.
Answer:
The ppm carbon in the seawater is 104.01.
Explanation:
Mass of seawater = 6.234 g
Mass of carbon dioxide gas produced = 2.378 mg = 0.002378 g
1 mg = 0.001 g
Moles of carbon dioxide gas = 
1 mol of carbon dioxde gas has 1 mole pf carbon atoms,then
will have ;
of carbon
Mass of
of carbon ;

To calculate the ppm of oxygen in sea water, we use the equation:
(Both the masses are in grams)

The ppm carbon in the seawater is 104.01.
there should be less liquid at the end of the experiment since heating liquid is an endothermic process, and endothermic processes typically break the bonds between liquids. The applied heat would soon break the bonds that hold the molecules of the liquid together, and evaporation would occur once the temperature is hot enough. Thus, the evaporated water would decrease the volume of the liquid.
Answer:
The mass of oxygen gas dissolved in a 5.00 L bucket of water exposed to a pressure of 1.13 atm of air is 0.04936 grams.
Explanation:
Henry's law states that the amount of gas dissolved or molar solubility of gas is directly proportional to the partial pressure of the liquid.
To calculate the molar solubility, we use the equation given by Henry's law, which is:
where,
= Henry's constant =
= partial pressure of oxygen
We have :
Pressure of the air = P
Mole fraction of oxygen in air = 

= Henry's constant =
Putting values in above equation, we get:
Moles of oxygen gas = n
Volume of water = V = 5 L



Mass of 0.001542 moles of oxygen gas:
0.001542 mol × 32 g/mol = 0.04936 g
The mass of oxygen gas dissolved in a 5.00 L bucket of water exposed to a pressure of 1.13 atm of air is 0.04936 grams.