Help pls!! Question number 7

6.69×10²⁵ molecules

Explanation:

From the question given above, the following data were obtained:

Mass per bottle of water = 500 g

Number of molecules of water =?

Next, we shall determine the mass of 4 bottles of water. This can be obtained as follow:

1 bottle = 500 g of water

Therefore,

4 bottles = 4 × 500

4 bottles = 2000 g of water.

Finally, we shall determine the number of molecules of in 2000 g of water. This can be obtained as follow:

From Avogadro's hypothesis:

1 mole = 6.02×10²³ molecules.

1 mole of water (H₂O) = (2×1) + 16

= 2 + 16

= 18 g

Thus, we can say that:

18 g of water = 6.02×10²³ molecules.

Therefore,

2000 g = 2000 × 6.02×10²³ / 18

2000 g = 6.69×10²⁵ molecules

From the calculations made above, we can conclude that the chemist consumes 6.69×10²⁵ molecules of water daily.

if the concentration of products is decreased, the equilibrium will shift toward the products). add an inert gas (one that is not involved in the reaction) to the constant-volume reaction mixture: this will increase the total pressure of the system, but will have no effect on the equilibrium condition.

explanation:

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