As the magnesium reacts, the hydrogen gas produced is collected by water displacement at 23.0oC. The pressure of the gas in the collection tube is measured to be 749 torr. Given that the equilibrium vapor pressure of water is 21 torr at 23.0oC, calculate the pressure that the H2(g) produced in the reaction would have if it were dry.

The pressure that the produced in the reaction would have if it were dry will be 728 torr

Explanation:

According to Dalton's law, the total pressure is the sum of individual pressures.

Given :  =total pressure of gas = 749 torr

= partial pressure of hydrogen = ?

= partial pressure of water = 21 torr

putting in the values we get:

Thus the pressure that the produced in the reaction would have if it were dry will be 728 torr

answer: the primary difference between a hypothesis and a theory is that b hypothesis is falsifiable, but a theory has been proven to be correct. theory is an explanation of something that is happening but hypothesis is a guess of something that can happen

explanation:

we can conclude that the melting point of table salt is above room temperature (it's actually 801 deg c). the melting point of mercury must be below room temperature (- 39 deg c).