After 1.00 ml of water is completely vaporized to gas, how many milliliters of vapor are produced at standard temperature and pressure? (density of water is 1.00 g/ml; molar volume of any gas at stp is 22.4 l/

Answer : The volume of water vapor will be, 1232 ml

Explanation :

Density is defined as the mass contained per unit volume.

Given :

Volume of water = 1.00 ml

Density of water = 1.00 g/ml

Putting in the values we get:

Mass of water = 1 gram

Now we have tot calculate the moles of water.

As, 1 mole of gas occupies 22.4 L of volume at STP

So, 0.055 moles of water vapor will occupy = of volume      (Conversion factor: 1 L = 1000 mL)

Therefore, the volume of water vapor will be, 1232 ml

the dependant variable is spilled water

the independent is the heat

hey there!

mass = 6.75 g

volume =   9 cm³

therefore:

d = mass / volume

d   = 6.75 / 9

d = 0.7 g/cm³

answer b