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

atomic number of carbon is 6

electronic configuration of carbon is 1s²2s²2p²

orbital diagram of c is as shown here in the image.

every chemical equation adheres to the law of conservation of mass, which states that matter cannot be created or destroyed. therefore, there must be the same number of atoms of each element on each side of a chemical equation.