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

adding or remove a gaseous reactant or product changes the concentrations. if the concentration of reactant or product is increased, the system will shift away from the side in which concentration was increased (i.e. if the concentration of reactants is increased, the system will shift toward the products. if more products are added, the system will shift to form more reactants). conversely, if the concentration of reactant or product is decreased, the system will shift toward the side in which concentration was decreased (i.e. if reactants are removed, the system will shift to form more reactants. if the concentration of products is decreased, the equilibrium will shift toward the products).

explanation: