Calculate the volume, mass and number of molecules of hydrogen liberated when 230 g of sodium reacts with excess of water at STP.
(atomic masses of Na = 23U, O = 16U, and H = 1U)
(atomic masses of Na = 23U, O = 16U, and H = 1U)
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Answer:
230g x 2g / 46 g = 10g of Hydrogen. 1 gram molar mass of any gas at STP i.e., standard temperature 273 K and standard pressure 1 bar, occupies 22.4 litres known as gram molar volume. 2.0 g of hydrogen occupies 22.4 litres at STP.
Explanation:
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Answer:
230g x 2g / 46 g = 10g of Hydrogen.
1 gram molar mass of any gas at STP i.e., standard temperature 273 K and standard pressure 1 bar, occupies 22.4 litres known as gram molar volume. 2.0 g of hydrogen occupies 22.4 litres at STP.