consider the chemical reaction between hydrogen gas and oxygen gas to form water
2H2(g)+O2(g) ➡️ 2H2O(g)
Hydrogen(H): 1 g/mol
Oxygen(O): 16 g/mol
Water(H2O): 18 g/mol
Calculate the mass of the reactants and products. Use your calculations to determine if the reaction is shows conservation of mass. Show your work and explain your reasoning
To calculate the mass of the reactants and products in the given chemical reaction, we need to consider the molar masses of hydrogen, oxygen, and water.
Given:
Hydrogen (H) = 1 g/mol
Oxygen (O) = 16 g/mol
Water (H2O) = 18 g/mol
1. Mass of hydrogen gas (H2):
In the reaction, we have 2 moles of hydrogen gas (H2). Therefore, the mass of hydrogen gas can be calculated as:
Mass of H2 = 2 moles of H2 x (1 g/mol) = 2 g.
2. Mass of oxygen gas (O2):
In the reaction, we have 1 mole of oxygen gas (O2). Therefore, the mass of oxygen gas can be calculated as:
Mass of O2 = 1 mole of O2 x (16 g/mol) = 16 g.
3. Mass of water (H2O):
In the reaction, we have 2 moles of water (H2O). Therefore, the mass of water can be calculated as:
Mass of H2O = 2 moles of H2O x (18 g/mol) = 36 g.
Now, let's check if the reaction shows conservation of mass by adding up the masses of the reactants and comparing them with the mass of the products.
Mass of reactants = Mass of H2 + Mass of O2 = 2 g + 16 g = 18 g
Mass of products = Mass of H2O = 36 g
Since the mass of the products (36 g) is equal to the mass of the reactants (18 g), it indicates that the reaction shows conservation of mass. This means that the mass of the products formed is equal to the mass of the reactants consumed.