in the reaction between sodium and water, hydrogen gas is given off and sodium hydroxide is formed. The gas is collected and there is found to be 1.8 moles of hydrogen.
a) what mass of sodium would have been used in the reaction?
To find the mass of sodium used in the reaction, we need to use the balanced chemical equation, the molar ratio, and the molar mass of sodium.
The balanced chemical equation for the reaction between sodium and water is:
2 Na + 2 H2O → 2 NaOH + H2
From the equation, we can see that 2 moles of sodium react to produce 1 mole of hydrogen gas (H2). This means that the molar ratio of sodium to hydrogen gas is 2:1.
Given that there are 1.8 moles of hydrogen gas produced, we can use the molar ratio to calculate the moles of sodium used:
Moles of sodium = 1.8 moles of hydrogen gas × (2 moles of sodium / 1 mole of hydrogen gas) = 3.6 moles of sodium
Now, to find the mass of sodium, we need to multiply the moles of sodium by its molar mass. The molar mass of sodium is 22.99 g/mol.
Mass of sodium = 3.6 moles of sodium × 22.99 g/mol = 82.764 g
Therefore, the mass of sodium used in the reaction would be approximately 82.76 grams.
Balance the equation:
Na + 2HOH= NaOH + H2
so the mole ratio of Na:H2 is 1:1
how many grams of Na is in 1.8 moles>