Answer:
0.7 moles of Ca(OH)₂ are produced.
Mass of hydrogen gas = 1.4 g
Explanation:
Given data:
Mass of water = 25.0 g
Mass of hydrogen gas produced = ?
Number of moles of Ca(OH)₂ formed = ?
Solution:
Chemical equation:
Ca + 2H₂O → Ca(OH)₂ + H₂
Number of moles of water:
Number of moles = mass/molar mass
Number of moles = 25.0 g/ 18 g/mol
Number of moles = 1.4 mol
Now we will compare the moles of water with hydrogen:
H₂O : H₂
2 : 1
1.4 : 1/2×1.4 = 0.7 mol
Mass of hydrogen gas produced:
Mass = number of moles × molar mass
Mass = 0.7 mol × 2 g/mol
Mass = 1.4 g
Now we will compare the moles of water and Ca(OH)₂
H₂O : Ca(OH)₂
2 : 1
1.4 : 1/2×1.4 = 0.7 mol
Thus, 0.7 moles of Ca(OH)₂ are produced.
