Under certain conditions water can be separated into oxygen and hydrogen gases according to the equation to h2o2h2 + 02 in a lab of 112 G of hydrogen gas and 888 G of oxygen gas were collected student a says that the amount of water to start cannot be determined but student B says that the water must have been a thousand G's who is correct
To determine who is correct, let's calculate the amount of water that would be required to produce 112 g of hydrogen gas and 888 g of oxygen gas.
From the balanced equation: 2H2O → 2H2 + O2
The molar mass of H2O is 18 g/mol, H2 is 2 g/mol, and O2 is 32 g/mol.
To find the number of moles of hydrogen gas:
112 g H2 / 2 g/mol = 56 mol H2
To find the number of moles of oxygen gas:
888 g O2 / 32 g/mol = 27.75 mol O2
According to the balanced equation, hydrogen gas and oxygen gas are produced in a 2:1 ratio. This means that for every 2 mol H2O, we get 2 mol H2 and 1 mol O2. Therefore, the moles of water should be the same as the moles of oxygen gas.
Moles of water = 27.75 mol
To find the mass of water:
Mass of water = moles of water × molar mass of water
Mass of water = 27.75 mol × 18 g/mol = 499.5 g
Hence, the amount of water required to produce 112 g of hydrogen gas and 888 g of oxygen gas is around 499.5 g.
Student B is correct.