Under certain conditions, water can be separated into oxygen and hydrogen gases according to the equation 2H20 → 2H2 + O2 In a lab, 112g of hydrogen gas and 888g 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 1000g. Who is correct? (1 point)

Answer

Student B is correct. The amount of water that was separated is approximately 499.67 g.

Q: What is the given equation? A: The equation is 2H20 → 2H2 + O2.
Q: How much hydrogen gas and oxygen gas were collected in the lab? A: 112g of hydrogen gas and 888g of oxygen gas were collected.
Q: How can we find the amount of water that was separated? A: Using the molar mass of water and the given amounts of hydrogen and oxygen gases, we can find the amount of water that was separated.
Q: What is the molar mass of water? A: The molar mass of water is 18.02 g/mol.
Q: How many moles of hydrogen gas were collected? A: (112 g) / (2.02 g/mol) = 55.45 mol.
Q: How many moles of oxygen gas were collected? A: (888 g) / (32.00 g/mol) = 27.75 mol.
Q: How many moles of water were separated? A: Since the equation is balanced, we know that for every 2 moles of H2, 1 mole of O2 and 2 moles of H2O are produced. Therefore, the number of moles of H2O produced is half the number of moles of H2, which is 55.45/2 = 27.73 mol.
Q: What is the mass of water separated? A: (27.73 mol) x (18.02 g/mol) = 499.67 g.