kg 4. 9.2 x 10 mol dL mol L bl)

Fe2O3(s)  +  2 Al(s) ------>  Al2O3(s)   +   2 Fe(l) 159.70           26.98                101.96             55.85      Molar masses in g/mol If 50. g of iron (III) oxide are combined with 45 g of aluminum how many grams of aluminum oxide are formed?

Seoyeon needs to determine the formula of an unknown hydrate (AB-XH2O). Given the following data: mass of empty crucible mass of ABXH2O + crucible mass of AB + crucible 16.5245 g 26.9416 g 21.6515 g Which of the following is the correct formula of the hydrate? (The molar mass of AB is 120.37 g mol-1) A) AB-7H2O B) AB-H20 C) AB-5H2O D) AB-3H2O

The empirical formula of a compound is HO. This molecule has a molar mass of 17.01 g/mol. The molecular formula is: HO H₂O H₂O2 H0.500.5

If 31.0 g of MgSO4⋅7H2O is thoroughly heated, what mass of anhydrous magnesium sulfate will remain? Express your answer to three significant figures and include the appropriate units.

How many grams are in 6.56*; 10 ^ 15 * r molecules of CO?

Fe2O36) + 2 Alis) Al2O316) + 2 Fe() ------> 159.70 26.98 101.96 55.85 Molar masses in g/mol If 40. g of iron (III) oxide are combined with 12.5 g of aluminum how many grams of molten iron are formed? O 18 g O 47 g 28 g O 26 g

Moles of H2C2O4·2H2O? the mass is = 1.32191 grams.

This is a lab experiment on Stoichiometry. I am struggling with questions 2b, 2c, 2d?  I attached the photo.

Using the initial mass 1.510 g and the molecular formula of the hydrate CuCl2​⋅2H2​O). Predict the expected mass of water that should be released if heated.