

Calculate the formula mass and molar mass of NH3. Formula mass a mu Molar mass= g/mol
Calculate the molar mass of calcium nitrate. Calculate the molar mass of calcium nitrate. 164.10 g/mol 132.10 g/mol 102.09 g/mol 136.03 g/mol none of the above I typically understand how to calculate the molar mass but not when it is a compound. I originally got 102.09 but it was marked wrong on my homework and I do not know how to get to the correct answer.
16. You synthesized 3.204 g of Ni(NH3)nCl2. The mass percent of NH3 and Ni2+ in the synthesized Ni(NH3)nCl2 were 44.1% and 25.3%, respectively. Molar mass of Ni2+ , NH3 and Cl2 are 58.69 g/mol, 17.04 g/mol, and 70.90 g/mol, respectively. a) (1 pts) Calculate the mass percent of Cl2. b) (1 pts) Calculate the masses of Ni2+ , NH3 and Cl2. c) (1 pts) Calculate the number of moles of Ni2+ . d) (1 pts) Calculate the number of moles...
A compound with the empirical formula of NaSO₄ and a molar mass of 238 g/mol has a molecular formula of:
Calculate the molecular formula of the hormone estradiol. Empirical formula is C9H12O and the molar mass of the molecular formula is 274.30 g/mol.
Calculate the molar mass of each compound. CH g/mol C3H2,02 g/mol
Empirical formula C2H4O, molar mass = 132.0 g/mol Express your answer as a chemical formula.
1) if 6.85 of glucose( C6H12O6, molar mass=180.2 g/mol) is dissolved in 155g of chloroform( CHCL3,molar mass= 119.4 g/mol) , what is the boiling point of the solution. ( the boiling point of pure CHCl3 is 61.2 celsius, and Kb = 3.63 celsius/m for CHCl3) 2) a,) Liquid ammonia (boiling point = -33.4C) can be used as a refrigerant and heat transfer fluid. How much energy is needed to heat 25.0 g of NH3(l) from -65.0C to -12.0C? Heat of...
A compound with the empirical formula CH, has a molar mass of 70 g/mol. What is the molecular formula for this compound? molecular formula:
Cyclohexylbenzene has the empirical formula C3H4. Its molar mass is 160.3 g/mol. Its molecular formula is:
A powder contains FeSO4⋅7H2O (molar mass=278.01 g/mol),(molar mass=278.01 g/mol), among other components. A 3.455 g sample of the powder was dissolved in HNO3 and heated to convert all iron to Fe3+. The addition of NH3 precipitated Fe2O3⋅?H2O, which was subsequently ignited to produce 0.502 g Fe2O3. What was the mass of FeSO4⋅7H2O in the 3.455 g sample? Please include every step.