this is for a lab - determining the chemical formula of a hydrate. suppose the hydrate was heated too quickly and some of it was lost of spattered out of the container. explain how hthis would effect a) the calculated percent by
suppose the hydrate was heated too quickly and some of it was lost as it spattered out of the container . explain how this would effect . a. the calculated mass of water in the compound b. the molecular formula you determined.
A sample of CuSO4*5H2O was heated to 110 degrees C, where it lost water and gave another hydrate of copper (II) ion that contains 32.50% Cu. A 98.77-mg sample of this new hydrate gave 116.66 mg or barium sulfate precipitate when
A hydrate of copper (II) sulfate with formula CuSO4.xH2O has a molar mass of 250.0 g/mol. 2.545 g of hydrate is heated and 63.85% of the residue is found after heating. a) Determine the value of x in the formula of the compound b)
Predict the effect of each of the following by mass of water in the hydrate and the chemical of the hydrate? a) not heating the hydrate enough b) overheating the hydrate and producing some copper (ii) oxide C) the initial hydrate
A sealed flask contains 1 mole of hydrogen and 3 moles of helium gas at 20DC. If the total pressure is 40kPa, what is the partial pressure of the Hydrogen gas? AND :) The data below was obtained by a student in order to determine
Okay I've got a HUGE chem test tomorrow and I desperately need help! Please help!!!! 73. Hematite (Fe2O3) and magnetite (Fe3O4) are two ores used as sources of iron. Which ore provides the greatest percentage of iron per kilogram?
Do you think it is more useful to have the percent by mass of water in hydrate or the percentage composition, assuming that you know the formula for the associated dehydrated compound? Can someone please explain what's the meaning