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A sample of hydrate lost 22.7% of its original weight on being heated. Determine the number...
A student is given a sample of a calcium sulfate hydrate. He places the sample in a dry, covered crucible and weighs it. The total mass (crucible, cover, and hydrate) is 19.39219.392 g. The crucible and cover together had previously weighed 17.98717.987 g. He then heats the crucible to redness for 10 minutes with the cover slightly ajar. After the crucible cools, he weighs the crucible and its contents; the mass is now 19.09819.098 g, due to the loss of...
if a hydrate was found to contain 12% water and original weight of the sample was 30g, what will be the final weight of the anhydrous sample
A sample of hydrate was heated thoroughly. How many waters of hydration are there if the anhydrous salt had a dry mass of 12 grams and a molar mass of 185 g/mol? The mass of water evaporated from the hydrate was 5.0 g.
Experiment 3: Determination of Percent Water in a Hydrate Data Sheet Run #1 Run #2 _37.032 g Mass of crucible and cover 38.067 g Mass of crucible, cover and hydrate Mass of hydrate taken for 2-1- analysis 38.Ona _37.713 g Mass of crucible, cover and residue (after heating) _8 - Mass of H20 lost 6. _(FW=18.015 g/mol) mol Moles of H20 lost 13 3521 % % Percent of H20 lost .8 Mass of residue (anhydrous salt) mol Moles of anhydrous...
A 6.2351 g sample of an unknown hydrate of cobalt(II) bromide is heated until all the water of hydration is removed. The CoBr2 that remains has a mass of 5.0000 g. 1. How many moles of CoBr2 are in the sample? mol 2. How many grams of water were lost in the dehydration? g 3. How many moles of water were lost? (mol) 4. What is the value of "n" in the formula CoBr2 · n H2O? (1, 2, 3,...
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What was the weight percent of water in the hydrate before heating? Put answer in one decimal place. weight of water O.505 weight of hydrate 2.209 How many moles of water were lost if the amount of water lost was 0.415 grams? Do not include units and assume three significant figures m all numbers. Be sure to include the zero before the decimal if the number is less than one. How many moles of water...
A student is given a sample of a manganese(II) chloride hydrate. She weighs the sample in a dry, covered crucible and obtains a mass of 24.747 g for the crucible, cover, and sample. Earlier she had found that the crucible and cover weighed 23.599 g. She then heats the crucible to drive off the water of hydration, keeping the crucible at red heat for about 10 minutes with the cover slightly ajar. She then lets the crucible cool, and finds...
Epsom salts, a strong laxative used in veterinary medicine, is a hydrate, which means that a certain number of water molecules are included in the solid structure. The formula for Epsom salts can be written as MgSO4⋅xH2O, where x indicates the number of moles of H2O per mole of MgSO4. When 4.555 g of this hydrate is heated to 250 ∘C, all the water of hydration is lost, leaving 2.225 g of MgSO4. What is the value of x?
A hydrate of Cobalt(ii)Chloride had mass of 166.04g before heating. After heating, the anhydrous CoCl2 weighed 130.9g. - what is the mass of the water that was driven off? - how many moles of water were driven off? - how many moles of anhydrous CoCl2 remain? - what is the hydration number (moles of water per mole compound)?
Data Table 1. CuSO4 Data Mass of empty cup (grams) Mass of CuSO, hydrate (erams)S Cuso, hydrate after 1st heating (grams) CuSO, hydrate after 2nd heating (grams) Mass of released H20 (grams) Number of moles of released H201 Mass of anhydrous Cuso (grams) Number of moles of anhydrous CuSO 02a mo Questions: A) Calculate the ratio of moles of H2O to moles of anhydrous Cuso4. Note: Report the ratio to the closest whole number. B) Write the empirical formula for...