i have no idea how to start this problem off. can someoneplease explain step by

Question

i have no idea how to start this problem off. can someoneplease explain step by step so I can learn how to do it for futureproblems ? thank you in advance! i will rate you lifesaver forsure!! 1. A student carried out a dehydration experiment usingMgSO4. nH2O. The student placed anevaporating dish which contained 3.8457 g of MgSO4.nH2O in an oven at 110 C. At this temperature, some butnot all of the water in this hydrate was lost. When a constant masswas achieved, the salt weighed 2.4402 g. The student then placed the evaporating dish and contents backin the oven at 160 C. The residue came to a constant mass of 1.8779g. Stronger heating produced no further loss in mass so we canassume all the water has evaporated. Assume that this final residueis the completely anhydrous compound. The water is lost in molecular steps and the formulas must bewritten with integers and not fractions. a. What is the formula of the 1.8779 g sample? b. What is the formula of the 2.4402 g sample? c. What is the formula fo the 3.8457 g sample? 2. A hydrate of sodium carbonate loses 63% of its mass whenheated to 110 C. How many molecules of water are attached to eachmolecule of sodium carbonate? i have no idea how to start this problem off. can someoneplease explain step by step so I can learn how to do it for futureproblems ? thank you in advance! i will rate you lifesaver forsure!! 1. A student carried out a dehydration experiment usingMgSO4. nH2O. The student placed anevaporating dish which contained 3.8457 g of MgSO4.nH2O in an oven at 110 C. At this temperature, some butnot all of the water in this hydrate was lost. When a constant masswas achieved, the salt weighed 2.4402 g. The student then placed the evaporating dish and contents backin the oven at 160 C. The residue came to a constant mass of 1.8779g. Stronger heating produced no further loss in mass so we canassume all the water has evaporated. Assume that this final residueis the completely anhydrous compound. The water is lost in molecular steps and the formulas must bewritten with integers and not fractions. a. What is the formula of the 1.8779 g sample? b. What is the formula of the 2.4402 g sample? c. What is the formula fo the 3.8457 g sample? 2. A hydrate of sodium carbonate loses 63% of its mass whenheated to 110 C. How many molecules of water are attached to eachmolecule of sodium carbonate?

Explanation / Answer

moles MgSO4 = 1.8779 g/ 120.367 g/mol = 0.01560 mass water = 3.8457 - 1.8779=1.9678 g moles water = 1.9678 g/ 18.02 g/mol=0.1092 0.1092 / 0.01560 = 7 2.4402 - 1.8799 = 0.5603 = mass water 0.5603/ 18.02 =0.03109 0.03109/ 0.01560=2 a formula of the 1.8779 g sample = MgSO4 b formula of the 2.4402 sample = MgSO4 *2 H2O c formula of the 3.8457 g sample = MgSO4 * 7 H2O moles H2O = 63 g / 18.02 =3.50 moles Na2CO3 = 100 - 63 / 105.99 g/mol= 0.349 3.50/ 0.349=10 molecules of water

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