2. A mixture of Na2SO4 and its hydrate Na,SO4-10H2O has a mass of 1.5099 g. After heating to drive off all the water, the mass is only 1.1410 g. What is the weight percentage of NażSO4-10H2O in the original mixture? Report your answer to 4 significant figures. Molar masses: Na,SO4 142.04 g/mol; Na,SO4-10H,O 322.19 g/mol.

0.279 g of the hydrate CoCl2•nH2O is heated to produce 0.197 g of anhydrous CoCl2 (MM = 129.83 g/mol).  We want to use this to determine n, how many waters of hydration were in the original sample, be the end of the questions that follow. How many grams of water were in the original 0.279 g of hydrate? How many grams of CoCl2 were present on the original 0.279 g of hydrate?

Please help me, and double and triple check your answers previous tutors got questions wrong

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

S + 6 HNO3 --> H₂SO4 + 6 NO2 + 2 H₂O In the above equation how many moles of water can be made when 162.9 grams of HNO3 are consumed? Round your answer to the nearest tenth. If you answer is a whole number like 4, report the answer as 4.0 Use the following molar masses. If you do not use these masses, the computer will mark your answer incorrect.: Molar Element Mass Hydrogen 1 Nitrogen 14 Sulfur 32 Oxygen 16

A chemist invents a new combustion analysis instrument that uses less O2(g) which saves money on each analysis. The improvement is that instead of CO2(g) being formed and trapped, CO(g) is formed and trapped. H2O (g) is also formed and trapped when substances that contain hydrogen are analyzed.(a) The chemist places 2.184 g of an unknown compound of carbon and hydrogen in the new analyzer. 4.627 g of CO (g) and 1.795 g of H2O (g) are produced. Find the empirical formula for the compound.(Molar masses (g/mol): CO = 28.0104, H2O = 18.015) (b) Despite the best efforts of the chemist, the molar mass of the compound cannot be determined (using this method). Clearly explain why this prevents the determination of the molecular formula

The chemical formula for chlorophyll is C₅₅H₇₂MgN₄O₅. a) What is the molar mass of the compound? Provide an answer to two decimal places. b) What is the percent by mass of carbon in the compound? c) What is the mass in grams of chlorophyll that are in 2.185 moles of the compound? d)What quantity in moles of chlorophyll are there in 2.185 grams of the compound?

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.

Aspirin can be prepared from salicylic acid (C7H6O3 ), which has a molar mass of 138.12 g/mol, and acetic anhydride (C4 H6 O3), which has a molar mass of 102.04 g/mol. The density of acetic anhydride is 1.082 g/mL. C;H,O3 + C4H6O3 → C9HgO4 + C2H3O2 What is the theoretical yield, in grams, of aspirin (C9H3O4), which has a molar mass of 180.15 g/mol, possible when reacting 3.06 g of salicylic acid with 3.71 mL of acetic anhydride? Type answer:

Hand written solutions are strictly prohibited.