Percent Composition and Molecular Formula Worksheet 1. What’s the empirical formula of a molecule containing 65.5% carbon‚ 5.5% hydrogen‚ and 29.0% oxygen? 2. If the molar mass of the compound in problem 1 is 110 grams/mole‚ what’s the molecular formula? 3. What’s the empirical formula of a molecule containing 18.7% lithium‚ 16.3% carbon‚ and 65.0% oxygen? 4. If the molar mass of the compound in problem 3 is 73.8 grams/mole‚ what’s the molecular formula? Write the molecular formulas
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_______ Al(NO3)3 + ______ Pb 10.____ P + _____ O2 ® _______P2O5 Section II - Predict the product(s) and balance the chemical equation 1._______ C6H6 + ______ O2 ® 2._____ Pb + _______ AgNO3 ® 3.______ Ca + ______ O2 ® 4. ______ Li2SO4 + _______ BaCl2 ® 5.______Sr3N2 ® Section III - On a separate sheet of paper‚ write a balanced equation for the following reactions and classify the type of reaction. a. Aluminum metal reacts with oxygen (in the air) to form aluminum oxide. b. Sodium oxide reacts
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butter product. In this experiment‚ salt was extracted from the aqueous phase of known quantity butter. The following salt content determination was done by Mohr’s titration method with silver nitrate (AgNO3) in the presence of potassium chromate K2CrO4 indicator. The end-point was then spotted when the red silver chromate forms. The amount of salt in butter was obtained by calculation of the experimental result. Method 1. Determination of the concentration of a standard sodium chloride solution
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(OH)2(aq)+H2(g) Step 4: Mg(s) +H2O->Mg (OH)2(aq)+H2(g) Step 10: CaSO4 + H2O-> Ca(OH)2 + H2SO4 MgSO4 + H2O ->Mg (OH)2 + H2SO4 Barium Sulfate: No reaction Step 13: MgCl2 + Na2CO3 -> MgCO3 + 2NaCl CaCl2 + Na2CO3 -> CaCO3 + 2NaCl BaCl2 + Na2CO3 -> BaCO3 + 2NaCl 2. The reactivity of the metal increases with each period it goes down. Magnesium is the least reactive and is in the third period with an atomic number of 12. Calcium is slightly more reactive being in the fourth period
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compounds exchange partners. AX + BY AY + BX This reaction can occur between two inorganic salts when one product is insoluble in water‚ driving the reaction forward. A typical example is as followed and is considered a molecular equation. BaCl2(aq) + 2AgNO3(aq) Ba(NO3)2(aq)+2AgCl(s) To better identify the strong electrolytes we write a more realistic equation as follows: Ba2+(aq)+2Cl-(aq)+2Ag+(aq)+2NO3(aq) Ba2+(aq)+2NO3-(aq)+2AgCl(s) This is called an ionic equation an AgCl
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by itself. The masses were obtained along the way and then used to calculate the moles of silver chloride‚ the chloride‚ and the barium. This was then used with the masses to calculate the Empirical formula for the hydrated salt. This formula was BaCl2 (H2O). Error could have occurred at this experiment at many different places. Error
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mass of the hydrate was 1.35g and the mass of the beaker‚ watch glass‚ and anhydrous salt was 153.8g. The mass of the water was 0.15g and the percent of water in the unknown hydrate was 11.1%. % Of water in barium chloride dehydrate BaCl2 * 2H2O *Mass of beaker‚ watch glass + hydrate 154.14g (before heating) *Mass of beaker + watch glass 152.72g *Mass of hydrate
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Χηεμιστρψ Ινϖεστιγατορψ Προϕεχτ To prepare of Rayon Thread from Filter Paper Name : MOHAMMAD ARSHAD SHEIKH Class : XII ‘B’ Roll No. : School Name: KENDRIYA VIDYALAYA‚ BIBROD‚ RATLAM (M.P.) Λαβορατορψ Χερτιφιχατε This is to certify that_____________________________ has satisfactorily completed the course of chemistry
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solution containing chloride ions: Ag+(aq) + Cl-(aq) -> AgCl(s) By adding silver ions until silver chloride is no longer precipitated‚ the amount of chloride in a solution can be found. Potassium chromate (VI)‚ K2CrO4‚ can be used to indicate the end-point of the titration‚ the point at which all chloride ions have been precipitated. Silver ions combine with chromate (VI) ions to form a red precipitate of silver chromate (VI): 2Ag+(aq) + CrO2-4(aq)
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investigation were test tubes‚ a porcelain well‚ a centrifuge‚ a Bunsen burner‚ and reagents to be used for synthesis of four compounds. The compound were Na2SO4‚ AgCl‚ BaSO4‚ and ZN(OH)2. The reagents used to synthesize these compounds were NaOH‚ H2SO4‚ BaCl2‚ Zn(NO3)2‚ AgNO3‚ and HCl‚ all .1M concentrations in aqueous solution. The groups then identified the isolation method to be used on each one of the compounds. The
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