Repeat steps 2-5 using the Sodium Carbonate. Tabulate results in table below. COMPOUNDS REACTION TIME/MINS AMOUNT OF GAS COLLECTED Calcium Carbonate Sodium Carbonate VARIABLES: 1. Control: Masses of Ca(Co3)2 and Na2Co3‚ Vol. of HCL and Conc. Of HCL. 2. Manipulated: Carbonates 3. Responding: Gas Evolution EXPECTED RESULTS: It is expected that Calcium Carbonate
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number of moles that the student has‚ based on the amount weighed out. For each calculation‚ show your work. Be sure to include the formula mass of water for CaCl2 ( 2H2O and NaH2PO4 ( H2O. Substance Formula Weight (g/mol) Number of Moles Mass (g) NaCl 58.4 74 180.2 84 147.01 246.47 120.4 0.14 58.5 74.55 1.01 KCl C6H12O6 NaHCO3 CaCl2 ( 2H2O MgSO4 NaH2PO4 ( H2O 0.005 .75 0.0262 .01173 0.0008 .0033 84.01 0.15 120.336 0.14 Answer: (5 points) Score
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carbon dioxide Purpose: The purpose of the practical that we completed was to determine the molar mass of carbon dioxide (CO2) by experimental means and to observe the reaction of hydrochloric acid and sodium carbonate. Using the balanced equation: Na2CO3 + 2HCl → 2NaCl + H2O + CO2 Materials / Apparatus: 1) 8.00g of sodium carbonate‚ 2) 30mL of hydrochloric acid (6molL-1) 3) 100mL of hydrochloric acid (6molL-1) 4) 100mL conical flask‚ 5) 150mL glass beaker 6) 50mL glass beaker 7) Glass funnel‚ 8)
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EXPERIMENT-1 CHEMICAL REACTIONS AIM: To perform and observe the following reactions and classify them into: (i) Combination reaction (action of water on quick lime) (ii) Decomposition reaction (action of heat on ferrous sulphate crystals) (iii) Displacement reaction (iron nails kept in copper sulphate solution) (vi)Double decomposition reaction (reaction between sodium sulphate and barium chloride) APPARATUS REQUIRED: 1. A rack of at least six clean test tubes and a boiling
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For the completion of this experiment the procedures were guided with the Rainbow Transformation1 lab manual. An Escherichia coli bacterial reference plate was used to obtain colonies which were resuspended into a CaCl2 solution that was previously kept on an ice bath. The rainbow transformation mixture containing the plasmid DNA was then added to half of the E. coli cells. These cells were later placed into a water bath set to 42ºC and “heat shocked” to promote the entrance of DNA into the cells
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____P2O5 12) ____ Na + ____ H2O ____ NaOH + ____H2 13) ____ Ag2O ____ Ag + ____O2 14) ____ S8 + ____O2 ____ SO3 15) ____ CO2 + ____ H2O ____ C6H12O6 + ____O2 16) ____ K + ____ MgBr ____ KBr + ____ Mg 17) ____ HCl + ____ CaCO3 ____ CaCl2 + ____H2O + ____ CO2 18) ____ HNO3 + ____ NaHCO3 ____ NaNO3 + ____ H2O + ____ CO2 19) ____ H2O + ____ O2 ____ H2O2 20) ____ NaBr + ____ CaF2 ____ NaF + ____ CaBr2 21) ____ H2SO4 + ____ NaNO2 ____ HNO2 +
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Two microcentrifuge tubes 500 uL of ice cold 0.05 CaCl2 E. coli bacteria A sterile plastic loop A sterile P-20 micropipette 10 uL of pAMP solution A timer Ice A water bath 500 uL of Luria broth A spreading rod Four plates Incubator Procedure: Day before lab 1. Streak E. coli host cells for isolation. 2. Prepare six source plates. Day of lab 1. Get two microcentrifuge tubes‚ which should each contain 200 uL of cold CaCl2 solution. Label one tube with your initials and a (+)
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→ C2 H6 + O2 Al → Remember → List the atoms‚ count‚ and solve! H2O2 → P4 + + CO2 O2 → O2 + H2O + O2 P4O6 Fe + H2O T. Trimpe 2006 Na2SO4 + http://sciencespot.net/ Na + O2 C+ H2O → CaCl2 → → H2 → Fe3O4 + CaSO4 + Na2O CH4 H2 NaCl Answer Key Balancing Balancing Equations Challenge Part A: Parts & Pieces (1) Circle each subscript in each chemical formula. (2) Draw a square around each coefficient. (3)
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a substance that conducts an electric current when dissolved in water is called an electrolyte a non-electrolyte is a substance that does not conduct an electric current in aqueous solution NH4+‚ NO3-‚ and group 1A cations are ions that always form soluble ionic compounds a precipitation reaction is a reaction in which two or more water-soluble ionic compounds react in aqueous solution to form one or more insoluble precipitates. a precipitate is a solid that separates from a solution a species
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hypochlorite (liquid bleach). Preparation It is manufactured by the calcium process: ~\mathrm{2Cl_2 + 2Ca(OH)_2\longrightarrow \ Ca(OCl)_2 + CaCl_2 + 2H_2O}. "Bleaching powder" is a mixture of calcium hypochlorite (Ca(OCl)2) and the basic chloride CaCl2‚ H2O with some slaked lime‚ Ca(OH)2. Properties Calcium hypochlorite is a yellow white solid which has a strong smell of chlorine. It is not highly soluble in water and is more preferably used in soft to medium-hard water. It has two forms: dry
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