(b) Calculate the volume of 0.2M UO3- needed to react with 20.00 cm3 of 0.1M Cr2O72-. 3. 24.40 g of hydrated iron(II) sulphate, FeSO4.xH2O was dissolved and made up to 1.0 dm3 of aqueous solution, acidified with sulphuric acid. 25.00 cm3 of the solution was titrated with 20.00 cm3 of 0.022M potassium manganate(VII) solution for complete oxidation. a) Write the equation for the reaction.
What mass of MgCO3 is contained in a 2.750g solid sample consisting of only MgCO3 and MgO if heating to decompose all the MgCO3 according to the following equation leaves a solid residue weighing 2.160g? Magnesium oxide is unaffected by the heat. MgCO3(s) MgO (s) + Co2 (g) 2. a) Consider the reaction of question 2. Suppose a 3.250 g sample containing only MgCO3 and MgO is 42.6% MgO. How many grams of CO2 would be liberated by complete thermal decomposition of the MgCO3 in the sample?
What is the identity of the element Z? The two reactions are: Z(OH)2(s) + 2HCl(aq) →ZCl2(aq) + 2H2O(l) HCl(aq) + NaOH(aq) →NaCl(aq) + H2O(l) [Ans. : Mg, calculated molar mass 24.31 g] 6) A sample of “compound X,” known to contain only C and H, was burned and the resulting CO2 and
Find the volume of 2.40 mol of gas whose temperature is 50.0 °C and whose pressure is 202 kPa. 6. How many moles of gas are contained in a 50.0 L cylinder at a pressure of 10100 kPa and a temperature of 35.0 °C? 7. Determine the number of grams of carbon dioxide in a 450.6 mL tank at 1.80 atm and minus 50.5 °C.
Conclusion 10 Grams of Potassium chlorate when decomposed produces 3.915576 grams oxygen gas and 6.083363 grams potassium chloride Atomic Weight of Magnesium Introduction In this lab we will determine the atomic weight of magnesium by measuring the amount of hydrogen gas evolved when hydrochloric acid reacts with magnesium. The reaction is as follows: Mg + 2HCl -> H2 + Mg2+ (aq) + 2Cl- (aq) There is a one to one relationship between the number of moles of hydrogen gas evolved and the
Place 10 drops of zinc nitrate into A3 of the 24 well plate. 5. Place 10 drops of iron (III) chloride into A4 of the 24 well plate. 6. Place 10 drops of copper (II) sulfate into A5 of the 24 well plate.
Percent Yield Calculations 1) Balance this equation and state which of the six types of reaction is taking place: ____ Mg + ____ HNO3 ( ____ Mg(NO3)2 + ____ H2 Type of reaction: __________________________ 2) If I start this reaction with 40 grams of magnesium and an excess of nitric acid, how many grams of hydrogen gas will I produce? 3) If 1.7 grams of hydrogen is actually produced, what was my percent yield of hydrogen? 4) Balance this equation and state what type of reaction is taking place: ____ NaHCO3 ( ____ NaOH + ____ CO2 Type of reaction: __________________________ 5) If 25 grams of carbon dioxide gas is produced in this reaction, how many grams of sodium hydroxide should be produced? 6) If 50 grams of sodium hydroxide are actually produced, what was my percent yield?
|is less than the mass of the reactants | |b. |is greater than the mass of the reactants | |c. |is equal to the mass of the reactants | |d. |has no relationship to the mass of the reactants | ____ 23. Calculate the number of moles of Al[pic]O[pic] that are produced when 0.60 mol of Fe is produced in the following reaction.
How is the formula of a conjugate acid similar to its conjugate base, and how is it different? (2) They all transform to same molecules, vut Conjugate acid donates an H+ ion and conjugate base gains an H+ ion 10. Show how ammonia, NH3, is a base according to the Bronsted-Lowry definition, but not according to the Arrhenius definition. (Hint: See #8a.) (2) Although NH3 forms OH- with water, it did not donate any proton to form OH- but only gain.
10. Repeat the procedure for a second metal. Analysis: Our data | Trial #1 | Trial | Mass of zinc | 1.99g | 4.01g | Mass of water in Calorimeter | 45g | 45g | Temp. of water in Calorimeter | 20°C | 21°C | Temp. of boiling water | 100°C | 100°C | Peak temp.