Limiting Reactants Lab Report

Superior Essays
The purpose of the experiment was to observe limiting reactants by using a fixed amount of one reagent along with a varying the amount of the second reagent used in a chemical reaction. Through these results, the concept of limiting reactants can be determined. Using a graph to demonstrate the relation between the volumes of hydrogen gas produced versus the moles of the reagents will help figure out the stoichiometric balance required. The success of the experiment will be determined by the comparing the experimental values with the fixed values.

Introduction
Stoichiometry involves converting chemical formulas and equations that represent individual atoms, molecules, and formula units to the laboratory scale that uses milligrams, grams, and kilograms, of these substances (1). A limiting reactant is the reactant that has been completely consumed in a chemical reaction. It is
…show more content…
A graph of the volume of hydrogen gas produced versus moles of a reagent that is varied will be able to tell you the point in which the stoichiometric balance is achieved and what the limiting reactant is. In this experiment group A used a constant mass of magnesium metal (0.100 g) and varying volumes of 2.00 M hydrochloric acid added from 2.00 mL to 7.00 mL in progressions of 1.00 mL which in total came out to be six distinctive chemical reactions. Group B used the consistent volume of 2.00 M hydrochloric acid (5.00 mL) and changed the mass of the magnesium metal used from 0.070 g to 0.170 g in growths of 0.020 g which resulted in a total of six different chemical reactions as well. The percent yield for magnesium, according to the data, was 107.3% and the percent yield for hydrochloric acid, according to the data, was 96.0%. Overall, the experiment was fairly successful as observed by the percent yields of both

Related Documents

  • Improved Essays

    It can be calculated y subtracting the sum of enthalpies of formation of reactants from the sum of enthalpies of formation of the products. The enthalpy of formation is the ΔHrxn when 1 mole of a compound is formed from its elements in their standard states at 25℃ at 1 atm.2 The change in enthalpy per mole of a reaction was illustrated by part B of the experiment, because the change in enthalpy per mole of HCl or NH4OH was calculated. The standard molar enthalpy of formation was illustrated by part C of this experiment, because the various reactions added up to a reaction that led to the creation of 1 mole MgO from its elements at their standard states. Hence, the ΔHrxn in this reaction represented the enthalpy of…

    • 833 Words
    • 4 Pages
    Improved Essays
  • Improved Essays

    3. Results 3.1 Cyclic voltammetry measurement CV of the redox reaction of the hydrolysate was measured at various concentrations. In the 80 °C bath, the initial hydrolysate concentration was 2% and was further diluted to 1% and 0.5%. Fig. 2(A) shows the CV curves, indicating the tendency and relation of current with varying potential (volt).…

    • 1213 Words
    • 5 Pages
    Improved Essays
  • Improved Essays

    Batch adsorption experiments Adsorption of the Pb2+ ions by the Fe3O4@GMA-AAm nanocomposite was measured from batch adsorption experiments by mixing 10 mg of adsorbent with an aqueous solution containing a predetermined concentration of Pb2+ ions (50 mL). The mixture was shaken at 200 rpm to reach equilibrium. After a specified time, the solid and liquid were separated by external magnet and the concentrations of Pb2+ ions were measured by AAS. To find the optimized pH in adsorption of Pb2+ ions the effect of the pH was studied. The initial pH of the solutions was adjusted in the range of 2.0 –7.0 by adding 0.1N HCl or 0.1N NaOH solution at 25 ◦C.…

    • 1394 Words
    • 6 Pages
    Improved Essays
  • Superior Essays

    Formal Lab Report: Molar Volume of a Gas at STP Abstract: The purpose of this experiment is to find out how to experimentally determine what the volume of a mole of H₂(g) is at STP by using gas laws. The hypothesis for the experiment is that if H₂(g) is produced at RT and STP, Avogadro’s law can be used to experimentally determine the amount of H₂(g) because equal gases at the same pressure and temperature have the same amount of particles. In order to find the molar volume, hydrogen gas was produced in a eudiometer tube by reacting magnesium and hydrogen chloride. The results showed that the molar volume of H₂(g) was 27.5L per mole of H₂(g). It was concluded that the molar volume of a gas can be experimentally determined by using gas…

    • 1765 Words
    • 8 Pages
    Superior Essays
  • Improved Essays

    Phenolphthalein Lab Report

    • 1370 Words
    • 5 Pages

    For both trials, we used 25ml of Sprite. In Trial 1, 5.3ml of sodium hydroxide was added to the solution via titration. In Trial 2, 5.2ml of sodium hydroxide was used. To calculate molarity for Trial 1, we used the molarity of sodium hydroxide (NaOH), .101 and multiplied this number by the milliliters of NaOH used, 5.3. Then we used the molar relationship from the equation and divided by 3 moles of NaOH which is related to 1 mole of Acid, because they have a 3:1 relationship respectively.…

    • 1370 Words
    • 5 Pages
    Improved Essays
  • Great Essays

    This law makes it possible for the partial pressure of the water vapor to be removed from the total pressure of the gases in the eudiometer tube to yield the partial pressure of hydrogen gas. Molar volume is the volume occupied by one mole of a gas, in this case, hydrogen gas. Molar volume relates to the lab as the entire purpose of this lab is to find the molar volume of hydrogen gas at STP. The ideal gas law describes a relationship between pressure (P), volume (V), the number of moles (n), temperature (T), and the universal gas constant (R) where PV = nRT. This ideal gas law is essential to the lab as it explains the relationships between the different measurements of a gas and reduces into the combined gas law.…

    • 1741 Words
    • 7 Pages
    Great Essays
  • Decent Essays

    Content Stoichiometry is the relationship of the masses of the reactants and products in a chemical reaction. For a given mass of a substance in a reaction, the mass of any other substance in the reaction can be obtained using the coefficients of the balanced chemical equations and the molar masses of the substances involved. The amounts obtainable from a balanced chemical equation are called stoichiometric amounts (Villamar Jr., 2004). As what was said in the introduction, the first topic that is going to be discussed is a brief background of stoichiometry and terms to remember. Based from the definition, we can derive the two parts of stoichiometry, the composition and the reaction.…

    • 940 Words
    • 4 Pages
    Decent Essays
  • Great Essays

    Research Question: To compare the enthalpy change of reaction of 3 neutralization reactions by using 3 different acids of distinct pH. The same base of NaOH will be used in all three experiments. Introduction: Chemical reactions always have energy change. Energy in the form of heat, if liberated is known as exothermic and if absorbed in the reaction is known as endothermic. When a reaction carried out under standard condition at a of temperature 298K and 1 atm of pressure and 1 mole of water is formed it is called the starndard enthalpy of neutralisation (ΔHno).…

    • 889 Words
    • 4 Pages
    Great Essays
  • Great Essays

    KMnO4 is an oxidising agent which means it brings about oxidation and therefore it is being reduced. This means that the Fe (II) is the reducing agent and therefore is being oxidised. Carrying out a redox titration means for this experiment, using the average titre, which is determined by the colour change of the end point, it can determine: The moles of KMNO4 in the average titre, the amount of moles needed of Fe(II) to complete the reaction in 25cm3, using the Balanced equation for the reaction, from this the amount of Fe (II) in volumetric flask. Using these values the weight of Fe (II) can be calculated and then the % weight, respectively. Experimental Procedure Part…

    • 2461 Words
    • 10 Pages
    Great Essays
  • Improved Essays

    Lastly, we multiplied by 1000 ml over 1 L because molarity is moles over liter of solution. These calculations resulted in the M NaH as 0.099927 or approximately 0.1M. For trial two, we used .50 g KHP and 24.4 ml NaOH, resulting in a molarity of 0.1003 or approximately 0.1M. We applied the same steps mentioned above, with different substitutions for g KHP and mL NaOH. In addition, using the above results, we were able to find the average value of molarity of NaOH by adding to two molarity values and dividing it by two.…

    • 1233 Words
    • 5 Pages
    Improved Essays