a) Write the equation for the reaction. b) Calculate the number of moles of Fe2+ present in 1.0 dm3 of the solution. c) Calculate the molar mass of hydrate iron(II) sulphate. Hence calculate the value of x. 4.
Introduction: The purpose of this experiment is to determine the empirical formula of magnesium oxide formed by the reaction of magnesium with oxygen. To work out formula by the experiment it is necessary to measure the exact masses of each element present in a sample of a compound. Knowing the masses of magnesium and oxygen and its molar masses it is possible to find how many moles of each element is present in the magnesium oxide. The number of moles then can be used to obtain a molar ratio, which gives us the empirical formula of the compound. During the combustion reaction the ribbon of magnesium metal is heated, it reacts with oxygen from the air in a crucible, producing magnesium oxide: magnesium + oxygen → magnesium oxide We measure the mass of magnesium we use for the reaction, and the mass of magnesium oxide produced at the end of it, then we can work out the mass of oxygen that has been combined with the magnesium.
To work out the formula of the magnesium oxide, we need relative atomic masses and number of moles of magnesium and oxygen. By finding the moles involved in the reaction, we can work out the ratio of the magnesium to oxygen in the compound (magnesium oxide) should be 1:1. A balance formula of the experiment: 2Mg(s) + O2(g) → 2MgO(s) Method The same balance was used for the weighing in the experiment 1. All apparatus were set up. 2.
The Empirical Formula of an Oxide, Purpose: The purpose of this lab was to determine the empirical formula of magnesium oxide. To do this, we measured the weight of the magnesium before the reaction with oxygen, and then measure it after it had bonded with the oxygen. After the mass of the items were collected, the data was calculated in empirical formula. Background: The empirical formula of a compound is the whole number ratio of the elements in a compound. For example, the empirical formula of water is H2O meaning for every 1 O atom there are 2 H atoms.
Fraction Distillation Aim/Purpose: The main goal of the experiment Fraction Distillation was to use a technique called distillation to separate a mixture of liquids into three separate fractions. Also, the composition of each fraction is determined by recording Gas Chromatography. Theory: The original mixture that is distilled is comprised of equal amounts of hexane and toluene. Separation of this mixture is based on the differences in the component’s boiling point. Since boiling point and vapor pressure are inversely proportional, the separation is thus based on the vapor pressure as well.
The mole can be also defined as the number of atoms in exactly 12g of Carbon. In this experiment, the magnesium will be heated and this magnesium will react with the oxygen in the air to form magnesium Oxide. DIAGRAM: METHOD: 1. An empty crucible and its lid were weighed on an electrical balance. The mass of the crucible and its lid were recorded.
From there, in order to balance oxygen, water molecules are enumerated to the opposite of the equation/reaction. Then from there, the Hydrogen ions need to be balanced, so the same numbers of Hydrogen ions are added to the opposite of the equation. Then it comes to the electrons, the same number of electrons added to a substance in the reduction half of reaction is taken away from the substance in the oxidation of half reaction. The last step is to add
The suffix -ic is given to the compound that contains the cation with the highest charge. To create the formula, you switch the charges, and that tells you how many of each element you will need. For example: Type 2 Ion Stock Name Latin Name Co2+ Cobalt (II) Ion Cobaltous Ion Co3+ Cobalt (III) Ion Cobaltic Ion Type 2 Compounds Stock System Latin System Charge of Metal Original Elements Co2O3 Cobalt (III) Oxide Cobaltic
Date : 18/02/2013 Micro-scale Determination of the Activation Energy of the Hydrogen Peroxide-Iodide Reaction Abstract: The purpose of this experiment was to determine the rate at which hydrogen peroxide decomposes to water and oxygen with the use of an iodide catalyst. Using the logarithmic form of the Arrhenius equation: ln k’ = -Ea/RT + ln A . the activation energy was determined to be 52.3 kJ/mol. It was also found that increasing the temperature also increased the rate, as there was more energy available to increase the speed of the reaction. Introduction: The purpose of this experiment was to determine the Activation Energy of the Hydrogen Peroxide-Iodide reaction.
Determining the Empirical Formula of Magnesium Oxide Lab Purpose The purpose of this lab was to determine the percent composition and empirical formula of magnesium oxide. Hypothesis If a strip of pure magnesium metal reacts with oxygen in the air to create magnesium oxide, then the molecular formula will be MgO. The percent composition for magnesium oxide would be 60.31% magnesium and 39.69% oxygen. Apparatus Refer to attached sheet Procedure Refer to McGraw-Hill Ryerson Chemistry 11, page 212-213. 4.