In this reaction, calcium is being oxidised. In 2Ca, its oxidaton state is 0 and after the reaction it is increased to +2 which forms a bong with oxygen ion. Methods for preparation of calcium oxide: 2Ca + O2 = 2CaO (above 300° C, burning on air). The two half equations for this reaction are: Ca -> Ca 2+ + 2e - (this reaction shows oxidation). A) CaCO3 → CaO + CO2 It is a Thermal decomposition reaction. 2Ca + O 2 2CaO This reaction can also be classified as synthesis (combination) reaction Single Replacement (Single Displacement) – one element replaces similar element in compound Calcium undergoes oxidation reaction to form Calcium oxide(quick lime). B) 2Ca + O2 → 2CaO It is combination reaction as two reactants react to form a single product. Our channel. On the products side, the oxidation state of Ca is +2 while that of oxygen is -2. The reaction of calcium with oxygen, which is expressed by the equation 2Ca + O2 --> 2CaO is a synthesis reaction. For example, C6H5C2H5 + O2 = C6H5OH + CO2 + H2O will not be balanced, but XC2H5 + O2 = XOH + CO2 + H2O will. For this, we need to identify their oxidation numbers. View Notes - Solubility from CHM 1101 at University of Ottawa. Thus, as Ca is oxidized while O is reduced and this is a redox reaction. CaH2 + O2 = CaO + H2O (300-400° C). 2Ca + O 2 2CaO [ Check the balance ] ... Find another reaction. and O 2 + 4e - -> 2O 2-(this reaction shows reduction) Therefore, you can conclude that this reaction is a redox reaction because it involves both reduction and oxidation. CaCO3 = CaO + CO2 (900-1200° C). The amount of oxygen present and the temperature determine whether the reaction is complete or incomplete. However, this is not a precipitation reaction. Approved by eNotes Editorial Team Posted on October 10, 2011 at 9:46 PM It is a redox reaction (reduction and oxidation both occur) On the reactants side, the oxidation states of both Ca and O2 are 0. How To Balance Equations You can use parenthesis or brackets []. Classify these elements by whether they get oxidized or reduced in the reactions shown here: (Ech element A) 2Ca(s)+O2(g)→2CaO(s) B) F2(g) + 2Li(s) ------> 2LiF Identify the oxidizing agent and the reducing agent in each reaction below. 2Ca + O2(g) —> 2CaO(s) Step 1: Determine the oxidizing agent and the reducing agent. Compound states [like (s) (aq) or (g)] are not required. Half Reactions 2 Ca (s) + O2 (g) 2CaO (s) Step 1: The oxidation half-reaction shows electrons being lost by an element (electrons are Thermodynamic properties of substances The solubility of the substances Periodic table of elements. where heat energy is supplied to split calcium carbonate into calcium oxide and carbon dioxide. Equation: 2Ca + O_2 --> 2CaO 2Ca + O 2 (g) —> 2CaO(s) 0 0 (+2) (-2) Both of the reactants have the oxidation number zero. 2Ca (g) + O 2 (g) -> 2CaO (s), . Picture of reaction: Сoding to search: 2 Ca + O2 cnd [ temp ] = 2 CaO. 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