In a reaction, the substance undergoing oxidation serves as the...(mult choices in detail portion)?
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d) Reducing agent. Oxidation is the loss of electrons. The substance getting oxidized donates the electrons to the subnstance getting reduced. For that reason, a) Electron donor is also correct.\n\nI don't know if you're allowed more than one answer to this question. It may be that the teacher did not see that the reducing agent was an electron donor, and thought of electron donation in the Lewis base sense, which does not come up in this question.
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It should be a) oxidizing agents.
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a) [O 2-]\nb) [ I - ]\nc) [Na+]\nd) [Al 3+]\ne) [Ni 2+]\nf) [Mg 2+]
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e.g. of formula: Magnesium+oxygen=magnesium oxide\ne.g. of Mixture: Air\ne.g. of Compound: Magnesium oxide
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CO2\nCarbon Dioxide\nHere is the reaction:\nHC2H3O2(aq) + NaHCO3(aq) ----> NaC2H3O2(aq) + H2O(l) + CO2(g)
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Different chemical composition, one has a reaction the other doesn't..☺
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strictly speaking, substances undergo combustion in the presence of oxygen and 'burn' would not be precise. \nhowever answering the question, oxygen is an oxidising substance and hence it is able to oxidise the organic subs. and usually converting them into carbon di oxide and water, and this is accompanied by the release of energy in the form of heat
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A) an oxidation reaction\n\nthat's why they are called redox
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Thier all chemical reactions.
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It is simply sum of products minus sum of reactants\n\n[H2O + N2] - [O2 + NH3]\n\nSince this is a 1 to 1 ratio reaction, the coefficients are one. (if there was a coefficient for NH3, you must multiply the enthalpy value of NH3 by that # because that is how many moles you have, and the value given is for only one mole.)
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I'm assuming you're asking for the reactions.  Here are a couple:\nH2 + F2 → 2HF \n\n4Fe + 3O2 → 2 Fe2O3
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U CAN MAKE A PROJ ON REACTIONS ON THE FOLLOWING PTS  .\n INTRO OF REACTIONS\nDEFINITION OF A REACTION\n TYPES OF REACTIONS\n THEN, DESCRIBE THEM SEPARATELY
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You must figure out the oxidation number of each element in an equation.  The substance oxidized goes up in oxidation number (becomes more positive) and the substance reduced goes down in oxidation number (becomes more negative).  The substance that is oxidized is the reducing agent (causes reducing in the other element) and the substance that is reduced is the oxidizing agent (causes oxidation in the other element).\nSO . . .\nin (a) carbon on the left side is -4 and on the right side is +4 so it is oxidized and CH4 is the reducing agent\n     oxygen on the left side is zero (all elements are zero) and on the right side is -2 so it is reduced and O2 is the oxidizing agent\nin (b) zinc on the left is zero and is +2 on the right, so it's oxidized and Zn is the reducing agent\n     hydrogen on the left is +1 and is 0 on the right, so it's reduced and HCl is the oxidizing agent\nI'll leave the rest for you!
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2\nthe reaction is\nCa(OH)2+2HNO3=2H2O+Ca(NO3)2
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If an element combines with another element to form more than one compound, the various weights of one compound which combine with the fixed weight of the other element bear a simple ratio to one another eg\nCarbon Monoxide C 12  + O 16\ncarbon Dioxide  C 12  + O 32\nRatio of 1 to 2
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in oxidations and reductions..
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Oxidation.  \n\nWhen an ion or atom gains an electron, it's reduction.  When both reactions happen, then it's redox.