What observation suggests that carbon dioxide is a product of the combustion of ethyne?
Carbon dioxide .... If you were to perform the reaction in a sealed container where the reactants are in a stoichiometric ratio, the fire will go out before the reactants are consumed. The denser CO2 will "smother" the fire. If the gas being given off is bubbled into water containing bromthymol blue, an acid-base indicator, the solution will turn from green to yellow as the dissolved CO2 acidifies the water. CO2(g) + H2O(l) <==> H+ + HCO3^- ... acidic solution ("carbonic" acid") A similar demo which is even easier is to put a wet piece of blue (or neutral) litmus paper in the gas coming off the combustion. The indicator paper will turn red indicating the formation of an acid. Bubble the gas coming off into a saturated solution of calcium hydroxide. The solution will turn cloudy as insoluble calcium carbonate is formed. This is a classic test for CO2. It is called the "lime-water" test. Ca(OH)2(aq) + CO2(g) --> CaCO3(s) + H2O(l) Example of lime-water test: https://www.youtube.com/watch?v=_wzJQFl1...
Does a combustion reaction always produce water and carbon dioxide?
No. For example, the combustion of sulfur produces sulfur dioxide. S(l) + O2(g) --> SO2(g) The combustion of carbon produces carbon dioxide. The combustion of hydrogen produces water. The combustion of hydrocarbons producecarbon dioxide and water.
Limewater reacts with carbon dioxide (CO2) in a two step process. Limewater is calcium hydroxide dissolved in water.Ca(OH)2 + H2O -> Ca++ + 2OH-Then, the Ca++ reacts with the CO2 to give calcium carbonate which is very insoluble in water:Ca(OH)2 + CO2 -> CaCO3 + H2O (CaCO3 will precipitate, creating a milky solution)In the presence of more, or excess, CO2, the CaCO3 reacts with more Co2 to give calcium bicarbonate, which is water soluble: CaCO3 + CO2 -> Ca(HCO3) + H2O So the milky appearance goes away as the insoluble CaCO3 reacts forming the soluble Ca(HCO3)2. The magic is explained.
[math]Ca(OH)_2(aq) + CO_2(aq) → CaCO_3(s)+ H_2O(l)[/math]Well lime water is SATURATED calcium hydroxide….and the reaction of limewater with carbon dioxide results in a precipitate of insoluble calcium carbonate, and water…And so calcium hydroxide and carbon dioxide gives calcium carbonate and water. The balanced equation is a given; I finally managed to nut out the format. And it shows the action of carbon dioxide as an acidic oxide, i.e. the acid anhydride of carbonic acid…Note that in the lab, one of the best sources of aqueous carbon dioxide is sparkling mineral water…this is water SUPERSATURATED with carbon dioxide…
What is formed when carbon dioxide and water react?
CARBONIC ACID & ACIDIC Carbon dioxide dissolves slightly in water to form a weak acid called carbonic acid, H2CO3: CO2 + H2O H2CO3 Carbonic acid reacts slightly and reversibly in water to form a hydronium cation, H3O+, and the bicarbonate ion, HCO3-: H2CO3 + H2O HCO3- + H3O+ This chemical behavior explains why water, which normally has a neutral pH of 7 has an acidic pH of approximately 5.5 when it has been exposed to air. It also explains the burning/stinging sensation in your nose and eyes when you inhale too quickly from a freshly-opened container of soda pop; the gas quickly reacts with the water in your eyes and nose to form a small amount of carbonic acid.
Limewater is used as a test for the presence of carbon dioxide. Suppose I am doing an equation, I can see that a gas is being given off, but I need to check the identity of this gas. The limewater test helps me identify that it is CO2.Limewater is made of aqueous Ca(OH)2Ca(OH)2 + CO2 => CaCO3 + H20CaCO3 does not dissolve in water at room temperature, so forms a white precipitate (solid). Therefore, if this solid forms, you know that the identity of the gas is carbon dioxide. You may then be able to deduce that whatever produced the gas was a carbonate of some sort.
The molecular formula of octane is C8H18.The combustion of a hydrocarbon produces carbon dioxide and water. Thus the combustion of octane is given by -C8H18 + O2 ---> CO2 + H2OTo balance this equation, we need to balance the atoms on the left and right hand side. Octane has an excess of C and H and we use it as a reference. There are 8 carbon atoms and 18 hydrogen atoms in an octane molecule. Thus there should be 8 carbons and 18 hydrogens on the right, which is obtained by a prefix of 8 for CO2 and 9 for H2O.C8H18 + O2 ---> 8CO2 + 9 H2ONow we have to balance the oxygen atoms. On the right side, there are (8X2)+9 = 25 atoms. Thus we can balance the oxygen atoms by putting a prefix of 25/2 on the left side.C8H18 + 25/2 O2 ---> 8CO2 + 9 H2O.To obtain a equation containing whole numbers, we multiply the entire equation by 2. This gives the final equation.2 C8H18 + 25 O2 ---> 16 CO2 +18 H2O.
Are the products of combustion of a hydrocarbon are carbon dioxide and water?
Always? That is a very strong word to use in science. If I burn Magnesium ribbon I get Magnesium Oxide, no CO2 no H2O. In objective science words like never and always are seldom used. On the other hand if you burn hydrocarbons you WILL get CO2 and H2O - almost always. Depends on the conditions. In a low oxygen environment you can get Carbon monoxide instead of Carbon dioxide, usually a mixture. An example is a car exhaust - mostly CO2 and H2O but enough CO as well to kill you. The reason with hydrocarbons of course is that they are compounds that contain Carbon and Hydrogen, hence the name. So in summary CO2 and H2O are not "always" the products of combustion. They often are because the things we burn are usually based on the natural world and so contain Carbon and Hydrogen. These things are generally called hydrocarbons. Hope that is enough and good luck. Gary
When carbon dioxide is passed through lime water which is a diluted solution of Ca(OH) 2, it turns milky due to the formation of calcium carbonate which is CaCO3.The reaction is like this:Ca(OH) 2 + CO2 → CaCO3 + H2OIf you pay a little more attention, you will be able to observe that it is a neutralization reaction, where base is Ca(OH)2 and acid is H2CO3 and a salt CaCO3 and H2O are formed.So, actually the above reaction is a short form of actual reaction.Actually CO2 is no more CO2 after dissolving in water, it becomes H2CO3 via addition reaction as shown :CO2+H2O→ H2CO3Now, this CaCO3 is insoluble in water which is the reason behind the milkiness of solution.However if excess carbon dioxide is passed, the milkiness disappears, think about it… milkiness was due to CaCO3 and now the milkiness is disappeared… this must mean that CaCO3 is no more left and git converted into something.That something is actually calcium bicarbonate which is soluble in water and hence the solution becomes clear.The reaction is as follows :CO2+H2O→ H2CO3CaCO3 + H2CO3 → Ca(HCO3)2This is because…Carbonate + carbonic acid gives 2 bicarbonatesCO3 2- + H2CO3 → 2 HCO3-This is due to proton transfer.So… H2CO3 gives H+(acting as acid) and CO3 2- accepts it(acting as a base).This clearly means that, it is an acid base reaction in which no water is formed(coz its proton transfer)Hope it helps.
Chemistry reaction question? combustion?
It's a decomposition. Decomposition will always have only one reactant and at least two products because you're taking one compound and breaking it into two or more substances which can be either an element or a compound. Combustion reactions must have at least two reactants and can have any number of products. Combustion basically means that something, whether it be a compound or and element, is reacting with O2, and each element or compound on the reaction side will combine with oxygen on the product side (I hope that wasn't too confusing). Also, H20 and CO2 are the products of a combustion if you're combusting a hydrocarbon (hydrocarbon is a compound made up of both hydrogen and carbon such as C2H6). So if C2H6 reacted with O2 (because again a combustion just means its reacting with O2) then H20 an CO2 would be the products. But if you're not combusting a hydrocarbon that rule doesn't apply. Hope this made sense!