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K(s)+H2O ---- gt;???? - Socratic This is formally a redox reaction Potassium is an active alkali metal, that is capable of being oxidized by the water molecule stackrel(0)K(s) + stackrel(+I)H_2O(s) rarr stackrel(+I)KOH(aq) + 1 2stackrel(0)H_2(g)uarr Now you do this sodium, and the reaction is pretty zippy You do with potassium, a more potent reductant, and this is even zippier
How would you balance HCI + NaOH -- gt;H20 + NaCI? - Socratic Well in fact you have already balanced this In every chemical reaction, mass is conserved, and it is conserved in the acid base reaction above If there are 5 g of reactant there must be 5 g of product This is an example of stoichiometry To put this in another context, suppose you went to a shop with a £20-00 note, and made a purchase worth £8-15 If you received £5-85 in change, would
How do you balance and translate this reaction: - Socratic If we combine these we can obtain 1mole of H2O #Ca(OH)_2 + H_2SO_4 = 2H_2O + CaSO4# Now you can write down the ionic reaction #Ca^(2+) + 2OH^(-) + 2H^(+) + SO4^(2-) = 2H_2O+ Ca^(2+) + SO4^(2-)# (I know that SO4^-2 is confusing So I recommend you that to determine the charge of an ion Use the zero sum rule )
How do you balance _C4H16+_O2-- gt; _CO2+_H2O? I have tried to . . . - Socratic Combustion of butane: C_4H_10(g) + 13 2O_2(g) rarr 4CO_2(g) + 5H_2O(g) Hydrocarbons (of all stamps) react with oxygen to give CO_2 and H_2O Sometimes the carbon in hydrocarbons, where oxygen is limited, react to give particulate C, and gaseous CO (this occurs particularly in diesel engines) Balance the carbons (as CO_2 for complete combustion), then the hydrogens (as water), and then the
How would you find a balanced equation if acetylene gas Hydrogen sulfide reacts with sulfur dioxide to give H2O and S, H2S + SO2 = H2O + S(solid), If 100 mL of HCl gas at 300 K and 200 kPa dissolved in pure water requires 12 50 mL of the NaOH If 100 mL of HCl gas at 300 K and 100 kPa dissolved in pure water requires 12 50 mL of the NaOH
If 0. 454 kg of nitroglycerin explodes according to the following . . . As you know, nitroglycerine explosively decomposes we get approx 100*mol of gas produced 4O_2NOCH_2CH(ONO_2)CH_2(ONO_2)rarr6N_2(g) +12CO(g) + 10H_2O(g) + 7O_2(g) is I think the stoichiometric reaction and it is smokeless combustion there are no SOLID forms of carbon, whose emission would give away the location of your artillery piece, or whatever it is you use to kill people
How many grams of water are produced when propane (C3H8 . . . - Socratic 7 72 "g H"_2"O" The NIE for the complete combustion of propane is: "C"_3 "H"_8 + 5 "O"_2 -> 3 "CO"_2 + 4 "H"_2"O" The problem doesn't state how much propane is burned, so we're going to assume that there is enough to use up all the oxygen To find out how much that is, we need to convert liters of "O"_2 to moles of "O"_2 using the fact that at STP, a mole of gas is equivalent to 22 4 liters