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Look at the double replacement reaction chart. The rules are followed in order. Let's look at $\ce{KNO3}$ first. The first rule states that alkali metal salts are soluble. Potassium is an alkali metal, therefore potassium nitrate is soluble. The second product is $\ce{Pb(OH)2}$.
In normal displacement reactions, reactivity plays a large role and sometimes the reaction doesn't even happen. So is there anything limiting double displacement reactions? For example $\ce{2KI + Pb(NO3)2 -> 2KNO3 + PbI2}$. If reactivity plays a role in this reaction, why does it occur? Isn't the halogen ion (iodide) more reactive than $\ce{NO3-}$?
Question: DOUBLE REPLACEMENT REACTION FOLLOWED BY DECOMPOSITIONFormation of a gasa. Observations:b. Complete and balance this reaction equation: (Hint: See eqns. 6 and 7.)Na2CO3 (s)+HCllongrightarrowc. Write the formula for the gas evolved.d.
I was taught that double displacement reactions occur when reactants are aqueous. However, I came across this reaction $$\ce{ZnO(s) + H2S (g) -> ZnS(s) + H2O (g)}$$ This is the reaction that is used to remove hydrogen sulfide that is naturally found in methane gas. This reaction indeed looks like a double replacement reaction.
Question: Which products would result from the double replacement reaction between MgCl2 (aq) and Na2CO3 (g)? NaCl (aq) and MgCO3 (3) Na2Cl2 (aq) and MgCO3 (3) MgNa2 (aq) and CO3Cl2 (aq) NaCl (aq) and MgCO3 (3) NaCl (aq) and Mg (CO3)2 (3) Here’s the best way to solve it.
With double replacement reactions you generally either get: 1.) A neutralization reaction. HCl(aq) +NaOH(aq) NaCl(aq) +HX2O(l) H C l (a q) + N a O H (a q) N a C l (a q) + H X 2 O (l) 2.) Gas displacement.
Precipitation of silver chloride is a common example of a double replacement reaction. e.g. . Initially all four ions are present in solution. When the solutions are mixed the silver and chloride ions bond together and precipitate, leaving the sodium and nitrate ions remaining in solution along with a small number of silver and chloride ions ...
Yes, you were right in concluding that there are no spectator ions. How is that a problem? There is no commandment that says "Thou shalt not have two precipitates in one reaction". Indeed, such double precipitations are very much possible, though rare. The most famous example is probably the formation of lithopone.
Complete and balance the following chemical equation for a double replacement reaction: CuCl2 (aq) + Na2S (aq) → ? + NaCl (aq) Your solution’s ready to go! Our expert help has broken down your problem into an easy-to-learn solution you can count on.
EXPERIMENT 10 Double Replacement Reactions Driving Forces for Double Replacement Reactions So far, we have indicated that evidence for a double replacement reaction having occurred can be either (a) the formation of a precipitate, (b) the formation of a gas or (c) a temperature change this may be either a temperature increase, as in the case of reaction (9), or a temperature decrease).