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Potassium chlorate decomposes to potassium chloride and oxygen gas. Is this a physical or chemical change?
Chemical change is characterized by the formation of new substances, and the making and breaking of strong chemical bonds. Here, we have the reaction: $KClO_3(s) + Delta rarr KCl(s) +...
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When 2 moles of potassium chlorate crystals decompose to potassium chloride crystals and oxygen gas at constant temperature and pressure, 44.7 kJ are given off. What is the thermochemical equation?
A thermochemical equation is simply a chemical equation that contains information about the change of reaction, $DeltaH_"rxn"$. The first thing to do when writing a thermochemical equation is to...
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Potassium chlorate, $KClO_3$, decomposes to form potassium chloride, $KCl$ and oxygen gas. How do you write a balanced equation for this decomposition reaction?
$"KClO"_3("s")" + heat"$$rarr$$"KCl(s)" + "O"_2("g")"$ Notice that the number of atoms of $"K"$ and $"Cl"$ are the same on both sides, but the numbers of $"O"$ atoms are not. There...
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How do you write the formula for this reaction: Potassium chlorate decomposes to potassium chloride and oxygen gas?
Formula for Potassium chlorate is $KClO_3$. Formula for Potassium chloride is $KCl.$ Formula for Oxygen gas as molecule is $O_2.$ $:.$ Reaction is : $KClO_3$ $rarr$ $KCl$...
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The decomposition of potassium chlorate ($KClO_3$) is used as a source of oxygen in the laboratory. How much potassium chlorate is needed to produce 19.7 mol of oxygen?
Normally, this rxn must be calalyzed with a little $Mn(IV)$ salt, but we address the question with this . We spit out a $19.7*mol$ quantity of dioxygen gas. Given the...
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When sodium chlorate (I), NaClO is heated, sodium chlorate (V) and sodium chloride are formed. What is the ionic equation for this reaction? What type of reaction is this?
$"Oxidation:"$ $stackrel(I^+)ClO^(-) + 2H_2Orarr stackrel(V^+)ClO_3^(-)+4H^+ +4e^(-)$ $(i)$ $"Reduction:"$ $stackrel(I^+)ClO^(-) + 2H^+ + 2e^(-) rarr stackrel(""^(-)I)Cl^(-)+H_2O$ $(ii)$ And so we takes....$(i)+2xx(ii)$ $stackrel(I^+)ClO^(-) +2stackrel(I^+)ClO^(-) cancel(+2H_2O+ 4H^+ + 4e^(-))rarr stackrel(V^+)ClO_3^(-)+2stackrel(""^(-)I)Cl^(-)cancel(+4H^+ +2H_2O+4e^(-))$ ...to give....after...
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If a $2.96*g$ mass of potassium chloride, and a $1.92*g$ mass of dioxygen gas react, what mass of $"potassium chlorate"$ results?
There are $x*g$ $KClO_3$........... And we recover $(2.96*g)/(74.55*g*mol^-1)=0.0397*mol$ with respect to $KCl$. And $(1.92*g)/(15.999*g*mol^-1)=0.120*mol$ with respect to $"oxygen"$. Clearly, there were $0.0397$ $"mol"$ with respect to $KClO_3$. And...
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A sample of an unknown metal chlorate, weighing 5.837 g, is heated until all of the oxygen is driven off. The residue remaining in the container weighs 1.459 g. What is the percentage of oxygen in this metal chlorate?
While I have given the stoichiometric equation for the decomposition of the metal chlorate, this reaction is simpler than it seems. We know that a mass of $5.837-1.459=4.378$ $g$ was...
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In the decomposition of potassium chlorate, how many moles of potassium chlorate are needed to produce 50 moles of oxygen gas?
You'd need 33.3 moles of potassium chlorate, $KClO_3$, to produce that much oxygen. All you need in order to answer this question is the balanced chemical equation for the of...
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A teacher makes a saturated solution of potassium chlorate in 100g of 50°C water. The water cools down to 20°C. How much potassium chlorate precipitates out of the solution?
The teacher made a saturated solution. AS specified, the amount of potassium chlorate in solution is equal to the amount of that would be in equilibrium with undissolved solute. Now,...
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