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A chemist hypothesizes that mercury oxide ($HgO$) will undergo a decomposition reaction reaches a temperature. When the chemist designs his experiment what should be the only independent variable?
The independent variable of an experiment is the thing you change. In this case, what we are changing will be the temperature. This will allow us to find the...
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How do you write an equation to represent "Azomethane ($C_2H_6N_2$) decomposes to form ethane ($C_2H_6$) and nitrogen gas"?
All you have to do here is make sure that the chemical equation that describes this decomposition reaction obeys the . Azomethane, $"C"_2"H"_6"N"_2$, is said to decompose to form...
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How do you balance $HgO -> Hg + O_2$?
How would you remove the half coefficient on the oxygen? What does the $Delta$ symbol mean here?
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Is the equation, $2Hg + O_2 = 2HgO$ a synthesis, decomposition, or exchange reaction?
The equation $2Hg+O_2->2HgO$ is under the form of: $"Element "+" Element"->Product$ which is the general form of a synthesis reaction. It is similar to $2H_2+O_2->2H_2O$ for the synthesis of water.
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What type of reaction is $HgO -> Hg + O_2$?
Reddish Mercury(II)oxide solid is decomposed (broken down) upon heating into silver liquid mercury and colourless oxygen gas. The full balanced chemical equation is $2HgO->2Hg+O_2$
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When hydrogen peroxide decomposes naturally, what are the products?
Hydrogen peroxide, $H_2O_2$ (very slowly) decomposes naturally into water and oxygen gas. $2H_2O_2(l)->2H_2O(l)+O_2(g)$ This is an exothermic reaction, so heat is also evolved.
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Zena, warrior princess, had a rock with $HgO$ in it. If she had 60 grams of Mercury after heating the rock, how many moles of $HgO$ was in the rock?
She got $60*g$ of mercury metal....this represents a molar quantity of $(60*g)/(200.6*g*mol^-1)=0.299*mol$ with RESPECT to the metal. And thus there were $0.299*mol$ with respect to mercuric oxide... $HgO(s) + Delta...
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$"Mg"("HSO"_3)_2$ decomposes into a solid $"X"$, $"H"_2"O"$ vapor, and $"SO"_2$ gas. If $"186 g"$ of $"Mg"("HSO"_3)_2$ decomposes completely and leaves behind $"40 g"$ of solid $"X"$, what is the identity of $"X"$?
Start by writing the unbalanced chemical equation that can describe this decomposition reaction. $"Mg"("HSO"_ 3)_ (2(s)) -> "X"_ ((s)) + "H"_ 2"O"_ ((g)) + "SO"_ (2(g))$ Now, focus...
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If at a certain temperature, $"6.8 g"$ of $"NH"_3$ completely decomposes to form $"H"_2(g)$ and $"N"_2(g)$, how many mols of $"Al"(s)$ would be needed to react with excess aqueous $"HCl"$ to form the same amount of $"H"_2(g)$?
The idea is to see how many mols of $"H"_2$ you would have made in one reaction and reuse that value in the context of the other reaction. Assuming you...
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The $DeltaH$ value for the reaction $1/2O_2 (g) + Hg(l) -> HgO (s)$ is -90.8 kJ. How many kJ are released when 66.9 g $Hg$ is reacted with oxygen?
Start by taking a look at the thermochemical equation given to you $1/2"O"_ (2(g)) + "Hg"_ ((l)) -> "HgO"_ ((s))" "DeltaH = -"90.8 kJ"$ This equation tells you...
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