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And how do we know? Well, if we write the stoichiometric equation we have illustrated the :
Alternatively, we could write the net ionic equation...........
Given the stoichiometry,
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Given 7 equiv calcium atoms; 10 equiv of carbon atoms; and 9 equiv of nitrogen atoms, how many equiv of $"calcium cyanide"$ could we make?
$"Calcium cyanide"$ is formulated by taking the calcium ion, $Ca^(2+)$, and binding it to 2 equiv of the cyanide ion, $""^(-):C-=N$. So for $7xxCa$, $10xxC$, and $9xxN$, at most...
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How do you write the equation for this reaction: Potassium chloride and silver nitrate react to form potassium nitrate and silver chloride?
Formulas for the : $"KCl":$ potassium chloride (reactant) $"AgNO"_3":$ silver nitrate (reactant) $"KNO"_3":$ potassium nitrate (product) $"AgCl":$ silver chloride (product) $"KCl + AgNO"_3$$rarr$$"KNO"_3+"AgCl"$ If the compounds are in aqueous solution,...
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To make barium sulfate from 1 equiv barium nitrate, how many equiv of sodium sulfate are required?
$Na_2SO_4(aq) + Ba(NO_3)_2(aq) rarr BaSO_4(s)darr+ 2NaNO_3(aq)$ Barium sulfate is pretty insoluble stuff, and will precipitate from solution as a white solid. Its solubility in aqueous solution is negligible.
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How many nitrate ions, NO3-, and how many oxygen atoms are present in 1.00 microgram of magnesium nitrate, Mg (NO3)2? Also what mass of oxygen is present in 1.00 microgram of magnesium nitrate?
Number of nitrate ions $"Moles of Mg"("NO"_3)_2 = 1.00 × 10^"-6" color(red)(cancel(color(black)("g Mg"("NO"_3)_2))) × ("1 mol Mg"("NO"_3)_2)/(148.31 color(red)(cancel(color(black)("g Mg"("NO"_3)_2)))) = 6.743 × 10^"-9"color(white)(l) "mol Mg"("NO"_3)_2$ $"Moles of NO"_3^"-" = 6.743...
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If the percentage yield is 77.3 %, what is the yield of silver chloride when you
mix 16.7 mL of 0.7 mol/L silver nitrate with 1.7 mL of 0.668 mol/L sodium chloride?
This is a limiting reactant problem. We know that we will need a balanced equation, masses, and moles, etc., so let's gather all the information in one place. $M_text(r):color(white)(mmmmmmmmmmmmmmm)143.32$ $color(white)(mmmmmmm)"NaCl"...
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How many grams of silver chloride are produced when $"1.92 L"$ of a $"0.287-M"$ silver nitrate solution reacts with enough magnesium chloride?
So, you know that you're dealing with a between a solution of silver nitrate, $"AgNO"_3$, and solution of magnesium chloride, $"MgCl"""_2$ $2"AgNO"_text(3(aq]) + "MgCl"_text(2(aq]) -> 2"AgCl"_text((s]) darr + "Mg"("NO"_3)_text(2(aq])$...
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If $"100 mL"$ of $"0.01 mol/L"$ tetraaquadichlorochromium(III) chloride reacts with excess silver nitrate, how many mols of silver chloride get produced?
This is just a double replacement reaction in disguise. The balanced reaction has all coefficients of $1$: $"AgNO"_3(aq) + [stackrel(color(blue)(+3))("Cr")("H"_2"O")_4stackrel(color(blue)(-1))("Cl"_2)]stackrel(color(blue)(-1))("Cl")(aq) -> "AgCl"(s) + ["Cr"("H"_2"O")_4"Cl"_2]"NO"_3(aq)$ Only the ion in...
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What sort of solution will result if one equiv of hydrochloric acid is added to one equiv of calcium hydroxide? And how does $pH$ relate to $pOH$ in such solutions?
Whereas, calcium hydroxide gives TWO equivalents of hydroxide anion. The solution will thus be stoichiometric in $Ca(OH)Cl(aq)$, and thus there is still one equiv of $HO^-$ in solution. We could...
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How many equiv of nitric acid are required to oxidize one equiv of ammonia to give an half an equiv of dinitrogen gas?
$"Reduction half equation:"$ $HNO_3(aq) +H^(+) + e^(-) rarr NO_2(g) +H_2O(l)$ $stackrel(+V)Nrarrstackrel(+IV)N$ $"Oxidation half equation:"$ $NH_4^(+) rarr 1/2N_2(g)uarr +3e^(-) + 4H^+$ $stackrel(-III)Nrarrstackrel(0)N$ $3HNO_3(aq) +NH_4^(+)rarr 3NO_2(g) +3H_2O(l)+1/2N_2(g)uarr + H^+$ And we can...
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4. Suppose a laboratory has a 26 g sample of polonium 210. The half-life of Polonium 210 about 138 days. How many half-lives of polonium 210 occur in 276 days? How much polonium 210 is in the sample 276 days later?
As you know, the of a radioactive nuclide, $t_"1/2"$ represents the time needed for half of an initial sample to decay. This essentially means that a nuclide's half-life...
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