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If an Alka-Seltzer tablet contained 309 mg of aspirin, $1.927 xx 10^03$ mg of sodium hydrogen carbonate, and $1.004 xx 10^03$mg of citric acid and nothing else, what is the percent, by mass, of sodium hydrogen carbonate in the tablet?
Percent composition is determined by dividing the mass of the specified compound by the total mass, then multiply by 100. $"Percent composition"="mass of specified component"/"total mass"xx100"$ Add the masses of...
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Decomposing calcium carbonate yields calcium oxide and dioxide. What information is needed to calculate the mass of calcium oxide that can produced from 4.7 kg of calcium carbonate?
The balanced chemical equation The molar mass of $"CaCO"_3$ The molar ratio of $"CaO"$ to $"CaCO"_3$ The molar mass of $"CaO"$ Your strategy has four steps:...
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Calcium carbonate decomposes to form calcium oxide and carbon dioxide gas. If 44.5 grams of calcium oxide is produced, how many grams of calcium carbonate had to decomposez?
We need a stoichiometric reaction that represents the decomposition of calcium carbonate: $CaCO_3(s) + Delta rarr CaO(s) + CO_2(g)uarr$ And thus calcium oxide and calcium carbonate are present in equimolar...
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What mass of $"calcium carbonate"$ is equivalent to $"Avogadro's number"$ pf formula units of $CaCO_3$?
$6.022xx10^23$ units of ANYTHING, specifies 1 mole of that thing, i.e. $N_A$ individual units of that thing........... And thus in $1*mol$ of $CaCO_3$, $N_A$ formula units, there are: $N_A$...
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How do you calculate the percentage of calcium in calcium carbonate, $CaCO_3$?
You take the atomic mass of calcium over the atomic mass of $CaCO_3$ and multiply it by 100 to get the percentage. The mass of $Ca$ is 40.078 g; the...
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A $2.03*g$ mass of calcium salts contains $1.33*g$ calcium carbonate. What is the $%$ calcium carbonate; and what is the percentage by mass of of calcium in calcium carbonate?
So we have the $"%calcium carbonate, "m/m$. We are not finished yet, because we have to address the percentage by mass of calcium metal in calcium carbonate: $%Ca=(40.08*g*mol^-1)/(100.09*g*mol^-1)=40%$ with respect...
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How many mols $CaCO_3$ can be dissolved in .0250 mol $HCl$ in the equation $CaCO_3 + 2HCl -> CaCl_2 + H_2O + CO_2$?
The equation says $CaCO_3 + 2HCl$, which means that for every $2$ moles of $HCl$ there is one of $CaCO_3$. This is called the molar ratio, in this case...
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Calcium oxide and carbon dioxide are produced from the decomposition of calcium carbonate. How many moles of calcium carbonate are needed to produce 15.0 grams of the calcium oxide?
We interrogate the stoichiometric equation...... $CaCO_3(s) + Delta rarr CaO(s) + CO_2(g) uarr$ We require a molar quantity of $(15.0*g)/(56.08*g*mol^-1)=0.268*mol,$ with respect to $"calcium oxide"$. And clearly, we need a...
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Upon heating, calcium carbonate decomposes to produce calcium oxide and carbon dioxide. What is the theoretical yield of $CO_2$ if 235.0 g $CaCO_3$ is heated?
$CaCO_3(s) + Delta rarr CaO(s) + CO_2(g)uarr$ There is thus a 1:1 molar equivalence of carbonate to carbon dioxide. $"Moles of calcium carbonate"$ $=$ $(235.0*g)/(100.0869*g*mol^-1)$ $=$ $2.35$ $mol$. So, by...
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$CO_2$ gas, in the dry state, may be produced by heating calcium carbonate. $CaCO_3 (s)DeltaCaO(s) + CO_2(g)$. What volume of $CO_2$, collected dry at 55 C and a pressure of 774 torr, is produced by complete thermal decomposition of 10.0 g of $CaCO_3$?
$10gramsCaCO_3(s) => CaO(s) + (?)O_2(g)$ $"moles" CaCO_3 = ((10g)/(100(g/(mol))))$ = $0.10"mole"$ From reaction ratios => moles $CaCO_3(s)$ consumed = moles $O_2(g)$ produced = 0.10 mole $(O_2(g))$**** If a 'dry'...
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