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To find the molar mass of a compound you would use to find the molar mass of each element separately. In our case, our two are beryllium and oxygen. You would find the molar mass of Be (9.01 g/mol) and O (16.00 g/mol), then you would add the two masses together to obtain the molar mass of the entire compound, which is 25.01 g/mol.
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What is the mass of one mole of beryllium if the atomic mass of beryllium is 9.01?
A mole is defined as the amount of a substance whose mass in grams equals the atomic, molecular, or formula-unit mass in units. Example 1: Water ($"H"_2"O"$) has two hydrogen...
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A student performed a laboratory activity where beryllium was reacted with hydrochloric acid. If they actually produced 4.5g of beryllium chloride, what was the percent yield?
$"% yield"$ $=$ $"Equivalence mass of product"/"Equivalent mass of reactant"xx100%$. You have a stoichiometric eqaution: $Be(s) + 2HCl(aq) rarr BeCl_2(aq) + H_2(g)$. And you have a mass of product....
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What is the formula and molar mass of beryllium chloride?
Recall that the formula mass is the sum of the atomic weights of the atoms in substance while it is in its empirical formula, and that the is the weight...
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A student found that 1.19 g of chromium ($Cr$) formed 1.74 g f chromium oxide. The molar mass of $Cr$ is 52.00 g/mol. What is the empirical formula of chromium oxide?
As with all these problems, we calculate the molar quantities of each substituent, and normalize them according to the masses of the atomic constituents: $"Moles of metal"$ $=$ $(1.19*g)/(52.00*g*mol^-1)=0.0229*mol$ $"Moles...
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Oxide ions are also formed when aluminium oxide is dissolved. What is the formula of an oxide ion?
We would have got the same formalism had we considered the formula of $Al_2O_3$, given that we know that aluminum commonly forms an $Al^(3+)$ cation. Molten alumina is used in...
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Ferric oxide may be reduced to pure iron either with carbon monoxide or with coke (pure carbon). Suppose that 150.0 lb of ferric oxide are available. How many pounds of carbon monoxide would be required to reduce the oxide?
The answer relates to the stoichiometric equation, which tells us that $159.7*g$ $Fe_2O_3$ reacts with $84.0*g$ $CO$ to give $112*g$ $Fe$. You have $150*"lbs"xx454*g*"lb"^-1$ $=$ $68,100*g$ $Fe_2O_3$. Given the equations...
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What is the formula mass of beryllium chlorate, $Be(ClO_3)_2$, in atomic mass units?
Use to look up the atomic masses of the in the compound. Then multiply the for each element times its subscript, and add them together. $"Be":$ $"9.0122 u"$ $"Cl":$ $"35.45...
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What mass in grams of iron(III) oxide contains 71.6 g ofiron? Iron(III) oxide is 69.94% iron by mass.
A substance's essentially tells you how many grams of each constituent element you get per $"100 g"$ of said substance. In this case, a percent composition of $69.94%$...
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A mass of $2.40*g$ of calcium oxide is obtained by heating a mass of $5.00*g$ calcium carbonate. What is the stoichiometric equation that represents the formation of calcium oxide, and what is the percentage yield?
$CaCO_3(s) + Delta rarr CaO(s) + CO_2(g)uarr$ The $Delta$ symbol represents heat, and you have to fiercely heat these carbonates to effect decomposition. Note that this reaction is certainly stoichiometrically...
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If a mass of $"16.26 mg"$ contains $1.66 xx 10^20$ atoms, what is the molar mass of that atom? If you have $"1 million"$ silver atoms constituting a total of $1.79 xx 10^(-16) "g"$, what is the molar mass? $"1 amu"$ $=$ $1.660599 xx 10^(-24) "g"$.
Both questions ask the same thing in opposite ways. One gives you $"16.26 mg"$ containing $1.66xx10^20$ $"atoms"$. That gives you a mass and a quantity, which is enough to convert...
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