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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.
Formula Mass of
For more information about atomic mass units and unified mass units, see the following link:
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An average sample of chlorine contains 75.77% chlorine-35, with an atomic mass of 34.969 amu (atomic mass units), and 24.23% chlorine-37, with an atomic mass of 36.966 amu. What is the average atomic mass of chlorine?
The weighted average is the sum of each individual nuclide, multiplied by its isotopic abundance. So, we simply do the arithmetic: $0.7577xx34.969+0.2423xx36.966 = ???$ amu Then look at to...
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What is the total number of atoms in the compound $Ca(ClO_3)_2$?
Given: $Ca(ClO_3)_2$ The compound is Calcium chlorate. The Parentheses is a multiplier for all of the inside the parentheses. $"Element Symbol No. of Atoms"$ Calcium $" "Ca: "...
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What is diference between sodium chlorate (I) and sodium chlorate (V)?
And $"sodium chlorate(V)"$ is the old sodium chlorate, $NaClO_3$. $ClO_4^-$; i.e. $Cl(+VII)$, $"perchlorate."$ $ClO_3^-$; i.e. $Cl(+V)$, $"chlorate."$ $ClO_2^-$; i.e. $Cl(+III)$, $"chlorite."$ $ClO^-$; i.e. $Cl(+I)$, $"hypochlorite."$ $Cl^-$; i.e. $Cl(-I)$, $"chloride."$ And...
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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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What mass of precipitate will form if 1.50L of excess $Pb(ClO_3)_2$ is mixed with 0.100L of 0.270 M $NaI$? Assume 100% yield.
Start by writing a balanced chemical equation for this $"Pb"("ClO"_3)_text(2(aq]) + color(red)(2)"NaI"_text((aq]) -> "PbI"_text(2(s]) darr + 2"NaClO"_text(3(aq])$ Lead(II) chlorate will react with sodium iodide to form lead(II)...
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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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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 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 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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