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The molar mass of barium nitrate ($Ba(NO_3)_2$) is 261.35 g/mol. What is the mass of $5.30 x 10^22$ formula units of $Ba(NO_3)_2$?
It is fact that $6.023xx10^23$ formula units of barium nitrate have a mass of $261.35*g$. This is what we specify when we say molar mass. And thus the mass of...
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When the equation $Ni(NO_3)_3 + PbBr_4 -> NiBr_3 + Pb(NO_3)_4$ is balanced, what is the coefficient for $Ni(NO_3)_3$?
$"Typical oxidation states of nickel are 0, +I, +II, "and rarely" +IV.$
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How do you balance $Cr + Fe(NO_3)_2 -> Fe + Cr(NO_3)_3$?
We write the oxidation rxn: $CrrarrCr^(3+) + 3e^-$ $(i)$ And then the reduction rxn: $Fe^(2+) +2e^(-) rarr Fe$ $(ii)$ And then cross mulitply, $2xx(i) +3xx(ii)$ $2Cr+3Fe(NO_3)_2 rarr 3Fe +...
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How do you balance $Cr(s) + Fe(NO_3)_2(aq) -> Fe(s) + Cr(NO_3)_3(aq)$?
Chromium metal is oxidized.......... $Cr(s) rarrCr^(3+) +3e^(-)$ $(i)$ And $Fe^(2+)$ is reduced........... $Fe^(2+) +2e^(-) rarr Fe(s)$ $(ii)$ And we cross multiply to multiply to remove the electrons: $2xx(i)+3xx(ii):$ $3Fe^(2+)+2Cr(s) rarr...
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What is the missing coefficient in the balanced equation? What type of reaction is it? $Mg(OH)_2 + H_2SO_4 -> MgSO_4 + ?H_2O$
are balanced with respect to mass and charge. For every reactant particle, there is a corresponding product particle. And for every reactant charge, there must be a corresponding product...
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$Cu(NO_3)_2 + Zn(s) -> Cu(s) + Zn(NO_3)_2$ is an example of which type of reaction?
$Cu^(2+)$ is reduced to copper metal. Zinc metal is oxidized to $Zn^(2+)$. Formal electron transfer has taken place between the ion and the metal, i.e. a redox or oxidation/reduction reaction...
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A sample of calcium nitrate, $Ca(NO_3)_2$, with a formula weight of 164 g/mol, has $5.00 x 10^25$ atoms of oxygen. How many kilograms of $Ca(NO_3)_2$ are present?
Step 1. Calculate the moles of $"O"$ atoms. $"Moles of O" = 5.00 × 10^25 color(red)(cancel(color(black)("atoms O"))) × "1 mol O"/(6.022 × 10^23color(red)(cancel(color(black)("atoms O")))) = "83.03 mol O"$ Step...
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If 5.04 grams of iron (II) nitrate reacts with an excess of $H_2S$, what mass of iron(II) sulfide will be produced in the reaction $Fe(NO_3)_2 + H_2S -> FeS + H(NO_3)$?
$Fe(NO_3)_2(aq) + H_2S(aq) rarr FeS(s)darr + 2HNO_3(aq)$ The stoichiometrically balanced equation tells you explicitly that 1 mol of sulfide will result from every mole of ferrous nitrate. $"Moles of ferrous...
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Assuming an efficiency of 29.40%, how would you calculate the actual yield of magnesium nitrate formed from 123.5 g of magnesium and excess copper(II) nitrate in the equation $Mg + Cu(NO_3)_2 -> Mg(NO_3)_2 + Cu$?
The first thing to do here is to calculate the theoretical yield of the reaction, i.e. what you'd expect to see for a reaction that has a $100%$ yield....
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Consider the reaction: $K_2S_((aq))+Co(NO_3)_(2(aq)) -> 2KNO_(3(aq))+CoS_((s)) darr$. What volume of 0.220M $K_2S$ solution is required to completely react with 160mL of 0.145M $Co(NO_3)_2$?
You need 105 mL of 0.220-M potassium sulfide solution to completely react with that much cobalt nitrate. Start with the balanced chemical equation for this $K_2S_((aq)) + Co(NO_3)_(2(aq))...
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