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If 507 g $FeCl_2$ were used up in the reaction $FeCl_2 + 2NaOH -> Fe(OH)_2(s) + 2NaCl$, how many grams of $Fe(OH)_2$ would be formed?
Just use a little . $507g$ $FeCl_2$ / $126.751 g$ $FeCl_2$ = $4 mol$ $FeCl_2$ $4 mol$ $FeCl_2$ x $1 mol$ $Fe(OH)_2$ = $4 mol$ $Fe(OH)_2$ $4 mol$ $Fe(OH)_2$...
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$Zn(s) + 2HCl(aq) -> H_2 (g) + ZnCl_2(aq) + $heat energy.
If 30.0 g of $Zn$ react, how many grams of $H_2$ will form?
1. Write the balanced equation. $"Zn" + "2HCl" → "ZnCl"_2 + "H"_2$ 2. Calculate the moles of $"Zn"$. $"Moles of Zn" = 30.0 color(red)(cancel(color(black)("g Zn"))) × ("1 mol Zn")/(65.38...
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For the reaction $2HNO_3 + Mg(OH)_2 -> Mg(NO_3)_2 + 2H_2O$, how many grams of magnesium nitrate are produced from 8 moles of water?
We can use to find the moles of $Mg(NO_3)_2$ and then the respective grams of $Mg(NO_3)_2$. If 8 moles of water are produced, we can find out how many moles...
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$H_2(g) + Cl_2(g) rarr 2HCl(g)$
The give reaction occurs at constant pressure...which is the only viable observation?
YOu have been given the chemical equation: $H_2(g) + Cl_2(g) rarr 2HCl(g)$ There are 2 equiv (moles if you like) of gaseous product, and 2 equiv gaseous reactant. Clearly, mass...
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Which equation is unbalanced?
$HCl(aq)+H_2O(l)rarr Cu^(2+) + 2NO_3^-$;
$Ca(OH)_2(s) stackrel(H_2O)rarr Ca^(2+) +2HO^-$;
$Ca(NO_3)_2(s) stackrel(H_2O)rarr Ca^(2+) +2NO_3^-$
;$NH_3(aq) +H_2O(l) rightleftharpoonsNH_4^+ + HO^-$;
$HCl(aq)+H_2O(l)rarr Cu^(2+) + 2NO_3^-$ $Ca(OH)_2(s) stackrel(H_2O)rarr Ca^(2+) +2HO^-$ $Ca(NO_3)_2(s) stackrel(H_2O)rarr Ca^(2+) +2NO_3^-$ $NH_3(aq) +H_2O(l) rightleftharpoonsNH_4^+ + HO^-$ And one of these things is not like the other ones.........
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How does ammonia behave as a Bronsted base:
$"(i) "NH_3(g) + 7/2O_2(g) rarr 2NO_2(g) + 3H_2O$
$"(ii) "2NH_3(g) rarr NH_4^+ +NH_2^(-) $
$"(iii) "NH_3(g) + H_3CBr(g) rarr H_3CBr(g) + HBr(g)$
$"(iv) "NH_3(aq) +H_2O(l) rarr NH_4^+ + HO^-$?
Ammonia is a Bronsted base: $NH_3(aq) + H_2O(l) rightleftharpoons NH_4^+ + OH^-$ $pK_b = 4.75$ I am not going to solve this equation using $pK_b$, but most of the ammonia...
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For which equation, does the enthalpy of reaction represent $DeltaH_f^@$ for methanol?
$1.$ $CO(g) + 2H_2(g) rarr CH_3OH(l)$ $2.$ $C(g) + 2H_2O(g) rarr CH_3OH(l)+1/2H_2(g)$ $3.$ $C(s) + 2H_2(g) +1/2O_2(g) rarr CH_3OH(l)$ $4.$ $C(g) + 2H_2(g) rarr CH_3OH$
The standard of formation is the enthalpy associated with the formation of 1 mole of substance from its constituent in their standard states under specified conditions. And of course...
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Calculate the change in enthalpy $( DeltaH)$ for the chemical reaction modeled by this chemical equation: $H_2 + Cl_2 rarr 2HCl$
Is energy entering or leaving the system? How do you know? What happens to the covalent bonds during this reaction?
And I don't know offhand how they measured the enthalpy change for the reaction, $H_2(g)+Cl_2(g)rarr2HCl(g)+Delta$ but such a measurement could conceivably be done and no doubt has been done....
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Oxygen almost always has an oxidation number of -2. Therefore in the formula for the mineral wüstite, $FeO$, what must the oxidation number for iron be? In the formula for hematite, $Fe_2O_3$, what must the oxidation number for iron be?
In its oxides, an oxidation number of $-II$ is typical. And since, for neutral , the sum of the is $0$. For $"ferrous oxide"$ we have $Fe^(+II)O^(-II)$; and for $"ferric...
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What is the oxidation half reaction for $Fe(s) + 2HCl(aq) -> FeCl_2(aq) + H_2(g)$?
In this reaction Fe is being oxidized and H is being reduced. To check the balance of a redox reaction, make sure that the number of electrons exchanged are equal...
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