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Sulfide anion is oxidized to sulfur dioxide; dioxygen gas is reduced to oxide anion. This is formally a 6 electron transfer. Is this balanced? How could I remove the non-integral coefficient?
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A $3.6*g$ mass of water was decomposed to give $3.2*g$ dioxygen gas. What mass of dihydrogen gas was evolved?
Mass is conserved in every chemical reaction. So, if I start with 10 g of reactant I must finish with 10 g of product. You started with 3.6 g of...
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A $21.3*g$ mass of $"nitrous oxide"$, $N_2O$, is oxidized by dioxygen gas to $NO_2(g)$. How much dioxygen is required?
$"Moles of"$ $N_2O$ $=$ $(21.3*g)/(44.02*g*mol^-1)=0.483*mol$ And for stoichiometric reaction we need, $0.483*molxx3/2xx32.00*g*mol^-1=??*g$ $"dioxygen gas"$.
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According to the following reaction, how many moles of sulfur trioxide will be formed upon the complete reaction of 0.971 moles of sulfur dioxide with excess oxygen gas? sulfer dioxide (g) + oxygen (g) $->$ sulfer trioxide
We need a stoichiometic equation: $SO_2(g) + 1/2O_2(g) rarr SO_3(g)$ The equation unequivocally tells us that the reaction of $64*g$ $SO_2(g)$ with $16*g$ $O_2(g)$ gives $80*g$ $SO_3(g)$. The given masses...
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Hydrogen sulfide reacts with sulfur dioxide to give H2O and S,
H2S + SO2 = H2O + S(solid), unbalanced.
If 3.0 L of H2S gas at 760 torr produced 4.8 g of sulfur, what is the the temperature in Celsius?
You must convert $"grams of S" → "moles of S" → "moles of H"_2"S"$ and then use the Ideal Gas Law to find the temperature of the $"H"_2"S"$. 1....
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Hydrogen sulfide reacts with sulfur dioxide to give H2O and S,
H2S + SO2 = H2O + S(solid), unbalanced.
If 6.0 L of H2S gas at 750 torr produced 3.2 g of sulfur, what is the temperature in Celsius?
There are four steps in this problem: Write the balanced chemical equation. Calculate the moles of sulfur. Calculate the moles of H₂S. Use the to calculate the temperature....
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A $600*cm^3$ volume of ethane gas is completely combusted with $2500*cm^3$ of dioxygen gas to give carbon dioxide and water. What is the reagent in excess, and what volume would $CO_2(g)$ occupy after the reaction....?
We are given the amounts of two reactants, so this is a limiting reactant problem. We know that we will need a balanced equation with volumes of the involved....
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My textbook says that that for a mixture of $15.2*g$ helium gas, and $30.6*g$ dioxygen gas, the partial pressure is dominated by the helium. Can you find $P_"He"$, and $P_"dioxygen"$ and $P_"Total"$?
$"Dalton's Law of Partial Pressures"$ states UNEQUIVOCALLY that in a gaseous mixture, the partial pressure exerted by a gaseous component is the SAME as it would exert if it ALONE...
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What is the concentration of lead ions and sulfide ions in a saturated solution of lead sulfide ($PbS$) solution at 25°C?
PbS (aq) $<=>$ $ Pb^(2+)$ (aq) + $ S^(2-)$ (aq) $K_(sp)$ = [ $ Pb^(2+)$ (aq) ] . [ $...
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If a reaction of sulfur dioxide with dioxygen gas to form sulfur trioxide starts with $"5 mols SO"_2$ and $"5 mols O"_2$, and $60%$ of the $"SO"_2$ was consumed in the reaction, what is the total mols of gas at equilibrium?
$"8.5 mols of gas"$ Write the reaction: $2"SO"_2(g) + "O"_2(g) -> 2"SO"_3(g)$ For this reaction, you know that the starting mols are: $n_("SO"_2,i) = "5 mols...
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How is $"Mohr's salt"$ oxidized by $"potassium permanganate"$ to give $Fe^(3+)$ and $Mn^(2+)$? How is $"hydrogen peroxide"$ oxidized by the same reagent to give $"dioxygen gas"$?
You used the so-called $"Mohr's salt"$, which is a stable and convenient source of $"Fe(II) salt"$, i.e. $[(NH_4)_2Fe(SO_4)_2]*6H_2O$. We can ignore the ammonium and sulfate shrubbery, and represent the redox...
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