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Given that the reaction proceeds quantitatively, whatever the conditions of temperature and pressure, if there were
How much oxygen is required to form
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Oxygen and hydrogen react explosively to form water. In one reaction, 6 g of hydrogen combines with oxygen to form 54 g of water. How much oxygen was used?
I'll show you two approaches to solving this problem, one really short and one relatively long. $color(white)(.)$ SHORT VERSION The problem tells you that $"6 g"$ of hydrogen gas,...
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Elemental sulfur occurs as octatomie molecules, $S_8$. What mass of fluorine gas is needed to react completely with 28.6 g of sulfur to form sulfar hexafluoride?
We need (i) a stoichiometric equation: $S(s) + 3F_2(g) rarr SF_6(g)$. And (ii) the molar equivalence of sulfur and fluorine $=$ $(28.6*g)/(32.06*g*mol^-1)$ $=$ $0.892*mol$. And thus $0.892xx3xx38.00*g*mol^-1$ $~=$ $100*g$...
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If sulfur dioxide and oxygen can be made into sulfur trioxide, what is the reverse reaction?
Vast quantities of $"sulfur trioxide"$ are utilized industrially for sulfuric acid synthesis: $SO_3 + H_2Orightleftharpoons H_2SO_4$
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When propane $C_3H_8$ reacts with oxygen, carbon dioxide and water are produced. If 7.51 grams of propane react with excess oxygen, how many grams of carbon dioxide are formed?
From the equation above, 3 moles of carbon dioxide result from every mole of propane combusted. We had, $(7.51*g)/(44.1*g*mol^-1)$ $=$ $?? "moles of propane"$. So how many moles of...
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Elemental sulfur occurs as octatomic molecules, $S_8$. What mass (g) of fluorine gas is needed to react completely with 17.8 grams of sulfur to form sulfur hexafluoride?
Start with a balanced equation. $"S"_8+"24F"_2$$rarr$$"8SF"_6"$ Then determine the molar masses of $"S"_8"$ and $"F"_2"$ by multiplying the subscript of each element by its from in g/mol. $"S"_8":$ $(8xx32.06 "g/mol")="256.48...
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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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In the formation of carbon dioxide from carbon monoxide and oxygen, how many liters of carbon monoxide, CO, are needed to react completely with 1/2 mole of oxygen gas at STP?
2 CO (g) + O2(g) → 2 CO2 (g)
At constant pressure and temperature, the volume of a gas represents the number of particles. You have given te stoichiometric equation: $2C-=O(g) + O_2(g) rarr 2CO_2(g)$, And this equation...
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Ethene undergoes incomplete combustion to form carbon dioxide, carbon monoxide and water vapour. If the ratio of carbon dioxide to carbon monoxide formed is 9:1 when x cm^3 of ethene is burnt, what is the volume of oxygen gas consumed in the reaction?
Ethene undergoes incomplete combustion to form carbon dioxide, carbon monoxide and water vapour. The balanced equation of this incomplete combustion reaction is as follows. $C_2H_4(g)+5/2O_2(g)->CO_2(g)+CO(g)+2H_2O(g)$ But as per question the...
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