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If an average atom of sulfur weighs 32.07 many sulfur atoms are contained in sample with mass 8274 amu? What is the mass of $5.213 x 10^24$ sulfur atoms?
These are just conversions. Set up the equation so that you end up with the UNIT you desire for an answer, and the math will be correct. $(1/32.07)$ (atom/amu) *...
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What is the formal charge on the sulfur atom in sulfur trioxide $SO_3$?
Sulfur assumes a $+VI$ oxidation state in the acid anhydride sulfur trioxide, and of course has the same oxidation state in sulfuric acid. $(O=)S^(2+)(-O^-)_2$ Most chemists would settle for...
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7.0 moles of sulfur atoms and 10 moles of oxygen molecules are combined to form the maximum amount of sulfur trioxide, how many moles of which reactant remain unused at the end of the reaction?
.........And oxygen is in deficiency. Given $10$ $mol$ of dioxygen gas, at most, $6.67$ $mol$ of sulfur trioxide can be generated. This is clearly indicated by the stoichometric equation. Should...
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Solid arsenic reacts with Oxygen gas to synthesize solid arsenic trioxide. How many moles of arsenic trioxide will be produced from 3.4 moles of oxygen gas?
$4As$ + $ 3O_2$ -----> $2As_2O_3$ According to equation $3$ moles of oxygen gas is required to form arsenic trioxide = $2$ moles $3.4$ moles of O2 will be required...
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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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$"a. How many sulfur atoms in a 6 mole quantity of sulfur atoms?"$
$"b. How many sulfur atoms in a 6 mole quantity of"$ $S_8$ $"molecules?"$
is just another number, admittedly it is a very large number, $N_A=6.022xx10^23*mol^-1$. Let's do the problem by using $"dozens"$: $"1 dozen"="12 items of stuff"$. $a.$ $"6 dozen S atoms"$...
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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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What volume of $O_2$ (g) at $350^oC$ and a pressure of 5.25 atm is needed to completely convert 5.00 g of sulfur to sulfur trioxide?
We can combine the given equations........ $S(s) + 3/2O_2(g) rarr SO_3(g)$ And this clearly gives us the mass transfer; 1 equiv of sulfur is oxidized by 3/2 equiv dioxygen gas........
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What volume of $O_2(g)$ at 350. $"^o$C and a pressure of 5.25 atm is needed to completely convert 10.0 g of sulfur to sulfur trioxide?
$"Moles of sulfur"$ $=$ $(10.0*g)/(32.06*g*mol^-1)=0.312*mol$. Given the , we require $3/2xx0.312*mol$ of dioxygen gas, i.e. $0.468*mol$. And now we solve for volume in the Ideal Gas equation: $V=(nRT)/P$ $=$ $(0.468*cancel(mol)xx0.0821*L*cancel(atm)*cancel(K^-1)*cancel(mol^-1)xx623*cancel(K))/(5.25*cancel(atm))$...
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Which sample has the most number of atoms?
$A.$ $"1 mole of oxygen atoms;"$
$B.$ $"1 mole of oxygen molecules;"$
$C.$ $"1 mole of ozone molecules;"$
$D.$ $"Each sample contains the same number of atoms."$
Mass is a measure of the number of particles. Here you have $O$ atoms, and dioxygen, $O_2$, and ozone molecules, $O_3$ but each have the same mass by specification. There...
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