1 Answers
Call
So we have a molecule of sulfuric acid, which we represent as
0
like
0 dislike
Talk Doctor Online in Bissoy App
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) *...
1 Answers 1 views
$H_2SO_4$ can ionize to yield two $H^+$ ions an and one $SO_4^-2$ ion. What is $H_2SO_4 considered?
Sulfuric acid donates 2 equiv of $H_3O^+$ to aqueous solution. $H_2SO_4 + H_2O rarr HSO_4^(-) + H_3O^+$ $HSO_4^(-) + H_2O rarr SO_4^(2-) + H_3O^+$ The first equilibrium lies almost quantitatively...
1 Answers 1 views
You are given quantities of aluminum sulfate, $Al_2(SO_4)_3$, and sulfuric acid, $H_2SO_4$. If there are EQUAL numbers of SULFUR atoms with respect to each salt, what is the ratio of oxygen atoms...$Al_2(SO_4)_3:H_2SO_4$?
It is given that both salts contain the same number of sulfur atoms. Thus we have $Al_2S_3O_12$, and necessarily $3$ $xx$ $H_2SO_4$. There are $3$ $"equiv"$ sulfuric acid per equiv...
1 Answers 1 views
In the combustion of hydrogen gas, hydrogen reacts with oxygen from the air to form water vapor. Hydrogen + Oxygen $->$ water. If you burn 58.1 g of hydrogen and produce 519 g of water how much oxygen reacted?
The stoichiometrically balanced equation tells us unequivocally that $1$ $mol$ dihydrogen reacts with $0.50$ $mol$ dioxygen to give $1$ $mol$ water. $"Moles of dihydrogen"$ $=$ $(58.1*g)/(2.02*g*mol)$ $=$ $28.7*mol$ $H_2$ $"Moles...
1 Answers 1 views
How many moles of ammonium sulfate can be made from the 30.0 reaction of mol of $NH_3$ with $H_2SO_4$ according to $2NH_3 + H_2SO_4 -> (NH_4)_2SO_4$?
as per balanced equation we know 2moles ammonia produces 1 mole ammonium sulfate . hence 30 moles will produce 15 moles
1 Answers 1 views
How many moles of $H_2SO_4$ are present in half a liter of a 0.150 M $H_2SO_4$ solution?
$"Molarity"="Moles of solute"/"Volume of solution"$ And thus, $"Moles of solute"="Volume of solution"xx"molarity"$ $=0.5*Lxx0.150*mol*L^-1=0.075*mol$ with respect to $H_2SO_4$. Of course, we speak of a formal concentration. We know that in aqueous...
1 Answers 1 views
$"a. How many sulfur atoms in a 6 mole quantity of sulfur atoms?"$
$"b. How many sulfur atoms in a 6 mole quantity of"$ $S_8$ $"molecules?"$
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 $"dozens"$: $"1 dozen"="12 items of stuff"$. $a.$ $"6 dozen S atoms"$...
1 Answers 1 views
The atomic number of sulfur is 16. Sulfur combines with hydrogen by covalent bonding to form a compound, hydrogen sulfide. Based on the number of valence electrons in a sulfur atom, how do you predict the molecular formula of the compound?
We thus predict that hydrogen sulfide would have a formula of $H_2S$, an analogue of the popular $H_2O$ molecule.
1 Answers 1 views
The ratio of carbon atoms to hydrogen atoms to oxygen atoms in a molecule of dicyclohexyl maleate is 4 to 6 to 1. What is its molecular formula if its molar mass is 280 g?
We have been given an empirical formula of $C_4H_6O$. We know that the molecular formula is always a whole number multiple of the empirical formula. Thus ${4xx12.01+6xx1.01+16.0}xxn=280*g*mol^-1$. My arithmetic gives...
1 Answers 1 views
When 7.25 g of $Al$ reacts with excess $H_2SO_4$ in the reaction $2Al (s) + 3 H_2SO_4 (aq) -> Al_2(SO_4)_3(aq) + 3H_2(g)$ how many liters of $H_2$ is formed at 25° C and a pressure of 1.650 atm?
$2$ $Al(s)$ + $3$ $H_2SO_4(aq) to $ $Al_2(SO_4)_3(aq)$ + $3$ $H_2(g)$ First calculate the number of moles of $Al$ in $7.25$ $g$, knowing the molar mass of $Al$ is $27$...
1 Answers 1 views