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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...
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2Al+Zn(NO3)2=2Al(NO3)3+Zn net ionic equation?
The equation given above is wrongly balanced, so I have to correct it first. $Al^@$ + $Zn(NO_3)_2$ = $Al(NO_3)_3$ + $Zn^@$ (unbalanced) Tallying the atoms based on subscripts, left side:...
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Aluminum will react with sulfuric acid in the following reaction: $2Al(s) + 3H_2SO_4(l) -> Al_2(SO_4)_3(aq) + 3H_2(g)$. How many moles of $H_2SO_4$ will react with 18 mol Al? How many moles of each product will be produced?
With reference to the given balanced equation for the , the needed number of moles for each remaining compound involved in the reaction using the mass of $Al$ as basis...
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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 $27$...
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What is the mass of copper produced if 4.87 g of $Al$ reacts with copper sulfate in the reaction $2Al + 3CuSO_4 -> Al_2(SO_4)_3 + 3Cu$?
$2Al + 3CuSO_4 rarr Al_2(SO_4)_3 + 3Cu$ $"Moles of aluminum " =(4.87*g)/(26.98*g*mol^-1)$ $=$ $0.181$ $mol$ From the equation, we know that $3$ moles of copper are reduced per $2$ mol...
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How many formula units of aluminum are required to produce 9.9 grams of hydrogen in $2Al + 3H_2SO_4 -> Al_2(SO_4)_3 + 3H_2$?
Given the stoichiometric equation, you have established the . $"Moles of dihydrogen"$ $=$ $(9.9*g)/(2.0*g*mol^-1)$ $=$ $??*mol$. The moles of aluminum metal is $2/3$ this quantity. And of course $"1...
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In the reaction $Al_2(SO_4)_3 + 6NaOH -> 2Al(OH)_3 + 3Na_2(SO_4)_3$, how many moles of $Al(OH)_3$ can be made with 2.3 moles of $NaOH$ and excess $Al_2(SO_4)3$?
Since aluminium sulphate is in excess, it implies that sodium hydroxide is the limiting reactant and decides how much product is formed as it gets used up first. The balanced...
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Using the balanced equation $3Ba + Al2(SO_4)_3 -> 2Al + 3BaSO_4$, if 4g Ba react with 0.45 g $Al_2(SO_4)_3$, what is the excess reactant?
Balanced Equation $"3Ba + Al"_2"(SO"_4)_3"$$rarr$$"2Al + 3BaSO"_4$ The coefficients are the moles of each substance, and they can be used as molar ratios between two of the substances. No coefficient...
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In the equation, $2Al + 2Fe^(3+) + 3O^(2-) -> 2Fe + 2Al^(3+) + 3O^(2-)$m which element has been reduced?
Reduction involves a formal GAIN of electrons. Oxidation involves a loss of electrons. In the reaction above, clearly ferric ion, $Fe^(3+)$, has been REDUCED. The correct reaction is: $Al +...
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Given the equation: $2Al + 3Cu_2 ->2Al^(3+) + 3Cu$. What is the reduction half-reaction?
And the oxidation reaction......... $Al(s) rarr Al^(3+) + 3e^-$ And cross-multiplying to remove the electrons......... $2Al(s) + 3Cu^(2+) rarr 2Al^(3+) + 2Cu(s)$ Is charge balanced? Is mass balanced?
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