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The atomic weight of aluminum is 26.982 u, how many aluminum atoms are there in a 4.55g sample of aluminum?
The key to this problem is the correct interpretation of what atomic weight means. Notice that aluminium is said to have an of $"26.982 u"$. The unit used here...
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How many chloride ions would combine with an $Al^(3+)$ ion to form aluminum chloride?
Al has a charge of +3. Cl has a charge of -1. Hence 3 chloride ions are required to neutralize charge of +3 on aluminium and the compound formed is...
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How do you write "Iron (III) chloride plus aluminum yields aluminum chloride and iron" in a chemical equation?
You don't need to note charges in the equation, if that's what you meant. The charge is implied because of the three Chlorides. Hope this helps!
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How many aluminum-based electrons are present in a salt where there is an $81*g$ mass of aluminum ions....?
Well, we take the quotient, $(81*g)/(27*g*mol^-1)=3*mol$. And thus there are $3 *mol$ of aluminum ions, and since there are 10 electrons per $Al^(3+)$ ions (for $Al, Z=13)$, there are $30*mol$...
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Aluminum oxide is decomposed to extract pure aluminum from the mineral. If 6.7 tons of aluminum oxide is mined, calculate the mass of pure aluminum produced?
1 mole of aluminum oxide has a molecular weight of 102 grams (Al=27 grams and O=16 grams). It means that for 1000 kg of compound you can get 529 kilograms...
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Aluminum reacts with excess hydrochloric acid to form aqueous aluminum chloride and 46.5 mL of hydrogen gas over water at 27 degrees Celsius and 751 mmHg. How many grams of aluminum reacted? The partial pressure of water at 27 C is 26.8 mmHg.
We're asked to find the number of grams of $"Al"$ that reacted, given some $"H"_2 (g)$ product characteristics. Let's first write the chemical equation for this reaction: $2"Al"(s) +...
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What is the theoretical yield of aluminum oxide if 1.60 mol of aluminum metal is exposed to 1.50 mol of oxygen?
First, write the balanced chemical reaction. Then, see how many of the available moles of each reactant will be used. The theoretical yield is the value at which one of...
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Aluminum reacts with aqueous $HBr$ to produce hydrogen gas and aluminum bromide. How many mL of hydrogen gas are produced at 1.03 atm and 20.00 $"^o$C when 0.498 g of aluminum react with an excess of $HBr$?
Each equiv of metal reduces $3$ equiv of acid, and $3/2$ equiv of dihydrogen gas are evolved. $"Moles of aluminum"$ $=$ $(0.498*g)/(26.98*g*mol^-1)=0.0185*mol$. Now, given the conditions, clearly the metal is...
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Given a $1*L$ volume of solution that is $1.25*mol*L^-1$ with respect to $MgCl_2$, there are...?
$"a. 2 moles of ions in solution."$
$"b. 1.25 moles of ions in solution."$
$"c. 2.5 moles of ions in solution."$
$"d. 2 moles of ions in solution."$
The $"mole"$, $N_A$, is simply a number. Admittedly, it is a very large number, $N_A=6.022xx10^23*mol^-1$. And if you have a mole of stuff, you have $6.022xx10^23$ INDIVIDUAL ITEMS of that...
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Which solution contains the biggest amount, in mol, of chloride ions?
A. 20 cm3 of 0.50 mol dm−3 NH4Cl
B. 60 cm3 of 0.20 mol dm−3 MgCl2
C. 70 cm3 of 0.30 mol dm−3 NaCl
D. 100 cm3 of 0.30 mol dm−3 ClCH2COOH
And to answer the question, we must calculate the of of each solution with respect to chloride ions. And $"number of moles"="concentration"xx"volume"$ For $(a):$ there are $0.020*dm^3xx0.50*mol*dm^-3=0.01*mol$. For $(b):$ $0.060*dm^3xx0.20*mol*dm^-3xx"2...
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