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We cross-mulitply to remove the electrons.
A sheet of aluminum place in copper sulfate solution would rapidly acquire a coppery surface as the copper metal reduced.
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Pure copper may be produced by the reaction of copper(I) sulfide with oxygen gas as follows: $Cu_2S(s) + O_2(g) -> 2Cu(s) + SO_2(g)$. What mass of copper(I) sulfide is required in order to prepare 0.650 kg of copper metal?
You have given the stoichiometric equation that represents reduction of cuprous sulfide: $Cu_2S(s) + O_2(g) rarr 2Cu(s) + SO_2(g)$ Sulfur is oxidized; copper and oxygen are reduced. $"Moles of copper"=(650*g)/(63.55*g*mol^-1)=10.3*mol$....
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How do you balance $Al + CuCl_2 -> AlCl_3 + Cu$?
Aluminum is oxidized to $Al^(3+)$. $Al(s) rarr Al^(3+) + 3e^(-)$ $(i)$ And cupric ion is reduced to zerovalent copper.... $Cu^(2+) + 2e^(-) rarr Cu(s)$ $(ii)$ We cross multiply to remove...
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Sodium chloride reacts with copper sulfate to produce sodium sulfate and copper chloride. $2NaCI (aq) + CuSO_4 (aq) -> Na_2SO_4 (aq) + CuCl_2 (s)$. What type of reaction is this?
Aqueous sodium chloride, $"NaCl"$, will not react with aqueous copper(II) sulfate, $"CuSO"_4$, because the two potential products are soluble in aqueous solution. The chemical equation given to you is...
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How many moles of copper ion are present in a $2.00*g$ mass of $CuCl_2*2H_2O$?
The give quotient is $"mass"/"molar mass"$, and the answer represents the number of moles of $CuCl_2*2H_2O$, of aquated copper chloride.
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Copper will react with sulfur to form a copper sulfide, if 1.500g copper reacts with sulfur to form 1.880g of copper sulfide, what is the empirical formula of the copper sulfide?
The idea here is that you need to use the mass of copper and the mass of the copper sulfide to determine how much sulfur the produced compound contains, then...
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An oxide of copper contains 2.118 g of copper and 0.2666 g of oxygen. Another oxide of copper contains the same mass of copper but 0.5332 g of copper. What are the empirical formulas of the oxides?
The empirical formulas are $"Cu"_2"O"$ and $"CuO"$. Oxide 1 $color(white)(mmmmml)"Cu" +color(white)(m) "O" → "Oxide 1"$ $"Mass/g":color(white)(l) 2.118color(white)(ll) 0.2666$ Our job is to calculate the ratio of the moles of...
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Based on the following equation: $2 Al + 3 CuCl_2 -> 2AlCl_3 + 3 Cu$. lf 10.53 grams of $CuCl_2$ were reacted, how many grams of $AlCl_3$ will be produced?
According to this law a reactant will produce same no of equivalent of product/s as its reacting mass has. here the equivalent mass of $CuCl_2$ = Formula wt /total valency...
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Aluminum metal reacts with a solution of copper (II) nitrate. If you want to produce $5.4 * 10^24$ atoms of copper, how many moles of aluminum metal are needed?
First we should always have a balanced chemical equation for any reaction we are calculating. The balanced chemical equation for the reaction of aluminum metal with a solution of copper...
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How many grams of aluminum are contained in 100.0 g of aluminum chloride, $AlCl_3$?
100.0 g $AlCl_3 (1mol AlCl_3)/(133.34 g)= .74996 mol AlCl_3$ There is 1 mol of Aluminum per one mole of $AlCl_3$ Therefore there is .74996 mols of Al Rounded to correct...
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What volume of 133 mL, 7.90 M $CuCl_2$ solution should you dilute in order to have 51.5 mL of diluted solution that contains 4.49 g $CuCl_2$?
The first thing to do here is to use the and the volume of the initial solution to figure out how many grams of copper(II) chloride it contains....
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