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Which of the given equations correctly represents the neutralization of magnesium hydroxide by hydrochloric acid?
$"a. "Mg(OH)_2(s)+2HCl(aq) rarr MgCl_2(aq) + 2H_2O(l)$
$"b. "Mg(OH)_2(s)+2HCl(aq) rarr MgO(s) + 2H_2(g) + Cl_2(g)$
$"c. "MgO(s)+2HCl(aq)$
We need a stoichiometric equation that represents the reaction between $Mg(OH)_2$ and $HCl$, and here it is............ $Mg(OH)_2(s) + 2HCl(aq) rarr MgCl_2(aq) + 2H_2O(l)$ Here, $1$ $"equiv"$ of magnesium hydroxide...
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Magnesium reacts with hydrochloric acid according to the following equation: $Mg(s) + 2HCl(aq) -> MgCl_2(aq) +H_2(g)$. What mass of hydrogen will be obtained if 100 $cm^3$ of 2.00 mol $dm^-3$ HCl are added to 4.86 g of magnesium?
So you have the balanced equation, that's a good start. So what we're looking for is the ratio of hydrogen gas produced per the limiting reactant, let's find that first,...
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In the reaction$ Mg (s) + 2HCl (aq) -> H_2 (g) + MgCl_2 (aq)$, how many grams of hydrogen gas will be produced from 125.0 milliliters of a 6.0 M HCI in an excess of Mg?
I am assuming that $6.0 M HCl$ is a typo, and that it should be $6.0 molL^-1 HCl$, since that makes sense in the equation. First we have to find...
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A student investigated the reactions of copper carbonate and copper oxide with dilute hydrochloric acid. How can a sample of copper chloride crystals be made from copper carbonate and dilute hydrochloric acid?
$CuCO_3(s) + 2HCl(aq)rarrCuCl_2(aq) + CO_2(g)uarr + H_2O(l)$ Or........... $CuO(s) + 2HCl(aq)rarrCuCl_2(aq) + H_2O(l)$ For each acid base reaction the product is the beautiful blue-coloured $[Cu(OH_2)_6]^(2+)$ ion, which is commonly represented...
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In the reaction $Mg(s) + 2HCl(aq) -> MgCl_2(aq) + H_2(g)$, what role does magnesium play?
In the chemical equation given to you $"Mg"_ ((s)) + 2"HCl"_ ((aq)) -> "MgCl"_ (2(aq)) + "H"_ (2(g))$ magnesium is a reactant, which is why you see...
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In the equation $Mg(s) + 2HCl(aq) -> MgCL_2(aq) + H_2(g)$, what mass of hydrogen will be obtained if $100$ $cm^3$ of 2.00 mol $dm^-3$ $HCl$ are added to 4.86 g of magnesium?
Moles of metal, $=$ $(4.86*g)/(24.305*g*mol^-1)$ $=$ $0.200$ $mol$. Moles of $HCl$ $=$ $100 *cm^-3xx2.00*mol*dm^-3$ $=$ $0.200$ $mol$ Clearly, the acid is in deficiency ; i.e. it is the , because...
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Zinc oxide reacts with hydrochloric acid to produce zinc chloride and dihydrogen monoxide. If 3.6 moles of zinc oxide reacts with an excess of hydrochloric acid, then how many grams of zinc chloride were produced?
The reaction happening in solution is the following: $ZnO(aq)+2HCl(aq)->ZnCl_2(aq)+H_2O(l)$ Since the hydrochloric acid ($HCl$) is in excess, therefore, the number of moles of Zinc oxide ($ZnO$) will determine the mass...
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In the equation $Mg + 2HCl -> MgCl_2 + H_2$, what volume of hydrogen at STP is produced from the reaction of 50.0 g of $Mg$ and the equivalent of 75 g of $HCl$?
Moles of magnesium: $(50.0*g)/(24.31*g*mol^-1)$ $=$ $2.06$ $mol$ Moles of hydrogen chloride gas: $(75.0*g)/(36.2*g*mol^-1)$ $=$ $2.07$ $mol$ Given equimolar amounts, clearly, the gas is in deficiency as the stoichiometric equation requires...
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How many moles of hydrogen are produced from the reaction of three moles of zinc with an excess of hydrochloric acid in $Zn + 2HCl -> ZnCl_2 + H_2$?
as per given balanced equation one mole Zn produces 1mole Hydrogen when reacted with excess acid. So 3 moles Zn will give 3moles Hydrogen
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What volume of hydrogen at STP is produced when 2.5 g of zinc react with an excess of hydrochloric acid in the reaction $Zn + 2HCl -> ZnCl_2 + H_2$?
$1 "mol"$ of $"Zn"$ has mass of $65.39 "g"$. The amount of $"Zn"$ is $frac{2.5 "g"}{65.39 "g/mol"} = 0.038 "mol"$. The amount of $"H"_2$ produced is the same as the...
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