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A magnesium atom reacts to produce a magnesium ion. Which diagram shows a magnesium ion?
a magnesium atom reacts to form magnesium ion losing 2 electrons and thus has a +2 charge and 10 electrons .
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What is the molar mass of magnesium nitride, $"Mg"_3"N"_2$, if the mass of one mole of magnesium is 24.31 g and of one mole of nitrogen is 14.01 g?
The idea here is that you need to use the chemical formula for magnesium nitride, $"Mg"_3"N"_2$, to calculate the mass of one mole of the compound, i.e. its molar mass....
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Why is the first ionization energy of aluminum lower than the first ionization of magnesium?
Electronic configuration of atomic $Mg$: $1s^(2)2s^(2)2p^(6)3s^2$, versus $Al$, $1s^(2)2s^(2)2p^(6)3s^(2)3p^1$. Would you expect it to be easier to remove an electron from a $p$ orbital (with zero electron at the nucleus),...
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The IE of H is 1.31 MJ/mole. If all three electrons in Li were in the 1st shell at a distance equal to that of H, which of the following values would be the better estimate of the first ionization energy of Lithium: 3.6 MJ/mole or 0.6 MJ/mole? Why?
As is often the case with questions such as these, I often find that the best approach begins with a definition. Here, let's consider a typical definition of first ionisation...
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$"a. How many sulfur atoms in a 6 mole quantity of sulfur atoms?"$
$"b. How many sulfur atoms in a 6 mole quantity of"$ $S_8$ $"molecules?"$
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 $"dozens"$: $"1 dozen"="12 items of stuff"$. $a.$ $"6 dozen S atoms"$...
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Magnesium chloride has an atomic mass of 94 amu. What is the mass of one mole of magnesium chloride?
If $1$ particle of $MgCl_2$ has a mass of $"94 amu"$, then $1$ mole of $MgCl_2$ will have a mass of $"94 g"$. It might seem weirdly convenient that...
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How do i calculate the number of moles of magnesium, chlorine, and oxygen atoms in 7.70 moles of magnesium perchlorate, $"Mg"("ClO"_4)_2$. Express the number of moles of Mg, Cl, and O atoms numerically, separated by commas. moles of Mg, Cl, O =?
$1 "mol" " Mg"("ClO"_4)_2$ contains :- $color(red)(1 "mol Mg atoms")$ $color(blue)(2 "mol Cl atoms"$ $color(green)(8 "mol O atoms"$ To find no. of moles of each element,...
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A mixture of magnesium carbonate and magnesium oxide of mass $12.46*g$ underwent fierce heating. After heating, there were $8.43*g$ of salt remaining. What were the masses of magnesium carbonate, and magnesium oxide in the original sample?
$MgCO_3(s)+DeltararrMgO(s) + CO_2(g)$ And we would have to heat the magnesium salt VERY fiercely to get complete decarboxylation. $"Moles of carbon dioxide LOST"$ $=$ $(4.40*g)/(44.01*g*mol^-1)$ $=0.010*mol$ And therefore in...
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For the reaction,$2x$+$3y$+$4z$$ rarr$$ 5w$
Initially if 1 mole of $x$,3 mole of $y$ and 4 mole of $z$ is taken and 1.25 mole of $w$ is obtained then what is the % yield of this reaction?
This is a limiting reactant problem. We know that we will need a balanced equation and moles of each reactant. 1. Gather all the information in one place with...
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Magnesium will burn in oxygen to form magnesium oxide as represented by the following equation
2Mg(s) + O2(g) -> 2MgO(s)
What mass of magnesium will react with 498.1 ml of oxygen at 145.2 degrees Celsius and 0.927 atm?
We use the Ideal Gas Equation to access the molar quantity of dioxygen gas............ $n=(PV)/(RT)=(0.927*atmxx0.4981*L)/(0.0821*(L*atm)/(K*mol)xx418.4*K)=1.34xx10^-2*mol$. Given the stoichiometric equation.......... $Mg(s) + O_2(g) rarr MgO(s)$ There are $1.34xx10^-2*molxx24.31*g*mol^-1=??*g$ metal required for...
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