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What is the mass of $2.30 x 10^24$ formula units of magnesium chloride?
Here we use $N_A$, $"Avogadro's number"$ as our counting number, where $N_A=6.022xx10^23*mol^-1$. $"Avogadro's number"$ of $MgCl_2$ formula units have a mass of $95.21*g$. Alternatively we say the molar mass of...
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Magnesium reacts with titanium(4) chloride to produce magnesium chloride and titanium metal. How do you write a balanced equation for this reaction?
Because the magnesium ion has a +2 charge, the formula for magnesium chloride is $MgCl_2$. To balance the four Cl ions in titanium (IV) chloride, the reaction must produce 2...
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What molar quantity with respect to chloride ions is associated with $1.81xx10^24$ $"magnesium chloride formula units"$?
We (i) calculate the molar quantity of chloride ions....... $(1.81xx10^24*"magnesium chloride units")/(6.022xx10^23*MgCl_2*"units"*mol^-1)=3.0*mol$ And since there are TWO moles of chloride ions per mole of salt.... (ii) we could also calculate...
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How many formula units are in a $17.2*g$ mass of magnesium chloride?
And what does this mean? Well, the mass of $"Avogadro's Number"$, i.e. $6.022xx10^23$ of INDIVIDUAL $MgCl_2$ formula units have a mass of $95.21*g$. And thus is the link between the...
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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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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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Calculate the percentages by mass of magnesium, oxygen and hydrogen in magnesium hydroxide, $Mg(OH)_2$. What is the mass of magnesium in $97.4$ $g$ of $Mg(OH)_2$?
The molar mass of $Mg(OH)_2$ is $58.3$ $gmol^-1$. The formula mass contains one mole of $Mg$ $(24.3$ $gmol^-1)$ and two moles each of $O$ $(16$ $gmol^-1)$ and hydrogen $H$ $(1$...
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What are the empirical formulas for:
calcium chloride,
potassium oxide,
magnesium sulfide,
magnesium chloride,
lithium fluoride,
lithium oxide,
sodium sulfide?
Magnesium, Potassium, Lithium, and Sodium all have an oxidation state of $+1$. Calcium has $+2$. Oxygen and Sulfur have an oxidation state of $-2$. Fluorine and Chlorine have an oxidation...
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If $0.276*mol$ silver chloride was collected from a reaction between silver nitrate and magnesium chloride, how many equiv magnesium nitrate were used?
And how do we know? Well, if we write the stoichiometric equation we have illustrated the : $2AgNO_3(aq) + MgCl_2(aq) rarr Mg(NO_3)_2(aq) + 2AgCl(s)darr$ Alternatively, we could write the net...
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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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