1 Answers
Call
Let us first look at the equation. As per the equation , 2 moles of Magnesium produces two moles of MgO . If we double the amount of Magnesium , it will also double the amount of MgO we will obtain.
2 Moles of Mg produces 2 moles of MgO
4 Moles of Mg will produce X moles of MgO
2 Mole Mg / 4 Mole Mg = 2 moles of MgO/ X moles of MgO
1/ 2 = 2/X
1.X = 2.2
X = 4
0
like
0 dislike
Talk Doctor Online in Bissoy App
100 grams of magnesium and 2.50 grams of oxygen react together in synthesis reaction to form magnesium oxide. How do you write this balanced reaction?
It is abundantly clear that magnesium is in vast molar excess: i.e. $"Moles of metal"$ $=$ $(100*g)/(24.31*g*mol^-1)$ $~=$ $5*mol$ $"Moles of dioxygen"$ $=$ $(2.5*g)/(32.00*g*mol^-1)$ $~=$ $0.08*mol$ Clearly, $O_2$ is the...
1 Answers 1 views
What is the reaction $2Mg(s) + O_2(g) -> 2MgO(s)$ is an example of what type of reaction?
Magnesium metal is oxidized to magnesium ion: $Mg(s) rarr Mg^(2+) + 2e^(-)$ $(i)$ Oxygen gas is reduced to oxide anion: $O_2(g) + 4e^(-) rarr 2O^(2-)$ $(ii)$ Overall $2xx(i) + (ii)$,...
1 Answers 1 views
How many atoms of oxygen are there on each side of the chemical equation $2Mg + O_2 -> 2MgO$?
The expression $2Mg + O_2 -> 2MgO$ Means Two atoms of magnesium, plus one oxygen molecule (consisting of two atoms of oxygen) react to become two particles of magnesium oxide,...
1 Answers 1 views
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...
1 Answers 1 views
17.2 grams $MgO$ are produced according to the following equation: $2Mg + O_2 -> 2MgO$. How many grams of oxygen $O_2$ must have been consumed?
Balanced Equation $"2Mg(s)" + "O"_2("g")$$rarr$$"2MgO(s)"$ You need the molar masses of $"MgO"$ and $"O"_2"$. Molar Masses $"MgO":$$"40.304400 g/mol"$ )%22 $"O"_2:$$"31.9988 g/mol"$ Determine the moles of MgO by dividing the...
1 Answers 1 views
In the reaction $2Mg + O_2 -> 2MgO$, the law of definite proportions states that for every 2 moles of $Mg$ you will need how many moles of $O_2$?
It's in the balanced equation. Each number before a compound corresponds to how many miles you use, and when there is no number you put in a 1. So 2...
1 Answers 1 views
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...
1 Answers 1 views
Consider the following reaction: $2Mg(s) + O_2(g) -> 2MgO(s)$, $DeltaH = -1204kJ$. Is this reaction exothermic or endothermic? How do you calculate the amount of heat transferred when 2.4 grams of Mg(s) reacts at constant pressure?
We has.............. $2Mg(s) + O_2(g) rarr 2MgO(s)$ $DeltaH^@""_"rxn"=-1204*kJ*mol^-1$ $(i)$ To make the arithmetic a bit easier we could write........ $Mg(s) + 1/2O_2(g) rarr MgO(s)$ $DeltaH^@""_"rxn"=-602*kJ*mol^-1$ $(ii)$ I am CLEARLY free...
1 Answers 1 views
Given....$2Mg(s) + O_2(g) rarr 2MgO(s)$ $; DeltaH_"rxn"=-1203*kJ*mol^-1$
What enthalpy is associated with the combustion of FOUR moles of magnesium metal?
$2Mg(s) + O_2(g) rarr 2MgO(s)$ $ DeltaH_"rxn"=-1203*kJ*mol^-1$ Enthalpy terms are written per mole of reaction as written. We combust 4 moles of magnesium metal, and should therefore generate $2xx-1203*kJ=-2406*kJ$. Note...
1 Answers 1 views
What is the reduction half-reaction for $2Mg + O_2 -> 2MgO$?
Start by assigning to all the atoms that take part in the reaction--it's actually a good idea to start with the unbalanced chemical equation $stackrel(color(blue)(0))("Mg")_ ((s)) + stackrel(color(blue)(0))("O") _...
1 Answers 1 views