What is the correct overall reaction (combustion of magnesium)? MgO(s) + 2HCl(aq) → MgCl2(aq) + H2O(g)
What is the correct overall reaction (combustion of magnesium)? MgO(s) + 2HCl(aq) → MgCl2(aq) + H2O(g)
Homework Answers
ANs.
The combustion reaction of Mg is
...........(1)
You have given another reaction. So, I guess you need the overall reaction of the combustion reaction and the below reaction.
There is 2MgO on the RHS of the combustion chemical equation.
So, multiply the above reaction with 2. The equation becomes
...........(2)
Write eqn (1) and (2) together.
2MgO is present on the RHS of the first equation and on the LHS of the second equation. So, after adding the equations, 2MgO can be cancelled.
The final overall chemical equation is
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What is the correct overall reaction (combustion of magnesium)?
MgO(s) + 2HCl(aq) → MgCl2(aq) + H2O(g)
What is the correct overall reaction (the combustion of magnesium)? Mg(s) + 2HCl(aq) → MgCl2(aq) +...
What is the correct overall reaction (the combustion of magnesium)? Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g)
Identify the limiting reactant of the reaction: MgO(s) + 2HCl(aq) → MgCl2(aq) + H2O(g) 25.0mL HCL...
Identify the limiting reactant of the reaction: MgO(s) + 2HCl(aq) → MgCl2(aq) + H2O(g) 25.0mL HCL 0.25g MgO
Magnesium chloride hexahydrate (MgCl2·6H2O) can be prepared by the following reaction: MgO(s) + 2HCl(aq) + 5H2O(l)...
Magnesium chloride hexahydrate (MgCl2·6H2O) can be prepared by the following reaction: MgO(s) + 2HCl(aq) + 5H2O(l) ⟶ MgCl2∙6H2O(s) ΔH°rxn = -133 kJ/mol What is the standard molar enthalpy of formation of magnesium chloride hexahydrate in kJ/mol? ΔH°f(MgO)=-602 kJ/mol ΔH°f(HCl)=-167 kJ/mol ΔH°f(H2O)=-286 kJ/mol a) -1444 b) -133 c) -2499
Using the Hess Law and the thermochemical equations below, MgO(s) + + 2HCl(aq) ------> MgCl2(g) ...
Using the Hess Law and the thermochemical equations below, MgO(s) + + 2HCl(aq) ------> MgCl2(g) + H2O(l) ΔHrxn = -111.7 kJ/mol Mg(s) + 2 HCl(aq) ------> MgCl2(g) + H2(g) ΔHrxn = -548.3 kJ/mol H2(g) + 1/2 O2(g) ------> H2O(l) ΔHrxn = -142.9 kJ/mol find the heat of reaction of the following: (0.25 pt.) Mg(s) + 1/2 O2(g) ------> MgO(g) ΔHrxn = ? b) If the theoretical enthalpy of this reaction is -602 kJ/mol,...
Balanced equation : MgO(s)+2HCl(aq)->MgCl2(aq)+H2 H= -151kJ b. How many grams of magnesium oxide are required to...
Balanced equation : MgO(s)+2HCl(aq)->MgCl2(aq)+H2 H=
-151kJ
b. How many grams of magnesium oxide are required to react with excess hydrochloric acid to release 1.4 kJ of heat?
Question 16 In the reaction of magnesium metal with hydrochloric acid: Mg(s) + 2HCl(aq) --> MgCl2(aq)...
Question 16 In the reaction of magnesium metal with hydrochloric acid: Mg(s) + 2HCl(aq) --> MgCl2(aq) + H2(g) How many moles of hydrogen are produced if 10 moles of HCI react?
a) Using the Hess Law and the thermochemical equations below, MgO(s) + + 2HCl(aq) ------>...
a) Using the Hess Law and the thermochemical equations below, MgO(s) + + 2HCl(aq) ------> MgCl2(g) + H2O(l) ΔHrxn = -111.7 kJ/mol Mg(s) + 2 HCl(aq) ------> MgCl2(g) + H2(g) ΔHrxn = -548.3 kJ/mol H2(g) + 1/2 O2(g) ------> H2O(l) ΔHrxn = -142.9 kJ/mol find the heat of reaction of the following: Mg(s) + 1/2 O2(g) ------> MgO(g) ΔHrxn = ? b) If the theoretical enthalpy of this reaction is -602 kJ/mol, calculate the percent error
The average ΔHrxn for MgO (s) + 2 HCl (aq) --> MgCl2(aq) + H2O (l) is...
The average ΔHrxn for MgO (s) + 2 HCl (aq) --> MgCl2(aq) + H2O (l) is -150. kJ/mol What would be the ΔHrxn for the following reaction: MgCl2(aq) + H2O (l) --> MgO (s) + 2HCl (aq) Group of answer choices +300. kJ/mol -150. kJ/mol +150. kJ/mol +75.0 kJ/mol 2. The average ΔHrxn for Mg (s) + 2 HCl (aq) --> MgCl2(aq) + H2(g) is -466 kJ/mol What would be the ΔHrxnfor the following reaction: 2 MgCl2(aq) + 2 H2(g)...
In the reaction of magnesium metal with hydrochloric acid: Mg(s) + 2HCl(aq) --> MgCl2(aq) + H2(g)...
In the reaction of magnesium metal with hydrochloric acid: Mg(s) + 2HCl(aq) --> MgCl2(aq) + H2(g) What evidence of reaction would you see based on this balanced reaction? The solution cools down Solid formation Bubbles form in solution A color change In the lab, a student measures a teaspoon of an unknown liquid. The teaspoon of liquid has a mass of 6.84 g and a volume of 4.48 ml. How many teaspoons would be in 1.77 kg of this unknown...
Specific heat = 4.18 J/g*C MgO(s) + 2HCl(aq) → 2Cl(aq) + Mg(aq) + H2O(l): AH = A student added 0.250 g of Mg...
Specific heat = 4.18 J/g*C
MgO(s) + 2HCl(aq) → 2Cl(aq) + Mg(aq) + H2O(l): AH = A student added 0.250 g of MgO(s) to 45.0 mL HCI@ 22.0'C. The temp of the calorimeter rose to 23.5°C. What is qarin kJ? What is the AH in kJ/mol of Mgo for this reaction? Density HCI = 1.05 g/mL
Balanced equation : MgO(s)+2HCl(aq)->MgCl2(aq)+H2 H=
-151kJ
b. How many grams of magnesium oxide are required to react with excess hydrochloric acid to release 1.4 kJ of heat?
Question 16 In the reaction of magnesium metal with hydrochloric acid: Mg(s) + 2HCl(aq) --> MgCl2(aq) + H2(g) How many moles of hydrogen are produced if 10 moles of HCI react?
In the reaction of magnesium metal with hydrochloric acid: Mg(s) + 2HCl(aq) --> MgCl2(aq) + H2(g) What evidence of reaction would you see based on this balanced reaction? The solution cools down Solid formation Bubbles form in solution A color change In the lab, a student measures a teaspoon of an unknown liquid. The teaspoon of liquid has a mass of 6.84 g and a volume of 4.48 ml. How many teaspoons would be in 1.77 kg of this unknown...
Specific heat = 4.18 J/g*C
MgO(s) + 2HCl(aq) → 2Cl(aq) + Mg(aq) + H2O(l): AH = A student added 0.250 g of MgO(s) to 45.0 mL HCI@ 22.0'C. The temp of the calorimeter rose to 23.5°C. What is qarin kJ? What is the AH in kJ/mol of Mgo for this reaction? Density HCI = 1.05 g/mL
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