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
Homework Answers
Add Answer to:
a) Using the Hess Law and the thermochemical equations
below,
MgO(s)
+ + 2HCl(aq) ------>...
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,...
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)...
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
(6 pts.) Using Hess’s Law and the values for Standard Enthalpies of Formation from the table...
(6 pts.) Using Hess’s Law and the values for Standard Enthalpies of Formation from the table provided, calculate the enthalpy of reaction ΔH°rxn (in kJ) for each of the following reactions: Standard Enthalpies of Formation substance ΔHf° in kJ/mol Mg(s) 0 MgO(s) -601.6 HCl(aq) -167.2 MgCl2(aq) -801.2 H2(g) 0 H2O(l) -285.8 Reaction #1: Mg (s) + 2HCl (aq) è MgCl2 (aq) + H2 (g) Reaction #2: MgO (s) + 2HCl (aq) è MgCl2 (aq) + H2O (l) 2. (4 pts.)...
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
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
Part 11: Calculating the enthalpy of formation of MgO(s) Fill in the missing value (4) Ha(g)...
Part 11: Calculating the enthalpy of formation of MgO(s) Fill in the missing value (4) Ha(g) + 1/2O2(g) → H2O(1) AH = -286 kJ/mol (5) Mg(s) + 2 HCl(aq) → MgCl(aq) + Halg) Hºex (5)= -554 kJ/mol (6) MgO(s) + 2 HCl(aq) → MgCl(aq) + H2O(1) Hev(6) = -193 kJ/mol Calculate AHx(7) for the goal reaction: Mg(s) + 1/2 0.(g) → MgO(s) and show your work. AH'expe() = kJ/mol Calculate the percent error in your calculated value for the above...
which if the following equations balanzed? select all that apply. Mg(s)+2HCl(aq) --> MgCl2 (aq) +H2 (g) 3Al(s) + 3Br...
which if the following equations balanzed? select all that apply. Mg(s)+2HCl(aq) --> MgCl2 (aq) +H2 (g) 3Al(s) + 3Br2(I) --> Al2Br3 (s) 2HgO(s) --> 2Hg(I) + O2 (g) N2+O2--> 2NO 2H2O2 --> 2 H2 +O2
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)
Applying Hess’s Law, from the enthalpies of reactions, 2NaCl(s) + H2O(l) --> 2HCl(g) + Na2O(s) ΔH...
Applying Hess’s Law, from the enthalpies of reactions, 2NaCl(s) + H2O(l) --> 2HCl(g) + Na2O(s) ΔH = + 507.31 kJ NO(g) + NO2(g) + Na2O(s) --> 2NaNO2(s) ΔH = − 427.14 kJ NO(g) + NO2(g) --> N2O(g) + O2(g) ΔH = − 42.68 kJ 2HNO2(l) --> N2O(g) + O2(g) + H2O(l) ΔH = + 34.35 kJ Calculate the enthalpy change (ΔHrxn) for the reaction: HCl(g) + NaNO2(s) --> HNO2(l) + NaCl(s) (You should show work to get credit) 5-Magnesium burns...
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
Part 11: Calculating the enthalpy of formation of MgO(s) Fill in the missing value (4) Ha(g) + 1/2O2(g) → H2O(1) AH = -286 kJ/mol (5) Mg(s) + 2 HCl(aq) → MgCl(aq) + Halg) Hºex (5)= -554 kJ/mol (6) MgO(s) + 2 HCl(aq) → MgCl(aq) + H2O(1) Hev(6) = -193 kJ/mol Calculate AHx(7) for the goal reaction: Mg(s) + 1/2 0.(g) → MgO(s) and show your work. AH'expe() = kJ/mol Calculate the percent error in your calculated value for the above...
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