Question 9 (1 point) Use the following equations to calculate the molar enthalpy of formation for manganese(IV) oxi...

Question

Question

science chemistry

Answer 1

✔ Recommended Answer

Answer #1

reverse and double the first equation

2MnO_(s) + O2_(g) -----------> 2MnO2_(s) $\Delta$ H₁ = -264 kJ / mol

add second equation to above equationj

2MnO_(s) + O2_(g) -----------> 2MnO2_(s) $\Delta$ H₁ = -264 kJ / mol

MnO2_(s) + Mn_(s) ---------> 2MnO_(s) $\Delta$ H₂ = - 240 KJ/mol

---------------------------------------------------------------------------------------

Mn_(s)+ + O2_(g) -----------> MnO2_(s) $\Delta$ H = - 504 KJ/mol

answer = option 2 = - 504 KJ/mol

Answer 2

Similar Homework Help Questions

12) Use the following data to calculate the standard heat (enthalpy) of formation, ???, of manganese(IV)...

12) Use the following data to calculate the standard heat (enthalpy) of formation, ???, of manganese(IV) oxide, MnO2 (s). 2MnO2(s)--2MnO(s) + O2(g) MnO2(s) + Mn(s)- 2Mn0(s) ??-264 kJ ?? -240 kJ 13) Calculate the ??0nn for the following reaction. (Arf [SiO2(s)--910.9 kJ/mol; APf [SiCl4(g)]--657.0 kJ/mol; ??'f [HCI(g)1--92.3 kJ/mol; ? Hof [H2O(g),- -241.8 kJ/mol) SiO2(s) + 4HCI(g)-SiCI(g) + 2H2O(g)
using Hess's law what is the standard enthalpy of formation of manganese(ll)oxide, MnO(s)? 2MnO2(s)-->2MnO(s)+O2(g) rxn= +272.0...

using Hess's law what is the standard enthalpy of formation of manganese(ll)oxide, MnO(s)? 2MnO2(s)-->2MnO(s)+O2(g) rxn= +272.0 kJ/mol MnO2(s)+Mn(s)-->2MnO(s) rxn=-248.9 kJ/mol A. -520.9 kJ/mol B. -396.5 kJ/mol C. -384.9 kJ/mol D. -147.6 kJ/mol E. 24 kJ/mol
* 15.39 x - Question 7 (1 point) Manganese(II) oxide can react with oxygen to form...

* 15.39 x - Question 7 (1 point) Manganese(II) oxide can react with oxygen to form manganeso(IV) oxide as shown below: 2 MnO(s) + O2(g) → 2 MnOz(s) & Hm - Art mg When 15.3 g of the manganese(II) oxide reacted, 26.9 kJ of heat energy was released. What is the molar enthalpy of reaction for the manganese(II) oxide 4. Hm Answer to 3 S.D. in kJ/mol. Make sure that you include a + or - sign with your answer...

problem is together. 3. Calculate the enthalpy of formation of carbon dioxide in the following reaction:...

problem is together. 3. Calculate the enthalpy of formation of carbon dioxide in the following reaction: C(s) + O2(g) - CO, (g) Use the following equations: a) H2O(l) → H2(g) + 2O2(g) AH°-= +285.8 kJ/mol b) C2H6(g) → 2C (s) + 3H2(g) AH'= +84.7 kJ/mol c) 2CO2 (g) +3H2O (1) C2H6(g) + (7/2) O2(g) AH°F = +1560.7 kJ/mol
Using Hess's Law to Calculate a Standard Enthalpy of Formation On the Solution Calorimetry Lab Report...

Using Hess's Law to Calculate a Standard Enthalpy of Formation On the Solution Calorimetry Lab Report Form, vou will be asked to calculate a standard enthalpy of formation for magnesium oxide based on your experimental results. Below is an example of how to do this type of calculation. Calculate the standard enthalpy of formation of gaseous diborane (B2H6) using the following thermochemical equations: 4 B(s) + 3 O2(g)-> 2 B2O3(s) 2 H2(g) + O2(g) > 2 H20(0) B2H6(8) +3 O2(g)...
The normal boiling point of methanol is and the molar enthalpy of vaporization if 71.8 kJ/mol....

The normal boiling point of methanol is and the molar enthalpy of vaporization if 71.8 kJ/mol. The value of S when 1.75 mol of vaporizes at 64.7 °C is 0.372 4.24 × 107 372 1.94 × 103 1.

Question 10 Even in basic solution, MnO, can oxidize water. One product is manganese(IV) oxide. Write...

Question 10 Even in basic solution, MnO, can oxidize water. One product is manganese(IV) oxide. Write a balanced chemical equation for the reaction Mnog (aq) + 6H20(1) - MnO2(5) + 2H2(g) + SOH(aq) 4Mno. (aq) + 2H,0(1) --- 4MnO (5) + 302(g) + 40H (ag) 4Mno. (aq) + H20(1) - 4MnO(s) + O2(g) +2014(aq) 2MnO4 (aq) + 2H20(1) --- 2Mn?"(aq) + 302(g) + 4OH(aq) Mno," (aq) +H:0(1) --- MnO (s) +H3(e) -OH(aq)
5 Determine the standard enthalpy of formation of Fe2O3(s) given the thermochemical equations below. 2Fe(s) +...

5 Determine the standard enthalpy of formation of Fe2O3(s) given the thermochemical equations below. 2Fe(s) + 3/2 O2(g) → Fe2O3(s) AH(Fe2O3) = ? Fe(s) + 3 H2O() Fe(OH)3(s) + 3/2 H2(g) AH° = +160.9 kJ/mol-rxn H2(g) + 1/2O2(g) → H2O(1) A.H° = -285.8 kJ/mol-rxn Fe2O3(s) + 3 H2O(1) ► Fe(OH),(s) A,Hº +288.6 kJ/mol-rxn
Question 5 (1 point) The reaction of aluminum with oxygen is exothermic. The enthalpy of formation...

Question 5 (1 point) The reaction of aluminum with oxygen is exothermic. The enthalpy of formation for aluminum oxide is - 1676 kJ/mol. How much heat will the combustion of 4.50 g of aluminum produce, in kJ? Include the proper sign for an exothermic or endothermic reaction.

Use Hess's law to calculate standard enthalpy change of formation at 298K for carbon (iv) sulphide...

Use Hess's law to calculate standard enthalpy change of formation at 298K for carbon (iv) sulphide compound, Cs2. Given that: Cs2(s) + 3O2(g) - Co2(g) + 2So2(g) ∆H°298= -1113KJ/mol C(s) + O2(g) - Co2(g). ∆H°298 = -407 KJ/mol S(s) + O2(g) - So2(g) ∆H°298 = -298 KJ/mol