Enthalpy Changes of Reactions

The following equations show the oxidation of carbon and carbon monoxide to carbon dioxide. C(s) +O2(g) → CO2(g) ΔH = –x kJ mol–1 CO(g) + O2(g) → CO2(g) ΔH = –y kJ mol–1 What is the enthalpy change, in kJ mol–1, for the oxidation of carbon to carbon monoxide? C(s) + O2(g) → CO(g)

• x + y

• -x - y

• y - x

• x - y

Tags

NGSS.HS-PS1-4

ΔH means:

• temperature

• calorimetry

• enthalpy

• syntropy

A positive ΔH means that:

• In order for the reaction to happen, heat must be input. It is exothermic

• In order for the reaction to happen, heat must be input. It is endothermic.

• When the reaction happens, heat is released. It is exothermic

• When the reaction happens, heat is released. It is endothermic

Tags

NGSS.HS-PS3-1

Calculate ΔH when 2 moles of ethanol (C₂H₅OH) reacts with excess oxygen according to the following thermochemical equation?

• -2733.4 kJ

• -683.35 kJ

• -1366.7 kJ

• -910.67 kJ

Tags

NGSS.HS-PS1-4

NGSS.HS-PS3-1

The enthalpy change for the reaction C(s, graphite) + 1⁄2O₂(g) --> CO(g) cannot be measured directly since some carbon dioxide is always formed in the reaction. It can be calculated using Hess’s Law and the enthalpy changes of combustion of graphite and of carbon monoxide. C(s, graphite) + O₂(g) --> CO₂ ΔH=-394 kJmol^–1 CO(g) + 1⁄2O₂(g) --> CO₂ ΔH=-283 kJmol^–1 The enthalpy change for the reaction of graphite with oxygen to give carbon monoxide is

• -677 kJmol^–1

• +111 kJmol^–1

• -111 kJmol^–1

• +677 kJmol^–1

The enthalpies of combustion of C(s), H2(g) and C4H9OH(l) (in kJmol^-1) are as follows  
C(s) + O₂(g)   ->  CO₂(g)                                               ∆H=a
H₂(g) + ½O₂(g)   ->   H₂O(l)                                        ∆H=b
C₄H₉OH(l) + 6O₂(g)   ->   4CO₂(g) + 5H₂O(l)  ∆H=c
What is the enthalpy change for the reaction shown below?
  4C(g) + 5H₂(l) + ½O₂(g)   ->   C₄H₉OH(l)

• c – 4a – 5b

• 2a + 10b - c

• 4a + 5b - c

• 2a + 5b + c

Tags

NGSS.HS-PS1-4

The standard enthalpy changes of combustion of carbon, hydrogen and methane are shown in the table. Which one of the following expressions gives the correct value for the standard enthalpy change of formation of methane in kJ mol^–1? C(s) + 2H₂(g) → CH₄(g)

• 394 + (2 × 286) – 891

• –394 – (2 × 286) + 891

• 394 + 286 – 891

• –394 – 286 + 891

Tags

NGSS.HS-PS1-4

Given the following data: ΔH^○_f[FeO(s)] = –270kJmol^–1
ΔH^○_f [Fe₂O₃(s)] = –820 kJ mol^–1
S elect the expression which gives the enthalpy change, in kJ mol^–1, for the reaction:
2FeO(s) + 1⁄2O₂(g) → Fe₂O₃(s) 

• (–820 × 1⁄2) + 270 = –140

• (+820 × 1⁄2) – 270 = +140

• –820 + (270 × 2) = –280 

• +820 – (270 × 2) = +280 

Tags

NGSS.HS-PS3-1

What is the capital of France?

• Paris

• London

• Berlin

• Madrid

C₂H₄(g) + H₂(g)   ->   C₂H₆(g)  ∆H°=-137 kJ mol^-1
Which statement about this information is correct?

• The total energy of the bonds broken in the reactants is greater 
  than the total energy of the bonds 
  formed in the product 

• The bonds broken and the bonds made are of the same strength 

• The total energy of the bonds broken in the reactants is less than the total energy of the bonds formed in the product 

• No conclusion can be made about the sums of the bond enthalpies in the product compared with the reactants 

Tags

NGSS.HS-PS1-4