WorksheetsSK025 CHAPTER 2:THERMOCHEMISTRY
Total questions: 10
Worksheet time: 20mins
Which of equation example for the definition:
"The heat release when 1 mol of substance is burned completely in excess oxygen"
C(s) + 2H2(g) → CH4(g)
HCl(aq) + NaOH(aq) → NaCl (aq) + H2O(l)
C2H6(l) + 7/2 O2(g) → 2CO2(g) + 3H2O(l)
Cl-(g) → Cl-(aq)
Based on this equation, enthalpy of neutralization must be 1 mol of:
HCl(aq) + KOH(aq) → KCl (aq) + H2O(l)
HCl(aq)
KOH(aq)
KCl(aq)
H2O(l)
Enthalpy combustion:
"The heat release when 1 mol of ____________ is burned completely in excess oxygen"
compound
element
substance
water
Which of the following equation not the enthalpy of atomisation:
1/2Br2(l) → Br(g)
Al(l) → Al(g)
1/2Cl2(g) → Cl(g)
Mg(s) → Mg(g)
Given the enthalpy of formation NO2(g)
1/2N2(g) + O2(g) → NO2(g) ΔH = +33.0 kJ
Calculate enthalpy of combustion, N2(g)
ΔH = +16.5 kJ/mol
ΔH = +33.0 kJ/mol
ΔH = -33.18 kJ/mol
ΔH = +66.0 kJ/mol
Define enthalpy solution:
the heat absorbed when 1 mole of gaseous atoms is formed from its element
the heat released when 1 mole of gaseous ions is hydrated in water
the heat change when 1 mole of a substance is dissolves in excess water to form a very dilute solution
the heat change when 1 mole of a compound is formed from its elements
Which of the equation correct refer to definition of formation, CH3OH (g)
CH3(g) + OH(g) ----> CH3OH (g)
C(s) + H2(g) + OH2(g) ----> CH3OH (g)
C(s) + 2H2(g) + 1/2O2(g) ----> CH3OH (g)
C(s) + H4(g) + O(g) ----> CH3OH (g)
Which of the equation not the enthalpy of formation:
Na(s) + 1/2Br2(l) --------> NaBr(s)
2Na(s) + O2(g) --------> Na2O(s)
Al(s) + 3/2Cl2(g) --------> AlCl3(s)
Mg(s) + 1/2Cl2(g) --------> MgCl2(s)
Lattice energy :
Energy released when 1 mole of solid ionic compound formed from its gaseous ions.
Which of the equation refer for this definition.
Na(s) + 1/2 Cl2(g) --------> NaCl (s)
Na+(g) + Cl-(g) ---------> NaCl (s)
NaCl (s) ----------> Na+(g) + Cl-(g)
Na+(aq) + Cl-(aq) ---------> Na+Cl- (s)
Which of the pair FALSE about their definition of enthalpy:
Enthalpy of atomisation: 1 mol gaseous atom
Enthalpy of formation: 1 mol of a substance
Enthalpy of solution: 1 mol of a substance
Enthalpy of hydration: 1 mol gaseous ion
Enthalpy of combustion: 1 mol of substance
