Thermodynamics Test

Result

Thermodynamics Test - 7

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Question 1
1 / -0

During complete combustion of one mole of butane, 2658 kJ of heat is released. The thermochemical reaction for above change is

A
C₄H₁₀(g) + O₂(g) → 4CO₂(g) + 5H₂O(l) Δ _cH = +2658.0 kJ mol⁻¹

B
2C₄H₁₀(g) + 13O₂(g) → 8CO₂(g) + 10H₂O(l) Δ _cH = −2658.0 kJ mol⁻¹

C
C₄H₁₀(g) + O₂(g) → 4CO₂(g) + 5H₂O(l) Δ _cH = −1329.0 kJ mol⁻¹

D
C₄H₁₀(g) + O₂(g) → 4CO₂(g) + 5H₂O(l) Δ _cH = −2658.0 kJmol⁻¹

Solution

Enthapy of combustion is the energy released when 1mole of a hydrocarbon (butane ) reacts completely in presence of excess of oxygen. The chemical equation for exothermic reaction for combustion of one mole of butane is represented as;

2C₄H₁₀(g) + 13O₂(g) → 8CO₂(g) + 10H₂O(l) Δ _cH = −2658.0 kJ mol⁻¹
Question 2
1 / -0

Enthalpy of sublimation of a substance is equal to

A
enthalpy of fusion

B
enthalpy of vapourisation

C
enthalpy of fusion + enthalpy of vapourisation

D
twice the enthalpy of vapourisation

Solution

The process of sublimation involves the change of solid into vapour. Though in sublimation a solid does not pass through the liquid phase on its way to the gas phase, the enthalpy change is equal to the sum of enthalpy of fusion and enthalpy of vaporization because enthalpy is a state function.