Question bank: Thermochemistry: Enthalpy

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Question 1:

Medium

A researcher conducts an experiment in a laboratory, investigating the production of ammonia (NH3) from nitrogen (N2) and hydrogen (H2). To carry out this synthesis, he uses the following chemical reaction: N2(g) + 3H2(g) → 2NH3(g), known as the Haber-Bosch Reaction. Knowing that the enthalpy of formation of ammonia is -46.1 kJ/mol and the enthalpies of formation of hydrogen and nitrogen are 0 kJ/mol, as they are substances in the standard state:

Thermochemistry: Enthalpy

Question 2:

Medium

Thermochemistry: Enthalpy

Question 3:

Easy

Thermochemistry: Enthalpy

Theorical Question

Contextualized Question

Question 4:

Very Easy

During a practical Chemistry class, a group of students burned a small sample of magnesium in the laboratory. The observed chemical reaction was: Mg(s) + 1/2 O2(g) -> MgO(s). It is known that the enthalpy change for the formation of magnesium oxide is -601.6 kJ/mol. Considering that the reaction occurred at constant pressure, the students must determine the enthalpy change of the complete reaction. Based on this data, answer: 1) What is the enthalpy change of the overall reaction, considering that the reaction occurred at constant pressure? 2) Classify the type of reaction regarding the release or absorption of energy (exothermic or endothermic).

Thermochemistry: Enthalpy

Theorical Question

Contextualized Question

Question 5:

Medium

Thermochemistry: Enthalpy

IARA TIP

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