PracticeVideosBlogFlashcardsEspañol
All Practice Exams

100+ Free Sachsen-Anhalt Abitur Chemistry Practice Questions

Saxony-Anhalt Abitur Chemistry (Chemie) practice questions are available now; exam metadata is being verified.

✓ No registration✓ No credit card✓ No hidden fees✓ Start practicing immediately
100+ Questions
100% Free

Loading practice questions...

Same family resources

Explore More Saxony-Anhalt Abitur

Continue into nearby exams from the same family. Each card keeps practice questions, study guides, flashcards, videos, and articles in one place.

Saxony-Anhalt Abitur Ancient Greek (Griechisch)

Practice Questions

Saxony-Anhalt Abitur Biology (Biologie)

Practice Questions

Saxony-Anhalt Abitur Business and Economics (Betriebs- und Volkswirtschaftslehre)

Practice Questions

Saxony-Anhalt Abitur Engineering Sciences (Ingenieurswissenschaften)

Practice Questions

Saxony-Anhalt Abitur English (Englisch)

Practice Questions

Saxony-Anhalt Abitur French (Französisch)

Practice Questions
2026 Statistics

Key Facts: Sachsen-Anhalt Abitur Chemistry Exam

5 Kompetenzschwerpunkte

The Qualifikationsphase Chemie is organised into five Kompetenzschwerpunkte: Energetik, chemisches Gleichgewicht, Säure-Base, Redox/Elektrochemie and organische Chemie

Fachlehrplan Chemie Gymnasium Sachsen-Anhalt, Stand 01.08.2022

300 / 210 min

Written Bearbeitungszeit at erhöhtem and grundlegendem Anforderungsniveau, plus roughly 30 minutes Auswahlzeit; re-issued annually

RdErl. 'Vorbereitung und Durchführung der Abiturprüfung', Nummer 7.4

24.04.2026

Written Chemie date in the 2026 main session (Nachtermin 21.05.2026); mündliche Prüfungen from 11 May 2026

Ministerium für Bildung des Landes Sachsen-Anhalt, Pressemitteilung 27/2026 (10.04.2026)

0–15 Punkte

Grading scale for each Prüfungsfach, from Note 1 (15–13 Punkte) to Note 6 (0 Punkte)

Verordnung über die gymnasiale Oberstufe, Sachsen-Anhalt

200 / 100 Punkte

Minimum Gesamtqualifikation: 200+ from Block I (§38) and 100+ from the five Prüfungselemente in Block II (§39), out of 900 maximum

Verordnung über die gymnasiale Oberstufe, Sachsen-Anhalt

~5,600 candidates

Approximate number of Abitur candidates in Sachsen-Anhalt in the 2026 session across all eligible school types

Ministerium für Bildung des Landes Sachsen-Anhalt, Pressemitteilung 27/2026

Free 100-question English-language MCQ study bank for Sachsen-Anhalt Abitur Chemie, mapped to the five Qualifikationsphase Kompetenzschwerpunkte with over 40 genuine worked calculations. Official exam: German written Klausur with calculations and data interpretation, 300 min (eA) / 210 min (gA) plus ~30 min Auswahlzeit; written date 24.04.2026. Not an official-format simulation; no fee for regular school candidates.

Sample Sachsen-Anhalt Abitur Chemistry Practice Questions

Try these sample questions to test your Sachsen-Anhalt Abitur Chemistry exam readiness. Each question includes a detailed explanation. Start the interactive quiz above for the full 100+ question experience with AI tutoring.

1In an exothermic chemical reaction, how does the enthalpy of the products compare to the enthalpy of the reactants, and in which direction does energy flow?
A.The products have lower enthalpy than the reactants, and energy is released to the surroundings
B.The products have higher enthalpy than the reactants, and energy is released to the surroundings
C.The products have lower enthalpy than the reactants, and energy is absorbed from the surroundings
D.The enthalpy of products and reactants is always equal in an exothermic reaction
Explanation: An exothermic reaction releases energy to the surroundings because the products end up at a lower enthalpy level than the reactants; the enthalpy difference ΔrH is negative (ΔrH < 0). This is the basis of the Energiekonzept in the Sachsen-Anhalt Fachlehrplan, which links stored chemical energy to reaction enthalpy.
2The Fachlehrplan requires applying the 1. Hauptsatz der Thermodynamik to reaction enthalpy. What does this law state?
A.Energy can neither be created nor destroyed, only converted between forms
B.The entropy of an isolated system always increases over time
C.Every chemical reaction proceeds until equilibrium is reached
D.Reaction rate doubles for every 10°C rise in temperature
Explanation: The 1. Hauptsatz der Thermodynamik (first law) is the law of conservation of energy: the total energy of an isolated system is constant, so any energy released by a reaction as heat must equal the decrease in the system's internal energy. Sachsen-Anhalt's Fachlehrplan explicitly names this law as the basis for enthalpy calculations.
3What does the molare Standardbildungsenthalpie ΔfH°m of a compound represent?
A.The enthalpy change when one mole of the compound forms from its elements in their standard states under standard conditions
B.The total enthalpy contained within one mole of the compound
C.The enthalpy released when one mole of the compound is completely combusted
D.The enthalpy change when one mole of the compound dissolves in water
Explanation: ΔfH°m is defined as the enthalpy change for forming exactly one mole of a substance from its elements in their standard states (e.g., graphite for carbon, O2(g) for oxygen) under standard conditions. By definition, ΔfH°m of an element in its standard state is zero — this is the reference point used throughout the Fachlehrplan's Satz-von-Hess calculations.
4At grundlegendem Anforderungsniveau, what does the Fachlehrplan name as a driving force (Triebkraft) favoring chemical reactions proceeding spontaneously toward products?
A.The system tends toward a state of minimum enthalpy (Enthalpieminimum)
B.The system tends toward a state of maximum temperature
C.The system tends toward the highest possible concentration of reactants
D.The system tends toward the largest possible reaction rate
Explanation: At grundlegendem Anforderungsniveau, the Fachlehrplan names the Enthalpieminimum as a Triebkraft chemischer Reaktionen: exothermic reactions that release energy and reach a lower-enthalpy state are thermodynamically favored. At erhöhtem Anforderungsniveau this is extended with the Entropiemaximum and the Gibbs-Helmholtz-Gleichung.
5Using ΔfH°m(CH4,g) = -74.6 kJ/mol, ΔfH°m(CO2,g) = -393.5 kJ/mol, ΔfH°m(H2O,l) = -285.8 kJ/mol and ΔfH°m(O2,g) = 0, calculate the standard reaction enthalpy for CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(l).
A.-890.5 kJ/mol
B.-965.1 kJ/mol
C.-604.7 kJ/mol
D.+890.5 kJ/mol
Explanation: By the Satz von Hess, ΔrH° = ΣΔfH°m(products) − ΣΔfH°m(reactants) = [(-393.5) + 2×(-285.8)] − [(-74.6) + 2×0] = (-965.1) − (-74.6) = -890.5 kJ/mol. The large negative value confirms methane combustion is strongly exothermic, consistent with its use as a fuel.
6Given ΔfH°m(CO,g) = -110.5 kJ/mol, ΔfH°m(H2,g) = 0 and ΔfH°m(CH3OH,g) = -201.0 kJ/mol, what is the standard reaction enthalpy of CO(g) + 2 H2(g) → CH3OH(g)?
A.-90.5 kJ/mol
B.-311.5 kJ/mol
C.+90.5 kJ/mol
D.-201.0 kJ/mol
Explanation: ΔrH° = ΔfH°m(CH3OH) − [ΔfH°m(CO) + 2×ΔfH°m(H2)] = (-201.0) − [(-110.5) + 0] = -201.0 + 110.5 = -90.5 kJ/mol. Methanol synthesis from carbon monoxide and hydrogen is exothermic, which is why industrial methanol synthesis (an angewandte-Chemie context in the Fachlehrplan) must remove heat continuously.
7In a Schülerexperiment, 0.020 mol magnesium reacts completely with excess hydrochloric acid in 150 g of water, raising the temperature by 5.0 K. Using Q = cp·m·ΔT with cp(water) = 4.18 J/(g·K), calculate the molar reaction enthalpy ΔrHm.
A.-156.8 kJ/mol
B.-62.7 kJ/mol
C.+156.8 kJ/mol
D.-3.135 kJ/mol
Explanation: First find the heat released: Q = cp·m·ΔT = 4.18 J/(g·K) × 150 g × 5.0 K = 3135 J = 3.135 kJ. Then ΔrHm = -Q/n(Mg) = -3.135 kJ / 0.020 mol = -156.8 kJ/mol. The negative sign shows the reaction released heat into the water.
850.0 mL of 1.0 mol/L HCl are mixed with 50.0 mL of 1.0 mol/L NaOH in a calorimeter (total mass ≈ 100 g, cp = 4.18 J/(g·K)), and the temperature rises by 6.8 K. What is the molar neutralization enthalpy?
A.-56.8 kJ/mol
B.-28.4 kJ/mol
C.-1136 kJ/mol
D.+56.8 kJ/mol
Explanation: n(HCl) = n(NaOH) = c×V = 1.0 mol/L × 0.0500 L = 0.050 mol, and since they react 1:1, exactly 0.050 mol of water forms. Q = cp·m·ΔT = 4.18 × 100 × 6.8 = 2842.4 J = 2.842 kJ. ΔrHm = -Q/n = -2.842 kJ / 0.050 mol = -56.8 kJ/mol, close to the accepted value of about -57.3 kJ/mol for strong acid–strong base neutralization.
91.215 g of magnesium (M = 24.3 g/mol) reacts completely with excess hydrochloric acid in 200 g of water, and the temperature rises by 7.5 K (cp(water) = 4.18 J/(g·K)). Calculate the molar reaction enthalpy ΔrHm.
A.-125.4 kJ/mol
B.-250.8 kJ/mol
C.-62.7 kJ/mol
D.-6.27 kJ/mol
Explanation: First convert mass to amount: n(Mg) = 1.215 g / 24.3 g/mol = 0.0500 mol. Then Q = cp·m·ΔT = 4.18 × 200 × 7.5 = 6270 J = 6.27 kJ. Finally ΔrHm = -Q/n = -6.27 kJ / 0.0500 mol = -125.4 kJ/mol.
10Using S°m(C, graphite) = 5.7 J/(mol·K), S°m(O2,g) = 205.2 J/(mol·K) and S°m(CO2,g) = 213.8 J/(mol·K), calculate the standard reaction entropy ΔrS° for C(graphite) + O2(g) → CO2(g).
A.+2.9 J/(mol·K)
B.-2.9 J/(mol·K)
C.+424.7 J/(mol·K)
D.+8.3 J/(mol·K)
Explanation: ΔrS° = ΣS°m(products) − ΣS°m(reactants) = 213.8 − (5.7 + 205.2) = 213.8 − 210.9 = +2.9 J/(mol·K). The change is small and positive because one mole of gas (O2) is converted into one mole of gas (CO2) — the number of gas particles barely changes, so entropy barely changes, unlike reactions where the moles of gas increase or decrease sharply.

About the Sachsen-Anhalt Abitur Chemistry Practice Questions

Verified exam format metadata for Saxony-Anhalt Abitur Chemistry (Chemie) is pending. The practice questions above remain available while official exam length, timing, passing score, fee, and administrator details are reviewed.