Post Test Day 2

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For Grade 10 students

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Ma'am Dane

Philippines

Ce jeu est une version de

Pre Test Day 2

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Post Test Day 2


Post Test Day 2Version en ligne For Grade 10 students par Ma'am Dane 1 A science teacher asked, "What does molar mass describe?" a The number of particles in one atom b The mass of one mole of a substance c The volume of one mole of a gas d The number of atoms in a compound 2 Before calculating the molar mass of a compound, a student first looks at the Periodic Table. Why is the Periodic Table needed? a It shows the atomic masses of the elements. b It shows the color of each element. c It tells whether a compound is solid or liquid. d It gives the number of particles in one mole. 3 A student needs to calculate the molar mass of methane (CH₄). Use the atomic masses: ● C = 12 ● H = 1 What is the molar mass of CH₄? a 12 g/mol b 14 g/mol c 16 g/mol d 18 g/mol 4 A laboratory uses ammonia (NH₃) during an investigation. Use the atomic masses: ● N = 14 ● H = 1 What is the molar mass of NH₃? a 15 g/mol b 16 g/mol c 17 g/mol d 18 g/mol 5 A student calculated the molar mass of CO₂ as 28 g/mol. Which explanation best describes the mistake? a The student counted only one oxygen atom. b The student forgot to include both oxygen atoms when adding the atomic masses. c The student added an extra carbon atom d The student used the atomic number instead of the atomic mass. 6 Three students calculated the molar mass of methane (CH₄). ● Student A: 12 g/mol ● Student B: 16 g/mol ● Student C: 20 g/mol Based on the atomic masses C = 12 and H = 1, whose calculation is correct? a Student A b Student B c Student C d All of them 7 A student says, "Carbon dioxide (CO₂) and water (H₂O) have the same molar mass because both contain oxygen." How should you evaluate this statement? a Correct, because both compounds contain oxygen. b Correct, because every compound has the same molar mass. c Incorrect, because molar mass depends on all the atoms in the formula. d Incorrect, because oxygen has no mass 8 Four groups calculated the molar mass of sodium chloride (NaCl). ● Group A: 46 g/mol ● Group B: 58.5 g/mol ● Group C: 69 g/mol ● Group D: 81 g/mol Which group's calculation should the teacher accept? a Group A b Group B c Group C d Group D 9 Your group needs a compound with a molar mass of about 44 g/mol for an experiment. Which compound should your group choose? a H₂O b NH₃ c CH₄ d CO₂ 10 A classmate asks for the best way to calculate the molar mass of any compound. Which explanation should you give? a Multiply the number of moles by Avogadro's number. b Find the atomic mass of each element, multiply by the number of atoms shown in the formula, then add the values. c Divide the mass by the number of particles. d Add the atomic numbers of all the elements.

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Post Test Day 2

Test

À propos de cette activité

Créé par

Téléchargez la version pour jouer sur papier

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Post Test Day 2Version en ligne

par Ma'am Dane

A science teacher asked, "What does molar mass describe?"

Before calculating the molar mass of a compound, a student first looks at the Periodic Table. Why is the Periodic Table needed?

A student needs to calculate the molar mass of methane (CH₄). Use the atomic masses: ● C = 12 ● H = 1 What is the molar mass of CH₄?

A laboratory uses ammonia (NH₃) during an investigation. Use the atomic masses: ● N = 14 ● H = 1 What is the molar mass of NH₃?

A student calculated the molar mass of CO₂ as 28 g/mol. Which explanation best describes the mistake?

Three students calculated the molar mass of methane (CH₄). ● Student A: 12 g/mol ● Student B: 16 g/mol ● Student C: 20 g/mol Based on the atomic masses C = 12 and H = 1, whose calculation is correct?

A student says, "Carbon dioxide (CO₂) and water (H₂O) have the same molar mass because both contain oxygen." How should you evaluate this statement?

Four groups calculated the molar mass of sodium chloride (NaCl). ● Group A: 46 g/mol ● Group B: 58.5 g/mol ● Group C: 69 g/mol ● Group D: 81 g/mol Which group's calculation should the teacher accept?

Your group needs a compound with a molar mass of about 44 g/mol for an experiment. Which compound should your group choose?

A classmate asks for the best way to calculate the molar mass of any compound. Which explanation should you give?