Suppose a reaction were to happen in an open container in a lab. During the reaction, the scientist observes the chemicals bubble, and produce a gas. During the analysis the scientist notices that the reactants weighed 20 g when he started, and the product weighed 18 g. Explain what happened.

The gas that was produced was not able to be weighed since the container was open.

His chemical reaction defied the law of conservation of mass

The product destroyed mass during the reaction

The reactants created matter during the reaction

How does the concept of conservation of mass apply to chemical reactions?

The reactants and products have exactly the same atoms.

The reactants and products have exactly the same molecules.

The change in the amount of matter is equal to the change in energy.

The change in the amount of matter is only a small percentage of the total mass

A chemical reaction separates water into hydrogen gas and oxygen gas. Which of the following statements is true about the mass of the water and the combined mass of the two gases?

The combined mass of the two gases is the same as the mass of the water.

The mass of the water is greater than the combined mass of the two gases.

The combined mass of the two gases is much greater than the mass of the water

The mass of the water is the same as double the combined mass of the two gases

Which best explains why the total mass of the product(s) would be less than the total weight of the reactant(s) after a chemical reaction?

Gases were released to the atmosphere

Atoms involved in the reaction lost mass

Precipitates were created in the new solution

When chemicals react in a closed container, which must be true?

The mass both before and after the reaction is the same

The mass both before and after the reaction is variable

The same number of compounds is present both before and after the reaction

Which best represents a balanced equation?

120 grams of carbon plus 80 grams of oxygen → 200 grams of carbon dioxide

120 grams of carbon plus 20 grams of oxygen → 200 grams of carbon dioxide

120 grams of carbon plus 50 grams of oxygen → 200 grams of carbon dioxide

What is the importance of a closed container in a chemical reaction?

to observe the mass before and after the reaction occurs

to keep any materials from interfering with the reaction

to observe the loss of mass after the reaction occurs

The Law of Conversion of Mass

Authored by Charles Martinez

Chemistry

11th Grade

NGSS covered

Used 2+ times

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MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Law of conservation of mass states that

mass is created

mass is destroyed

mass is neither created nor destroyed

mass does not change

Tags

NGSS.MS-PS1-5

MULTIPLE CHOICE QUESTION

2 mins • 1 pt

100g of white powder reacts with 77g of clear liquid. The reaction bubbles and changes color producing a yellow liquid that has a mass of 90g. What can be concluded?

97g of gas was produced

This experiment violates the conservation of mass

87g of gas was produced

The excess reactant is destroyed & disappears during the reaction

Tags

NGSS.MS-PS1-5

NGSS.MS-PS1-2

MULTIPLE CHOICE QUESTION

1 min • 1 pt

What are the REACTANTS :
H₂O + CO₂ → HCO + HO

H₂O and CO₂

HCO and HO

H₂O ONLY

HCO ONLY

Tags

NGSS.MS-PS1-2

NGSS.MS-PS1-1

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

REACTANTS are always on what side of the chemical equation?

right

left

top

bottom

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Which of the following are PRODUCTS?
H₂O + CO₂→ HCO + HO

H₂O and CO₂

HCO and HO

H₂O ONLY

HCO ONLY

Tags

NGSS.MS-PS1-5

NGSS.MS-PS1-2

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

PRODUCTS are always on what side of the equation?

right

left

top

bottom

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

If there are 4 H atoms on the reactant side, how many H atoms will be on the product side?

You need more information to answer this question

Tags

NGSS.MS-PS1-5

NGSS.MS-PS1-2

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The Law of Conversion of Mass

Law of conservation of mass states that

100g of white powder reacts with 77g of clear liquid. The reaction bubbles and changes color producing a yellow liquid that has a mass of 90g. What can be concluded?

What are the REACTANTS :
H₂O + CO₂ → HCO + HO

REACTANTS are always on what side of the chemical equation?

Which of the following are PRODUCTS?
H₂O + CO₂→ HCO + HO

PRODUCTS are always on what side of the equation?

If there are 4 H atoms on the reactant side, how many H atoms will be on the product side?

Suppose a reaction were to happen in an open container in a lab. During the reaction, the scientist observes the chemicals bubble, and produce a gas. During the analysis the scientist notices that the reactants weighed 20 g when he started, and the product weighed 18 g. Explain what happened.

How many nitrogen atoms does NH₃ have?

Mass cannot be created or__________ during a chemical reaction?

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The Law of Conversion of Mass

Law of conservation of mass states that

100g of white powder reacts with 77g of clear liquid. The reaction bubbles and changes color producing a yellow liquid that has a mass of 90g. What can be concluded?

What are the REACTANTS :H2O + CO2 → HCO + HO

REACTANTS are always on what side of the chemical equation?

Which of the following are PRODUCTS?H2O + CO2 → HCO + HO

PRODUCTS are always on what side of the equation?

If there are 4 H atoms on the reactant side, how many H atoms will be on the product side?

Suppose a reaction were to happen in an open container in a lab. During the reaction, the scientist observes the chemicals bubble, and produce a gas. During the analysis the scientist notices that the reactants weighed 20 g when he started, and the product weighed 18 g. Explain what happened.

How many nitrogen atoms does NH3 have?

Mass cannot be created or__________ during a chemical reaction?

Access all questions and much more by creating a free account

Similar Resources on Wayground

Popular Resources on Wayground

Discover more resources for Chemistry

What are the REACTANTS :
H₂O + CO₂ → HCO + HO

Which of the following are PRODUCTS?
H₂O + CO₂→ HCO + HO

How many nitrogen atoms does NH₃ have?