quantitive chemcical reactions gcse aqa Flashcards

1
Q

What is a quantitative chemical reaction?

A

A reaction that involves measuring the amounts of reactants and products.

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2
Q

True or False: The law of conservation of mass states that mass is created in a chemical reaction.

A

False

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3
Q

What is the formula for calculating moles?

A

Moles = Mass (g) / Molar Mass (g/mol)

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4
Q

Fill in the blank: The molar mass of water (H2O) is ____ g/mol.

A

18

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5
Q

How do you calculate the mass of a reactant needed for a reaction?

A

Mass = Moles × Molar Mass

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6
Q

What is the role of a balanced chemical equation in quantitative reactions?

A

It shows the ratio of moles of reactants to products.

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7
Q

What does the term ‘yield’ refer to in a chemical reaction?

A

The amount of product obtained from a reaction.

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8
Q

What is the ideal yield in a chemical reaction?

A

Theoretical yield calculated from the balanced equation.

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9
Q

True or False: Actual yield is always equal to theoretical yield.

A

False

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10
Q

What is percentage yield?

A

Percentage yield = (Actual yield / Theoretical yield) × 100%

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11
Q

What is the molar volume of a gas at room temperature and pressure (RTP)?

A

24 dm³/mol

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12
Q

Fill in the blank: One mole of any gas occupies ____ dm³ at RTP.

A

24

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13
Q

What is the term for the smallest whole number ratio of moles in a reaction?

A

Stoichiometry

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14
Q

How do you find the limiting reactant in a reaction?

A

By calculating the moles of each reactant and determining which one runs out first.

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15
Q

What is the balanced equation for the reaction between hydrogen and oxygen to produce water?

A

2H₂ + O₂ → 2H₂O

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16
Q

What is the significance of the coefficients in a balanced equation?

A

They represent the number of moles of each substance involved.

17
Q

True or False: Increasing temperature generally increases the rate of a chemical reaction.

18
Q

What is the effect of concentration on the rate of reaction?

A

Higher concentration increases the rate of reaction.

19
Q

What is meant by ‘excess reagent’?

A

A reactant that remains after the reaction has gone to completion.

20
Q

Fill in the blank: The molar mass of carbon dioxide (CO2) is ____ g/mol.

21
Q

What is the formula to calculate the number of moles of a gas?

A

Moles = Volume (dm³) / Molar Volume (24 dm³/mol)

22
Q

What does a reaction yield of 50% indicate?

A

The actual yield is half of the theoretical yield.

23
Q

How do you convert grams of a substance to moles?

A

Divide the mass in grams by the molar mass.

24
Q

What is the formula for calculating the mass of product formed in a reaction?

A

Mass of product = (Moles of reactant used) × (Molar mass of product)

25
True or False: Stoichiometric calculations are based on the balanced equation.
True
26
What is the term for a reaction that goes to completion?
Irreversible reaction
27
Fill in the blank: The limiting reactant determines the ____ of the reaction.
amount of product formed
28
What is the significance of the term 'molarity'?
It measures the concentration of a solution in moles per liter.
29
What is the unit of molarity?
moles per liter (mol/L)
30
How do you calculate the concentration of a solution?
Concentration = Moles of solute / Volume of solution (L)
31
What does it mean if a reaction has a high percentage yield?
It indicates that most of the reactants were converted into products.
32
What is the purpose of titration in quantitative chemistry?
To determine the concentration of a solution.
33
What is the relationship between moles and volume for gases at RTP?
1 mole of gas occupies 24 dm³ at RTP.
34
Fill in the blank: The molar mass of sodium chloride (NaCl) is ____ g/mol.
58.5
35
What is the first step in performing a stoichiometric calculation?
Write and balance the chemical equation.
36
True or False: The coefficients in a balanced equation can be fractional.
False
37
What is the term for a reaction that can proceed in both directions?
Reversible reaction