8519895
Description
Quiz by Kate Blowers, updated more than 1 year ago
|
Created by Kate Blowers
over 7 years ago
|
|
Question 1
Question
What is the correct equation for working out the percentage mass of an element in a compound?
Answer
-
(Relative formula mass x number of atoms of that element)/relative atomic mass of compound
-
(Relative atomic mass x number of atoms of that element)/relative formula mass of compound
-
(Relative atomic mass x relative formula mass of compoun)/number of atoms of that element
Question 2
Question
A mole is a system chemists use to count huge quantities of [blank_start]atoms or molecules[blank_end]. It is given the symbol [blank_start]n[blank_end], and is measured in a unit called the mole, shorthand [blank_start]mol[blank_end]. A mole of any substance contains the same number of atoms that are contained in [blank_start]12[blank_end]g of the isotope [blank_start]carbon-12[blank_end]. One mole of a substance is simply the [blank_start]relative atomic mass[blank_end] or [blank_start]formula mass[blank_end] expressed in [blank_start]grams.[blank_end]
Answer
-
atoms or molecules
-
n
-
mol
-
12
-
carbon-12
-
relative atomic mass
-
formula mass
-
grams.
Question 3
Question
The reactant that gets used up first in a reaction is called the limiting reactant
Answer
- True
- False
Question 4
Question
Which of these do you need to work out the limiting reactant?
Answer
-
A balanced symbol equation
-
The relative formula mass
-
The number of moles of each reactant
-
The number of electrons
Question 5
Question
Percentage yield is the amount of a produce you [blank_start]actually make[blank_end] as a [blank_start]percentage of the amount[blank_end] you should [blank_start]theoretically make.[blank_end]
Answer
-
actually make
-
percentage of the amount
-
theoretically make
Question 6
Question
Why does a high percentage yield matter to people in the industry?
Answer
-
If a yield is know for a particular product you can work out how much reactant is needed
-
A higher percentage yield = less product to produce more = higher profit
-
It's easier to work out information
-
Raw materials are scarce and expensive and so must be carefully conserved
Question 7
Question
What is the correction equation for working out percentage yield?
Answer
-
Percentage yield = (Theoretical yield/actual yield) x 100
-
Percentage yield = (Number of atoms/theoretical yield) x 100
-
Percentage yield = (Actual yield/theoretical yield) x 100
Question 8
Question
Very few reactants have a percentage yield of 100% because:
Answer
-
Products may be left behind in the apparatus
-
It violates the law of conservation of mass
-
The reaction may not have completely finished
-
The raw minerals may not be pure
-
The atoms are destroyed in the reaction
-
Some reactants may give unexpected products
Want to create your own Quizzes for free with GoConqr? Learn more.