Currently unavailable: for new students
Degree: MChem Chemistry (Masters) - Warwick University
As a second year student at the University of Warwick studying an integrated Masters in Chemistry, I have always had a keen interest in all the sciences and maths, and enjoy these subjects at all levels of education. I aim to pass this enthusiasm onto you, providing an atmosphere that can help you learn and achieve your potential.
I am friendly, approachable and patient. I am looking forward to passing on the knowledge I have gained through my degree and other qualifications – the world of science is simply amazing! With the right explanations, connections can be made through all the sciences and the possibilities are endless!
Each tutorial is 55 mins long - as much, or as little, as you want can be covered in this time. Whether you would like to start from the foundations of a concept or build on top of your current knowledge, I will tailor the tutorials around you! The pace, topics and learning styles are all based on you – this is the advantage of a one-to-one tutorial.
Many different techniques will be used to aid your learning – simple explanations, diagrams, graphs, analogies and practice. These will help you reach your potential and achieve higher grades. In an exam, and in real life, you will need to know how to apply this knowledge and not just know all the information – I intend to develop those skills alongside passing on the knowledge.
Once concepts have been covered and firmly grasped, I aim for you to be confident enough to explain the topic to me – this way you will be ready to tackle any questions on the topic. I can also help you work through and explain past paper questions, providing you with an example of how to approach questions and apply your knowledge. As an alternative, feel free to try them and bring them to me to explain concepts you don’t understand and would like clarification.
Contact me through the mailing system if you have any questions, or arrange a ‘meet the tutor’ session through this website.
Before tutorials it would benefit both of us if you send me information regarding your exam board, level of education (GCSE or A-level) and topic area/specific questions you require more help with; this will enable me to tailor my tuition to your needs.
I look forward to hearing from you!
|Chemistry||A Level||£20 /hr|
|Before 12pm||12pm - 5pm||After 5pm|
Please get in touch for more detailed availability
Izzy (Student) April 27 2016
Ridwaan (Student) April 26 2016
Emily (Student) October 18 2016
Emily (Student) October 9 2016
When faced with this style of problem there are steps to correctly answer the quesion:
Step 1 - identify the atomic mass of carbon
Step 2 - calculate the atomic mass of the compound
Step 3 - work out the percentage, by mass, of carbon in the compound
To calculate the atomic mass, a periodic table is required. The atomic mass of each element is located at the top of the element, displayed as a number. In this case carbon has an atomic mass of 12 g/mol.
The same principles in step 1 are required and applied to the remaining atoms in the compound - sodium hydrogen carbonate. The atoms in the compound are sodium (Na), hydrogen (H), carbon (C) and oxygen (O). Looking at the value of atomic mass on the periodic table, the values of atomic mass are as follows:
Na = 23 g/mol
H = 1 g/mol
C = 12 g/mol
O = 16 g/mol
There is 1 Na atom, 1 H atom, 1 C atom and 3 O atoms in the compound. Now add these values together to get the atomic mass of the compound as such:
23+1+12+(3*16) = 84 g/mol
Now the percentage, by mass, needs to be calculated. The general rule for calculating a percentage is:
percentage = (value/total)*100%
Therefore by applying this rule for our problem we find that
Percentage = (12/84)*100% = 14.3 % (to 1 d.p)see more
An isotope is a different form of the same element. They differ from each other by the number of neutrons, however they have the same number of protons and electrons. This results in a different atomic mass.
Lets use an example - carbon:
Carbon (C) can form different isotopes, with the most abundant being C-12 and C-13.
C has 6 protons (stated under the element on a periodic table) and an equal number of electrons to balance the charge. C-12 has 6 neutrons and C-13 has 7 neutrons, because adding the number of neutrons and protons determines the atomic mass of the isotope (electrons have negligable mass).see more