education.com has been visited by 100K+ users in the past month
Bring learning to life with worksheets, games, lesson plans, and more from Education.com. Access the most comprehensive library of K-8 resources for learning at school and at home.
- Printable Workbooks
Download & print 300+ workbooks
written & reviewed by teachers.
- Education.com Blog
See what's new on Education.com,
explore classroom ideas, & more.
- Printable Workbooks
Search results
Revision notes on 1.6.2 Empirical Formulae for the Edexcel GCSE Chemistry syllabus, written by the Chemistry experts at Save My Exams.
EMPIRICAL FORMULAE 1. Benzene has the molecular formula C6H6. Its empirical formula is CH. Explain what each of these formulas tells us about benzene. molecular formula: 6C & 6H atoms in each molecule empirical formula: ratio of C:H is 1:1. The empirical formula of sodium chloride is NaCl. It does not have a molecular formula.
- 197KB
- 2
The periodic table lists the elements, each element has a symbol with two numbers. One number is above the symbol and the other number is below the symbol. The mass number is the total number of protons and neutrons. The atomic number is the number of protons in an atom of the element.
REACTING MASS CALCULATIONS 1. 1) Aluminium is extracted from aluminium oxide as shown. Calculate the mass of aluminium that can be formed from 1020 g of aluminium oxide. = 10.0 mol. 2) Calculate the mass of oxygen needed to react 10.0 g of calcium to form calcium oxide.
Worked Example 1 In a reaction between propane and oxygen, 36 g of water is produced. Use the balanced symbol equation below to calculate the mass of propane needed for this reaction (assume oxygen is in excess).
Nov 1, 2018 · Using Equation 1 Example 1: What is the number of moles in 35.0g of CuSO4? moles = mass/Mr = 35.0/ (63.5 + 32.0 +16.0 x4) = 0.219 mol Molar Mass (Mr) for a compound can be calculated by adding up the mass numbers (f rom the periodic table) of each element in the compound eg CaCO3 = 40.1 + 12.0 +16.0 x3 = 100.1 moles = mass Mr 1.
An element has the following natural abundances and isotopic masses: 90.92% abundance with 19.99 amu, 0.26% abundance with 20.99 amu, and 8.82% abundance with 21.99 amu. Calculate the average atomic mass of this element. Answer. Click here to see a video of the solution.
Access thousands of printable worksheets. Ideal for homeschooling and extra practice! Practice with our fun and free number and shapes worksheets to boost your child's learning
