The practical work inside the lab includes lab equipments, chemicals, and the practical outside a laboratory is more about conservation of nature and practicals include natural things in their living areas.
What are lab practicals?
Practicals are set up stations with lab equipments and chemicals and where students learn practical of the theoretical statements.
The exams of practicals are done to test the leaning of chemistry of the students.
Thus, the practical work inside the lab includes lab equipments, chemicals, and the practical outside a laboratory is more about conservation of nature and practicals include natural things in their living areas.
Learn more about lab practicals
brainly.com/question/11850721
#SPJ1
Answer:
An elastic collision.
Explanation:
When a ball is dropped to the ground, one of four things may happen: It may rebound with exactly the same speed as the speed at which it hit the ground. This is an elastic collision.
To find the amount of moles in 0.00032g of lithium, all you have to do is apply the formula n (moles) = m (mass, grams)/MM(molar mass). Molar mass is the atomic weight of the substance, and all you have to do is look at the periodic table. Lithium's is 6.94.
So, n (lithium) = 0.00032/6.94
n (lithium) = 0.000046 moles (2 d.p)
Take into account the number of atoms in the molecule for other calculations. Some elements are diatomic, which means they occur as two atoms of the same element bonded, such as hydrogen (H2) and chloride (Cl2). This means that to find moles of a substance such as Cl2, you need to multiply the molar mass by 2, since there are 2 atoms. Additionally, for compounds, you need to find the sum of all the elements involved's molar mass. For example, when you’re trying to find the moles in table salt, NaCl (sodium chloride), add the atomic weight of sodium and chlorine together for your molar mass.
Hope this helped!
Kg is the abbreviation for an SI unit of mass, which is kilogram
Atomic mass Au = 196.96 u.m.a
196.96 g ----------- 6.02x10²³ atoms
0.00x10⁻¹⁰ g ------- ( atoms ? )
( 0.00 x10⁻¹⁰) x 6.02x10²³ / 196.96
0 / 196.96
= 0 atoms