Answer; +3
Example Ca3(PO4)2
Wear gloves when handling chemicals.
Make sure that none of the liquids near the Bunsen burner are flammable.
Explanation:
The safety precautions the student must apply while completing his experiment is that he/she must wear gloves while handling the chemicals and they must make sure that none of the liquids near the Bunsen burner are flammable.
- Safety guidelines provides a detailed and careful way to carry out experiment and observations in the laboratory.
- This is all in a bid to accidents in the workspace.
- It is a good practices to wear gloves and laboratory coat while handling chemicals.
- Also make sure to put out the Bunsen burner when not in use.
- Keep papers and books away from the work area. Chemicals and papers are not friends.
- Ensure that flammable liquids are not close to the Burner.
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Answer:
There are 1031.85 grams in 4.50 moles of Ba(NO2)2
Explanation:
m = 4.50 × 229.3 = 1031.85
Answer:
Q = 19255.6 j
Explanation:
Specific heat capacity:
It is the amount of heat required to raise the temperature of one gram of substance by one degree.
Formula:
Q = m.c. ΔT
Q = amount of heat absorbed or released
m = mass of given substance
c = specific heat capacity of substance
ΔT = change in temperature
Given data:
Mass of water = 46 g
change in temperature = ΔT = 100-0.0 = 100 °C
Heat absorbed by water = ?
Solution:
Specific heat capacity of water = 4.186 j/g. °C
Q = m.c. ΔT
Q = 46 g×4.186 j/g. °C×100 °C
Q = 19255.6 j
According to the definition of half-life, the mass of the radioactive isotope halfs its mass after each half-life, which means the remaining mass is always half the amount of the previous mass.
Therefore, after the 1st half-life, there is (190/2) g left; after the 2nd half-life, there is (190/2)/2 g left; so on and so forth. After the 6th half-life, there is 190/(2*2*2*2*2*2) g = 190g/64 = 2.97 g left.
So 2.97 g of this radioactive isotope will be left after 6 half-lives.
