Answer:
If the hydrated salt is overheated, it causes the anhydrous salt to decompose, causing the product to be lost as gas. The reported percentage of water loss will be too high because the gap between the initial measurement and final (which will be lower due to loss of sample) measurement will widen.
Answer: Depending on the state of change it can be a physical change. Example: Evaporation is the physical change of a liquid turned into a gas.
That said, I'm pretty sure the answer is (True)
Note: Hope this is correct and it helps. Good luck :)
I believe the correct answer would be that b<span>oiling points and melting points are similar because they both involve the change in a state of a material, but they are different because boiling point involves a change from a liquid to a gas and melting point involves a change from a solid to a liquid. Boiling and melting are phase changes that can happen to a substance however they differ in the process that happens.</span>
Answer:
⇒ Percent yield = 80 %
Explanation:
Given:
Actual yield = 36 g
Theoretical yield = 45 g
Find:
Percent yield
Computation:
⇒ Percent yield = [Actual yield / Theoretical yield] 100%
⇒ Percent yield = [36 / 45] 100%
⇒ Percent yield =[0.8] 100%
⇒ Percent yield = 80 %
Answer:
See Explanation
Explanation:
By definition, 1 mole is the mass of substance (or, formula mass in grams) containing 1 Avogadro's Number (N₀ = 6.02 x 10²³) of particles. That is ...
1 mole of hydrogen atoms (H) = 1.00794 grams
1 mole of molecular hydrogen (H₂) = 2.01588 grams
1 mole of any substance = 1 formula weight in grams
1 mole = 1 Avogadro's Number (N₀) = 1 formula weight in grams
In the concept of 'gas laws' 1 mole of any (all) gas at STP conditions ( => 0°C & 1 atmosphere pressure) occupies 22.4 Liters & is known as the 'molar volume' of a gas at STP. If the temperature &/or pressure change the volume will not be 22.4 Liters.
For reactions whose coefficients are balanced to the lowest whole number values (i.e., no fractional coefficients) the equation is known as the 'standard reaction' and conditions are assumed to be STP and the coefficients of gas phase components indicate molar volumes. Example ...
Given N₂(g) + 3H₂(g) => 2NH₃(g) is assumed to be at 0°C; 1 Atm pressure.
Molecular Nitrogen = 1 molar volume = 22.4 Liters of N₂(g)
Molecular Hydrogen = 3 molar volumes = 3 x 22.4 Liters of H₂(g) = 67.2 Liters of H₂(g)
Molecular Ammonia = 2 molar volumes = 2 x 22.4 Liters of NH₃(g) = 44.8 Liters of NH₃
