Answer:
0.016M
Explanation:
First we find the mole of AgNO3 by using the formula mass/molar mass..
Then we find molarity by the formula mole/volume...
I hope you get this..
Answer:
The mixture is made up of different atoms and pure substance is made up of same type of atom.
The main difference is that mixture can be separated into its component by physical mean while pure substances can not be separated by physical process
Explanation:
Mixture:
- The properties of the mixture are not same and contains the properties of all those component present in it.
- it is a combination of one or more Pure substances and can be separated by simple physical methods.
- it have varying boiling and melting point
Examples are:
- mixture of salt and sand
- Salt water is mixture of water and NaCl and can be separated by physical mean.
- Alloys: its a mixture of different metal
- Air: mixture of gases
Pure Substance:
Pure substances are those made of same type of atoms all elements and compounds are pure substances.
- it can not be separated by simple physical mean
- it have very constant and consistent melting and boiling point
Examples are:
- Water : contain only water molecule
- All elements: all elements are pure substance made of same atoms
- All compounds: can not be separated by physical mean.
Answer:
Mass = 51 g
Explanation:
Given data:
Mass of nitrogen = 41.93 g
Mass of ammonia formed = ?
Solution:
Chemical equation:
N₂ + 3H₂ → 2NH₃
Number of moles of nitrogen:
Number of moles = mass/molar mass
Number of moles = 41.93 g/ 28 g/mol
Number of moles = 1.5 mol
now we will compare the moles of nitrogen and ammonia.
N₂ : NH₃
1 : 2
1.5 : 2/1×1.5 = 3 mol
Mass of ammonia formed:
Mass = number of moles × molar mass
Mass = 3 mol × 17 g/mol
Mass = 51 g
The correct answer of the given question above would be a PICTOGRAM. OSHA’s required pictograms must be in the shape of a square set at a point and
include a black hazard symbol on a white background with a red frame sufficiently wide enough to
be clearly visible.
Answer:
The reaction would shift toward the reactants
When the reaction reach equilibrium the partial pressure of NH3 will be greater than 1atm
Explanation:
For the reaction:
2NH₃(g) ⇄ N₂(g) + 3H₂(g)
Where K is defined as:
As initial pressures of all 3 gases is 1.0atm, reaction quotient, Q, is:
As Q > K, <em>the reaction will produce more NH₃ until Q = K consuming N₂ and H₂.</em>
Thus, there are true:
<h3>The reaction would shift toward the reactants</h3><h3>When the reaction reach equilibrium the partial pressure of NH3 will be greater than 1atm</h3>
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