Answer:
The answer is "Option C".
Explanation:
Please find the complete question and its solution in the attached file.
using Hoffman's elimination reaction.
Alkanes do not have a double bond, thus they are saturated. This makes them the simplest form of hydrocarbon, containing only hydrogen and carbon atoms. They are not very reactive as they don't have a double bond which can open up and join on to other molecules.
Answer : Option E) 50 grams.
Explanation : According to the solubility curves the compound 
to dissolve at 50 °C in 100 mL of water will need 50 grams of the compound. It is clearly indicated in the graph which is marked with red that at 50°C approximately 50.4 grams of the compound will be needed to dissolved in 100 mL of water to form a solution.
The final gas pressure : 175.53 atm
<h3>Further explanation</h3>
Maybe the complete question is like this :
A ridged steel tank filled with 62.7 l of nitrogen gas at 85.0 atm and 19 °C is heated to 330 °C while the volume remains constant. what is the final gas pressure?
The volume remains constant⇒Gay Lussac's Law
<em>When the volume is not changed, the gas pressure in the tube is proportional to its absolute temperature </em>
P₁=85 atm
T₁=19+273=292 K
T₂=330+273=603 K
Answer:
All of these are true
Explanation:
A buffer solution in chemistry is a solution that resists changes in pH when an acid or base is added to it. It is a solution that contains a weak acid and its conjugate base (anion) or a weak base and its conjugate acid.
A buffer is able to resist a change in pH due to the conjugate base and conjugate acid of the weak acids and bases contained in them respectively. The conjugate base/acid are present in an equilibrium quantity with their acid/base counterparts and help to neutralize or react with any additional H+ or OH- from an acid or base added to their solution.
However, when a strong acid or base is added to the buffer solution, there is only a slight change which practically does not change the pH of the solution.
Hence, all of the above options about a buffered solution is true.
