0.6 mol / L is the molarity of a solution prepared by dissolving 36. 0 g of NaOH in enough water to make 1. 50 l of solution.
The amount of a substance in a specific volume of solution is known as its molarity (M). The number of moles of a solute per liter of a solution is known as molarity. The molar concentration of a solution is another term for molarity.
The ratio employed to indicate the solution's concentration is called its molarity. Understanding a solution's molarity is important since it allows you to determine the actual concentration as well as whether the solution is diluted or concentrated.
Amount of NaOH = 36. 0 g
Amount of water = 1. 50 L
1 mol of NaOH = 40 g,
Moles of NaOH = 36. 0 / 40 g = 0.9 mol NaOH
Molarity of a solution = moles of solute / Liters of solution
Molarity of a solution = 0.9 / 1.50
Molarity of a solution = 0.6 mol / L
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The answer is leucine would be in the interior, and serine would be on the exterior of the globular protein.
The side chain (R group) of the amino acid serine is CH₂OH. The side chain of the amino acid leucine is CH₂CH(CH₃)₂. In globular protein, leucine found in the interior, and serine found on the exterior. The nature of side chain decides the amino acid position in the globular protein , as CH₂CH(CH₃)₂ this is hydrophobic and CH₂OH is hydrophlic.
WE CAN SEE ATOMS!?!?! I swear I'm getting dumber everyday
but I think is like a.... a penny?
Answer:
A. To focus on only those ions that form the precipitate
Explanation:
Net ionic equations cancel out the ions that appear on both sides of the reaction because they essentially don't participate in the reaction. This is very useful when dealing with redox reactions because are complicated enough without spectator ions being in the way, so they help focus on those ions that actually form the precipitate.
Key Terms
- Spectator Ions: an ion that does not take part in the chemical reaction.
- Net ionic equations: a equation where ions that appear on both sides are canceled out.
- Redox reaction: an oxidation-reduction reaction.
The Haber process (a) is used to manufacture ammonia.
The Haber process, which artificially fixes nitrogen, is currently the primary industrial method for producing ammonia.
Using a metal catalyst and high temperatures and pressures, the process turns atmospheric nitrogen (N2) into ammonia (NH3) by reacting with hydrogen (H2).
Haber's reaction is - N2 + H2 ------> NH3
The gases (nitrogen and hydrogen) are passed through four beds of catalyst in this conversion, which is normally carried out at pressures above 10 MPa (100 bar; 1,450 psi) and between 400 and 500 °C (752 and 932 °F). Cooling is applied between each pass to maintain a reasonable equilibrium constant.
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