A car manufacturer has been producing electric vehicles and decides to increase its production volume significantly by expanding its factory size and adding more assembly lines. As production increases, the fixed costs like factory rent, machinery, and administrative expenses are spread over a larger number of vehicles, reducing the average cost per car. Which economic concept best explains this decrease in average cost per vehicle? 

How much of a  30% solution do you use to make 150 mL of a 20% solution?

You require 60 mL of a 5% solution. You have a stock solution available to you in 8% strength. How much of your stock solution is needed to make this new solution?

A 5% solution is what in mg/mL?  

Assuming complete dissociation and ideal solution behavior, calculate the freezing point depression of a solution of 0.824 g of NaCl (58.44 g/mol) in 133 g of water (Kf = 1.86 ∘C·kg).

Ammonium chloride (NH₄Cl) is a salt that dissolves completely in water. The ammonium ion (NH₄⁺) acts as a weak acid with a Ka of 5.1 × 10⁻10. If a 0.050 M solution of NH₄Cl is prepared, what is the pH of the solution at 25°C?

Calculate the pH of an acetate buffer made with 0.15 M acetic acid and 0.15 M sodium acetate after adding 10.0 mL of 0.10 M NaOH to 100.0 mL of the buffer. Assume Ka​ of acetic acid is 1.8 × 10−5.

At a certain temperature, the following reaction reaches equilibrium: N2(g)+3H2(g)⇌2NH3(g) At equilibrium in a 2.00 L container, the concentrations are: [N2​]=0.400M [H2​]=0.500M The equilibrium constant at this temperature is Kc = 0.040. What is the concentration of NH3 at equilibrium?

Formic acid, HCOOH, has a Ka value equal to ~1.8 x 10-4. A student is asked to prepare a buffer with a pH of 3.2 from a 0.05 M HCOOH and a 0.05 M NaCOOH solution. How many milliliters of the NaCOOH solution should they add to 15 mL of the HCOOH solution to make the buffer?

The rate constant for a reaction is 2.5 × 10⁻³ s⁻¹ at 298 K, and 7.5 × 10⁻³ s⁻¹ at 308 K.Calculate the activation energy (Eₐ) for the reaction in kJ/mol.