<span>let x=gallons of current mixture to be drained
and replaced with pure antifreeze.
4-x=gallons of current mixture remaining in the car.</span>
<span>
0.15(4-x)+1.00x=0.50 x 4
0.6-.15x+x=2
0.85x=1.4
x=1.4/0.85 =1.65 gal
Thus, 1.65 gallons of current mixture to be drained and replaced with pure
antifreeze.</span>
Answer:
By increasing the pressure, the molar concentration of N2O4 will increase
Explanation:
We have the equation 2NO2 ⇔ N2O4
This equation is reversible and exotherm. By <u>decreasing the temperature</u>, the reaction will produce more energy, so the reaction will move to the right. But a lower temperature also lowers the rate of the process, so, the temperature is set at a compromise value that allows N2O4 to be made at a reasonable rate with an equilibrium concentration that is not too unfavorable
So <u>increasing the temperature</u> will shift the equilibrium to the left. The equilibrium shifts in the direction that consumes energy.
If we d<u>ecrease the concentration of NO2</u>, the equilibrium will shift to the left, resulting in forming more reactants.
To increase the molar concentration of the product N2O4, we have to <u>increase the pressure</u> of the system.
NO2 takes up more space than N2O4, so increasing the pressure would allow the reactant to collide more form more product.
By increasing the pressure, the molar concentration of N2O4 will increase
1 mole K ------------- 6.02x10²³ atoms
1.83 moles K ------ ?? atoms
1.83 x (6.02x10²³) / 1 =
1.101x10²⁴ atoms of K
hope this helps!
Answer:
You
Explanation:
Will have to fill in the graph organizer with a story
