Answer:
2.14 × 10⁻³ molecules/RSP
3.31 × 10⁻³ molecules/ESP
Explanation:
Step 1: Calculate the number of moles of Acetaminophen per Regular Strength Pill (RSP)
A Regular Strength Pill has 1.29 × 10²¹ molecules of Acetaminophen per pill. To convert molecules to moles we will use Avogadro's number: there are 6.02 × 10²³ molecules in 1 mole of molecules.
1.29 × 10²¹ molecules/RSP × 1 mol/6.02 × 10²³ molecules = 2.14 × 10⁻³ molecules/RSP
Step 2: Calculate the number of moles of Acetaminophen per Extra Strength Pill (ESP)
An Extra Strength Pill has 1.99 × 10²¹ molecules of Acetaminophen per pill. To convert molecules to moles we will use Avogadro's number: there are 6.02 × 10²³ molecules in 1 mole of molecules.
1.99 × 10²¹ molecules/ESP × 1 mol/6.02 × 10²³ molecules = 3.31 × 10⁻³ molecules/ESP
Answer:
<h2>12.82 moles </h2>
Explanation:
To find the number of moles in a substance given it's number of entities we use the formula

where n is the number of moles
N is the number of entities
L is the Avogadro's constant which is
6.02 × 10²³ entities
From the question we have

We have the final answer as
<h3>12.82 moles</h3>
Hope this helps you
Solution :
Time (sec) Volume of NaOH (mL)
339 26.23
1242 27.80
2745 29.70
4546 3.81
39.81
Now the example of the first order kinetics w.r.t volumetric analysis is :

Here, 

= volume at time 0 = 0
Since the interval is not constant, we take the time interval as


= 1402.3333
≈ 1402 seconds


= 0.001643 x 0.52045
= 0.00082

Therefore, the first order rate constant is k
.
NaCl and H2O.
The products are typically the elements/compounds on the right side of the equation or the right side of the arrow. The left side of the arrow would be the reactants of the equation.
Hope this helps!
<u>Answer:</u> The net ionic equation is written below.
<u>Explanation:</u>
Net ionic equation of any reaction does not include any spectator ions.
Spectator ions are defined as the ions which does not get involved in a chemical equation. They are found on both the sides of the chemical reaction when it is present in ionic form.
The chemical equation for the reaction of magnesium nitrate and aqueous ammonia (ammonium hydroxide) is given as:

A white precipitate of magnesium hydroxide is formed in the above reaction.
Ionic form of the above equation follows:

As, ammonium and nitrate ions are present on both the sides of the reaction. Thus, it will not be present in the net ionic equation and are spectator ions.
The net ionic equation for the above reaction follows:

Hence, the net ionic equation is written above.