O2 mol O2 2 mil CO2 O1molO2
110 calories are required to raise the temperature.
-
Specific heat = calories / mass * (final temperature - initial temperature)
Insert known factors of the equation before rearranging to isolate the unknown (in this case, calories)
0.11 = calories / 10 * (200 - 100)
0.11 = calories / 10 * 100
0.11 * (10 * 100) = calories
0.11 * 1000 = calories
110 = calories
Answer:
25 mol.
Explanation:
The balanced chemical equation for the reaction depicted in this question is as follows:
4Fe + 3O2 → 2Fe2O3
Based on the above balanced equation, 4 moles of Fe produced 2 moles of Fe2O3.
Hence, 50 moles of Fe will produce as follows:
50 mol Fe × 2 mol Fe2O3/4 mol Fe
= 100/4
= 25 mol of Fe2O3
Answer: 1. n
2. n
3.
4. l
Explanation:
Principle Quantum Numbers : It describes the size of the orbital and the energy level. It is represented by n. Where, n = 1,2,3,4....
Azimuthal Quantum Number : It describes the shape of the orbital. It is represented as 'l'. The value of l ranges from 0 to (n-1).For l = 0,1,2,3... the orbitals are s, p, d, f...
Magnetic Quantum Number : It describes the orientation of the orbitals. It is represented as . The value of this quantum number ranges from -l to +l.
Spin Quantum number : It describes the direction of electron spin. This is represented as s.
Answer:
6.57 L
Explanation:
First, calculate the <em>moles of hydrogen</em> produced, then use the Ideal Gas Law to calculate the <em>volume of hydrogen</em>.
Step 1. Write the <em>chemical equation</em>.
: 22.99
2Na + H₂O ⟶ 2NaOH + H₂
Step 1. Convert <em>grams of Na</em> to <em>moles of Na</em>
Step 2. Use the molar ratio of H₂:Na to convert <em>moles of Na</em> to <em>moles of H₂</em>.
Step 3. Use the Ideal Gas Law to calculate the <em>volume of hydrogen</em>.
<em>pV = nRT</em>