Answer:
![K_p= 0.00016](https://tex.z-dn.net/?f=K_p%3D%200.00016)
Explanation:
The relation between Kp and Kc is given below:
Where,
Kp is the pressure equilibrium constant
Kc is the molar equilibrium constant
R is gas constant
T is the temperature in Kelvins
Δn = (No. of moles of gaseous products)-(No. of moles of gaseous reactants)
For the first equilibrium reaction:
Given: Kc = 0.50
Temperature = ![400^oC=[400+273]K=673K](https://tex.z-dn.net/?f=400%5EoC%3D%5B400%2B273%5DK%3D673K)
R = 0.082057 L atm.mol⁻¹K⁻¹
Δn = (2)-(3+1) = -2
Thus, Kp is:
![K_p= 0.00016](https://tex.z-dn.net/?f=K_p%3D%200.00016)
Answer:837.9
Explanation:add those 2 numbers
Answer:
<h3>The answer is 14036.54 moles</h3>
Explanation:
To find the number of moles in a substance given it's number of entities we use the formula
![n = \frac{N}{L} \\](https://tex.z-dn.net/?f=n%20%3D%20%20%5Cfrac%7BN%7D%7BL%7D%20%5C%5C)
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
N = 8.45 x 10^27 molecules of H2O
We have
![n = \frac{8.45 \times {10}^{27} }{6.02 \times {10}^{23} } \\ = 14036.544850...](https://tex.z-dn.net/?f=n%20%3D%20%20%5Cfrac%7B8.45%20%5Ctimes%20%20%7B10%7D%5E%7B27%7D%20%7D%7B6.02%20%5Ctimes%20%20%7B10%7D%5E%7B23%7D%20%7D%20%20%5C%5C%20%20%3D%2014036.544850...)
We have the final answer as
<h3>14036.54 moles</h3>
Hope this helps you
Answer:
DMF is an aprotic polar solvent.
hence CN acts as a strong nucleophile in DMF to give SN2 reaction with the reactant resulting into inversion of configuration at stereo centers.
Explanation:
check the attached file for little explanation(diagram)
The balanced equation for the reaction is
C₃H₈ + 5O₂ → 3CO₂ + 4H₂<span>O
Moles (mol) = mass (g) / molar mass (g/mol)
Mass of the </span>C₃H₈ = 0.025 g
Molar mass of C₃H₈ = <span>44.1 g/mol
Hence, moles of </span>C₃H₈ = 0.025 g / 44.1 g/mol = 5.67 x 10⁻⁴ mol
The stoichiometric ratio between C₃H₈ and O₂ is 1 : 5.
Hence, moles of O₂ = moles of C₃H₈ x 5
= 5.67 x 10⁻⁴ mol x 5
= 2.835 x 10⁻³ mol
Molar mass of O₂ = <span>32.00 g/mol
Hence, mass of O</span>₂ = moles x molar mass
= 2.835 x 10⁻³ mol x 32.00 g/mol
= 0.09072 g
Hence, needed O₂ for the reaction is 0.09072 g.