Answer: partial pressure of NOBr is 7792 atm
Explanation:
Equilibrium constant is the ratio of the concentration of products to the concentration of reactants each term raised to its stochiometric coefficients.
Equilibrium constant is given as:
![K_{p}=\frac{[p_{NOBr}]^2}{[p_{NO}]^2\times [p_{Br_2}]^1}](https://tex.z-dn.net/?f=K_%7Bp%7D%3D%5Cfrac%7B%5Bp_%7BNOBr%7D%5D%5E2%7D%7B%5Bp_%7BNO%7D%5D%5E2%5Ctimes%20%5Bp_%7BBr_2%7D%5D%5E1%7D)
![28.4=\frac{[p_{NOBr}]^2}{[(119)^2\times (151)^1}](https://tex.z-dn.net/?f=28.4%3D%5Cfrac%7B%5Bp_%7BNOBr%7D%5D%5E2%7D%7B%5B%28119%29%5E2%5Ctimes%20%28151%29%5E1%7D)
![[p_{NOBr}]=7792](https://tex.z-dn.net/?f=%5Bp_%7BNOBr%7D%5D%3D7792)
atm
Partial pressure of NOBr is 7792 atm
Answer:
9.94 mL, the volume of ethanol needed
Explanation:
The reaction is:
C₂H₅OH(l) + 3 O₂(g) → 2 CO₂(g) + 3 H₂O(l)
We convert the mass of the formed product to moles:
15 g . 1mol / 44g = 0.341 moles
2 moles of dioxide are produced by 1 mol of ethanol, in order to stoichiometry.
Therefore, 0.341 moles of CO₂ must be produced by (0.341. 1) / 2 = 0.1705 moles of alcohol.
We convert the moles to mass, and then, the mass to volume by the use of density.
0.1705 mol . 46 g / 1 mol = 7.84 g of ethanol
Ethanol density = Ethanol mass /Ethanol volume
Ethanol volume = Ethanol mass /Ethanol density → 7.84 g /0.789 g/mL =
9.94 mL
Compound is a pure substance where atoms of two or more elements are chemically bonded togather
The others are wrong it's B. Condensation
Explanation:
Two events involving electrons are gain and loss of electrons.
When there is gain or loss of electrons between two atoms then it results in the formation of ionic bond.
Whereas when there is sharing of electrons between two atoms then it results in the formation of covalent bond.
Therefore, the chemical bonds formed can be ionic or covalent bonds.
