<h3><u>Answer;</u></h3>
C → CO₂ + 4e₋
O₂ + 4e₋→ CO₂
<h3><u>Explanation</u>;</h3>
- Given the reaction C + O2 ---> CO2
- During the formation of a carbon dioxide molecule, the carbon atom shares four electrons with the oxygen atom on the left and four electrons with the oxygen atom on the right.
- This means there will be eight electrons around each atom. Two pairs of electrons shared between two atoms make a double bond between the atoms, which is represented by a double dash.
<u>Answer:</u> The equilibrium constant for the given equation is 0.0315
<u>Explanation:</u>
We are given:
Total pressure in the container = 0.596 atm
The given chemical equation follows:
![N_2H_6CO_2(s)\rightleftharpoons 2NH_3(g)+CO_2(g)](https://tex.z-dn.net/?f=N_2H_6CO_2%28s%29%5Crightleftharpoons%202NH_3%28g%29%2BCO_2%28g%29)
<u>Initial:</u> -
<u>At eqllm:</u> - 2x x
Evaluating the value of 'x'
![\Rightarrow (x+2x)=0.596\\\\x=0.199](https://tex.z-dn.net/?f=%5CRightarrow%20%28x%2B2x%29%3D0.596%5C%5C%5C%5Cx%3D0.199)
The expression of
for above equation follows:
![K_p=p_{CO_2}\times (p_{NH_3})^2](https://tex.z-dn.net/?f=K_p%3Dp_%7BCO_2%7D%5Ctimes%20%28p_%7BNH_3%7D%29%5E2)
The partial pressure of pure solids and pure liquids are taken as 1 in the equilibrium constant expression.
Putting values in above expression, we get:
![K_p=(0.199)\times (2\times 0.199)^2\\\\K_p=0.0315](https://tex.z-dn.net/?f=K_p%3D%280.199%29%5Ctimes%20%282%5Ctimes%200.199%29%5E2%5C%5C%5C%5CK_p%3D0.0315)
Hence, the equilibrium constant for the given equation is 0.0315
Answer:
single displacement reaction
Explanation:
it is because an atom(Pb) dispalces another atom(H) in H3PI4
Answer: 94.07%
Explanation:
Percentage yield can be calculated by the formula
%yield = Experimental yield/Theoretical yield x100
Experimental yield = 7.93g
Theoretical yield = 8.43
%yield = Experimental yield/Theoretical yield x100
%yield = 7.93/8.43 x 100 = 94.07%