Answer: 1 Mole or 6.022 X 1023.
Answer:
6.2846
Explanation:
Given that:-
Concentrations at equilibrium :-
![[CH_4]=0.126\ M](https://tex.z-dn.net/?f=%5BCH_4%5D%3D0.126%5C%20M)
![[H_2O]= 0.242\ M](https://tex.z-dn.net/?f=%5BH_2O%5D%3D%200.242%5C%20M)
![[CO]= 0.126\ M](https://tex.z-dn.net/?f=%5BCO%5D%3D%200.126%5C%20M)
![[H_2]= 1.15\ M](https://tex.z-dn.net/?f=%5BH_2%5D%3D%201.15%5C%20M)
The equilibrium reaction is:-
The expression for equilibrium constant is:
![K_{c}=\frac {\left [ H_2 \right ]^3\left [ CO \right ]}{\left [ CH_4 \right ]\left [ H_2O \right ]}](https://tex.z-dn.net/?f=K_%7Bc%7D%3D%5Cfrac%20%7B%5Cleft%20%5B%20H_2%20%5Cright%20%5D%5E3%5Cleft%20%5B%20CO%20%5Cright%20%5D%7D%7B%5Cleft%20%5B%20CH_4%20%5Cright%20%5D%5Cleft%20%5B%20H_2O%20%5Cright%20%5D%7D)
Applying the values as:-
<u>The equilibrium constant for the reaction is:- 6.2846</u>
City B is at a higher temperature because as you go higher in altitude the boiling point of water becomes lower.
Red blood cells. Need glucose oxygen to convert to carbon dioxide
Answer:
Mass of magnesium oxide formed = 35.1 g
Explanation:
Given data:
Mass of Mg = 20.9 g
Mass of O₂ = 15.2 g
Mass of magnesium oxide formed = ?
Solution:
Chemical equation:
2Mg + O₂ → 2MgO
Number of moles of Mg:
Number of moles = mass/molar mass
Number of moles = 20.9 g/ 24 g/mol
Number of moles = 0.87 mol
Number of moles of O₂:
Number of moles = mass/molar mass
Number of moles = 15.2 g/ 32 g/mol
Number of moles = 0.475 mol
Now we will compare the moles of MgO with magnesium and oxygen.
Mg : MgO
2 : 2
0.87 : 0.87
O₂ : MgO
1 : 2
0.475 : 2/1×0.475 = 0.95
Number of moles of MgO formed by Mg are less thus Mg will limiting reactant.
Mass of MgO:
Mass = number of moles × molar mass
Mass = 0.87 mol × 40.3 g/mol
Mass = 35.1 g
