Answer:
1.Mg+O2.......MgO2
Explanation:
2.Very reactive towards halogens and reacts with water at room temperature. 3, Magnesium oxide is a simple basic oxide. 4.It will react with water to form magnesium hydroxide which is a base turning red litmus to blue 5.should be white. hope it helped. I help people although when I post a question it is left unanswered and then gets answers after two days when I don't really need it
Annswer is B Explanation:acording to this diagram i f
gffgdffdggfdfgd
Not all matter in the reactant goes to the product. Some matter is byproducts.
ΔHrxn = ΣδΗ(bond breaking) - ΣδΗ(bond making)
Bond enthalpies,
N ≡ N ⇒ 945 kJ mol⁻¹
N - Cl ⇒ 192 kJ mol⁻¹
Cl - Cl⇒ 242 kJ mol⁻¹
According to the balanced equation,
ΣδΗ(bond breaking) = N ≡ N x 1 + Cl - Cl x 3
= 945 + 3(242)
= 1671 kJ mol⁻¹
ΣδΗ(bond making) = N - Cl x 3 x 2
= 192 x 6
= 1152 kJ mol⁻¹
δHrxn = ΣδΗ(bond breaking) - ΣδΗ(bond making)
= 1671 kJ mol⁻¹ - 1152 kJ mol⁻¹
= 519 kJ mol⁻¹
Answer:
No, no precipitate is formed.
Explanation:
Hello there!
In this case, since the reaction between silver nitrate and sodium acetate is:
In such a way, we can calculate the concentration of silver and acetate ions in the solution as shown below, and considering that the final total volume is 50.00 mL or 0.0500 L:
![[Ag^+]=\frac{20.00mL*0.077M}{50.00mL}=0.0308M](https://tex.z-dn.net/?f=%5BAg%5E%2B%5D%3D%5Cfrac%7B20.00mL%2A0.077M%7D%7B50.00mL%7D%3D0.0308M)
![[C_2H_3O_2^-]=\frac{30.00mL*0.043M}{50.00mL}=0.0258M](https://tex.z-dn.net/?f=%5BC_2H_3O_2%5E-%5D%3D%5Cfrac%7B30.00mL%2A0.043M%7D%7B50.00mL%7D%3D0.0258M)
In such a way, we can calculate the precipitation quotient by:
![Q=[Ag^+][C_2H_3O_2^-]=0.0308*0.0258=7.95x10^{-4}](https://tex.z-dn.net/?f=Q%3D%5BAg%5E%2B%5D%5BC_2H_3O_2%5E-%5D%3D0.0308%2A0.0258%3D7.95x10%5E%7B-4%7D)
Which is smaller than Ksp and meaning that the precipitation does not occur.
Regards!
