Answer:
7.04 g
Explanation:
Let's consider the reaction in the last step of the Ostwald process.
3 NO₂(g) + H₂O(l) → 2 HNO₃(aq) + NO(g)
The molar mass of HNO₃ is 63.01 g/mol. The moles corresponding to 6.40 g are:
6.40 g × (1 mol/63.01 g) = 0.102 mol
The molar ratio of NO₂ to HNO₃ is 3:2. The reacting moles of NO₂ are:
0.102 mol HNO₃ × (3 mol NO₂/2 mol HNO₃) = 0.153 mol NO₂
The molar mass of NO₂ is 46.01 g/mol. The mass corresponding to 0.153 moles is:
0.153 mol × (46.01 g/mol) = 7.04 g
During the light reactions
Answer : The assumptions appears reasonable for the isothermal process is,
and ![\Delta H=0](https://tex.z-dn.net/?f=%5CDelta%20H%3D0)
Explanation :
First law of thermodynamic : It states that the energy can not be created or destroyed, it can only change or transfer from one state to another state.
As per first law of thermodynamic,
![\Delta U=q+w](https://tex.z-dn.net/?f=%5CDelta%20U%3Dq%2Bw)
The expression for internal energy is:
![\Delta U=nC_vdt](https://tex.z-dn.net/?f=%5CDelta%20U%3DnC_vdt)
The expression for enthalpy is:
![\Delta H=nC_pdt](https://tex.z-dn.net/?f=%5CDelta%20H%3DnC_pdt)
where,
= internal energy
q = heat
w = work done
n = number of moles
= specific heat capacity at constant volume
= specific heat capacity at constant pressure
= change in temperature
As we know that, the term internal energy and enthalpy is the depend on the temperature and the process is isothermal that means at constant temperature.
T = constant
= 0
So, at constant temperature the internal energy and enthalpy is equal to zero. That means,
and ![\Delta H=0](https://tex.z-dn.net/?f=%5CDelta%20H%3D0)
Answer: The species oxidized is
.
The species reduced is ![Hg^{2+}](https://tex.z-dn.net/?f=Hg%5E%7B2%2B%7D)
The oxidizing agent is ![Hg^{2+}](https://tex.z-dn.net/?f=Hg%5E%7B2%2B%7D)
The reducing agent is ![I^-](https://tex.z-dn.net/?f=I%5E-)
Explanation:
Oxidation reaction is defined as the reaction in which a substance looses its electrons. The oxidation state of the substance increases.
Reduction reaction is defined as the reaction in which a substance gains electrons. The oxidation state of the substance gets reduced.
![Hg^{2+}+2I^-\rightarrow Hg+I_2](https://tex.z-dn.net/?f=Hg%5E%7B2%2B%7D%2B2I%5E-%5Crightarrow%20Hg%2BI_2)
On reactant side:
Oxidation state of mercury = +2
Oxidation state of iodine = -1
On product side:
Oxidation state of mercury = 0
Oxidation state of iodine = 0
The oxidation state of mercury reduces from +2 to 0, it is getting reduced. Thus, it is getting reduced and acts as oxidizing agent.
The oxidation state of iodine increases from -1 to 0. Thus, it is getting oxidized and acts as reducing agent .
Answer:
Mg + 2CuNO3 -----> Mg(NO3)2 + 2Cu