<u>Answer:</u> The specific heat of metal is 2.34 J/g°C
<u>Explanation:</u>
To calculate the mass of water, we use the equation:
Density of water = 1 g/mL
Volume of water = 35 mL
Putting values in above equation, we get:
When metal is dipped in water, the amount of heat released by metal will be equal to the amount of heat absorbed by water.
The equation used to calculate heat released or absorbed follows:
![m_1\times c_1\times (T_{final}-T_1)=-[m_2\times c_2\times (T_{final}-T_2)]](https://tex.z-dn.net/?f=m_1%5Ctimes%20c_1%5Ctimes%20%28T_%7Bfinal%7D-T_1%29%3D-%5Bm_2%5Ctimes%20c_2%5Ctimes%20%28T_%7Bfinal%7D-T_2%29%5D)
......(1)
where,
q = heat absorbed or released
= mass of metal = 4.82 g
= mass of water = 35 g
= final temperature = 34.5°C
= initial temperature of metal = 115°C
= initial temperature of water = 28.7°C
= specific heat of metal = ?
= specific heat of water = 4.186 J/g°C
Putting values in equation 1, we get:
![4.82\times c_1\times (34.5-110)=-[35\times 4.186\times (34.5-28.7)]](https://tex.z-dn.net/?f=4.82%5Ctimes%20c_1%5Ctimes%20%2834.5-110%29%3D-%5B35%5Ctimes%204.186%5Ctimes%20%2834.5-28.7%29%5D)
Hence, the specific heat of metal is 2.34 J/g°C
It's 2, glass. Water, nitrogen, and sucrose don;t have a crystalline structure.
Answer:
C is the element thats has been oxidized.
Explanation:
MnO₄⁻ (aq) + H₂C₂O₄ (aq) → Mn²⁺ (aq) + CO₂(g)
This is a reaction where the manganese from the permanganate, it's reduced to Mn²⁺.
In the oxalic acid, this are the oxidation states:
H: +1
C: +3
O: -2
In the product side, in CO₂ the oxidation states are:
C: +4
O: -2
Carbon from the oxalate has increased the oxidation state, so it has been oxidized.
Answer : The enthalpy change for the reaction is, 201.9 kJ
Explanation :
According to Hess’s law of constant heat summation, the heat absorbed or evolved in a given chemical equation is the same whether the process occurs in one step or several steps.
According to this law, the chemical equation can be treated as ordinary algebraic expression and can be added or subtracted to yield the required equation. That means the enthalpy change of the overall reaction is the sum of the enthalpy changes of the intermediate reactions.
The balanced reaction of 
will be,
The intermediate balanced chemical reaction will be,
(1) 
(2) 
(3) 
(4) 
Now we will multiply the reaction 1 by 2, revere the reaction 2, reverse and half the reaction 3 and 4 then adding all the equations, we get :
(1) 
(2) 
(3) 
(4) 
The expression for enthalpy of the reaction will be,
Therefore, the enthalpy change for the reaction is, 201.9 kJ
