Answer:
0.903 A
Explanation:
We have given mass of Sn = 1 gram
Time t=30 minutes=30×60=1800 sec
According to Faraday law m=zit
Where z is electron chemical equivalent
z is calculated by 
where n is number of element and F is Faraday constant
So 
So 
i =0.903 A
Answer:
Explanation:PRESSURE: atmospheres or mm Hg; 1 atm = 760 mm Hg
TEMPERATURE: Kelvin, K, which is o
C + 273
STP: Standard Temperature and Pressure: 273 K and 1 atm (or 760 mm Hg)
BOYLE'S LAW (temperature is constant): PV = constant
This is an inverse relationship: if one variable increases the other must
decrease.
CHARLES' LAW (pressure is constant): V = constant x T
This is a direct relationship: if one variable increases so does the other.
GAY-LUSSAC'S LAW (volume is constant): P = constant x T
This is a direct relationship: if one variable increases so does the other.
<h2>Every one of this with the constant</h2>
Answer:
The molecules absorb heat and acquire more kinetic energy.
Explanation:
In a solid, the solids only vibrate about their mean positions but do not translate. When energy is supplied to the molecule in the form of heat, the molecules vibrate faster. Eventually, they acquire sufficient energy to leave their mean positions and translate. Hence the solid crystal collapses.
When ice is heated, water molecules acquire sufficient kinetic energy to translate. The intermolecular bonds are gradually broken in the solid framework as heat is absorbed. The heat required for this is known as the latent heat of fusion.
The temperature remains constant until phase transition is over, then temperature rise resumes.
Answer:
Explanation:
13 ) symbol of enthalpy change = Δ H .
14 ) enthalpy change is nothing but heat absorbed or evolved .
During fusion enthalpy change
Δ H .= m Lf , m is mass and Ls is latent heat of fusion
During evaporation, enthalpy change
Δ H .= m Lv , m is mass and Lv is latent heat of evaporation
during temperature rise , enthalpy change
Δ H = m c Δ T
In case of gas , enthalpy change can be calculated by the following relation
Δ H = Δ E + W , Δ E is change in internal energy , W is work done by gas.
15 ) When enthalpy change is negative , that means heat is released to the environment .So reaction is called exothermic .
when heat is absorbed enthalpy change is positive . Reaction is endothermic.
Complete question:
ΔU for a van der Waals gas increases by 475 J in an expansion process, and the magnitude of w is 93.0 J. calculate the magnitude of q for the process.
Answer:
The magnitude of q for the process 568 J.
Explanation:
Given;
change in internal energy of the gas, ΔU = 475 J
work done by the gas, w = 93 J
heat added to the system, = q
During gas expansion process, heat is added to the gas.
Apply the first law of thermodynamic to determine the magnitude of heat added to the gas.
ΔU = q - w
q = ΔU + w
q = 475 J + 93 J
q = 568 J
Therefore, the magnitude of q for the process 568 J.
