Answer:
1900 °C
Step-by-step explanation:
This looks like a case where we can use the <em>Combined Gas Law</em> to calculate the temperature.
p₁V₁/T₁ = p₂V₂/T₂ Multiply both sides by T₂
p₁V₁T₂/T₁ = p₂V₂ Multiply each side by T₁
p₁V₁T₂ = p₂V₂T₁ Divide each side by p₁V₁
T₂ = T₁ × p₂/p₁ × V₂/V₁
=====
Data:
We must convert the pressures to a common unit. I have chosen atmospheres.
p₁ = 675 mmHg × 1atm/760 mmHg = 0.8882 atm
V₁ = 718 mL = 0.718 L
T₁ = 48 °C = 321.15 K
p₂ = 159 kPa × 1 atm/101.325 kPa = 1.569 atm
V₂ = 2.0 L
T₂ = ?
=====
Calculation:
T₂ = 321.15 × 1.569/0.8882 × 2.0/0.718
T₂ = 321.15 × 1.766 × 2.786
T₂ = 321.15 × 1.569/0.8882 × 7.786
T₂ = 1580K
T₂ = 1580 + 273.15
T₂ = 1900 °C
<em>Note</em>: The answer can have only <em>two</em> significant figures because that is all you gave for the second volume of the gas.
Answer:
O2+H2 → H2O
become→zero to−2
∵ it will be reduced and oxidation state of H
2
becomes zero to +1 it will be oxidised.
∴ reaction will be redox
Explanation:
please mark me as brainalist
Answer:
When you heat ice, the individual molecules gain kinetic energy, but until the temperature reaches the melting point, they don't have energy to break the bonds that hold them in a crystal structure. They vibrate more quickly within their confines as you add heat, and the temperature of the ice goes up.
Nuclear binding energy is the energy that would be required to disassemble the nucleus of an atom into its component parts. These component parts are netrons and protons, which are collectively called nucleons
Explanation:
The given data is as follows.
T = 298 K, 
= -5645 kJ/mol
= -5798 kJ/mol
Relation between 
and 
are as follows.
= 
-5798 kJ/mol = -5645 kJ/mol - 
-153 kJ/mol = -
= 0.513 kJ/mol K
Now, temperature is 
= (37 + 273) K = 310 K
Since, =
= 
= (-5645 kJ/mol - 159.03 kJ/mol)
= -5804.03 kJ/mol
As, change in Gibb's free energy = maximum non-expansion work
= -5804.03 kJ/mol - (-5798 kJ/mol)
= -6.03 kJ/mol
Therefore, we can conclude that the additional non-expansion work is -6.03 kJ/mol.
