Respuesta :
Answer:
Gas B has the higher initial temperature
6,199 J
7,008 J
Explanation:
Mathematically;
The thermal energy of a gas is given by:
E = 3/2 n kT
Where n is the number of moles, K is the molar gas constant and T is the temperature
For Gas A;
4700 = 1.5 * 2.3 * 8.31 * T
T = 4700/28.6695
Thus, T = 163.94 K
For gas B
8500 = 1.5 * 2.6 * 8.31 * T
T = 8500/32.409
T = 262.27 K
This means that gas B has a higher temperature than gas A.
At equilibrium, temperature
T = naTa + nbTb / (na + nb )
T = [2.3(163.94) + 2.6(262.27)]/(2.3 + 2.6)
T = [377.062 + 681.902]/4.9 = 216.12 K
216.12 K is the equilibrium temperature
= 216.12 K is the equilibrium temperature.
Thus, final thermal energy of Gas A and B
Gas A = 1.5 * 2.3 * 8.314 * 216.12= 6,199 J
Gas B = 1.5 * 2.6 * 8.314 * 216.12 = 7,008 J
The gas that possesses a higher Initial temperature would be:
- Gas B
1). The final thermal energy of gas A would be:
[tex]6,199 J[/tex]
2). The final thermal energy of gas B would be:
[tex]7,008 J[/tex]
Gas A
Given that,
Number of moles [tex]= 2.3 mol[/tex]
Initial Thermal Energy [tex]= 4700 J[/tex]
We can determine T by using
[tex]E = 3/2 n kT[/tex]
with [tex]K[/tex] being constant of molar gas,
[tex]n[/tex] [tex]= number [/tex] [tex]of [/tex] [tex]moles[/tex]
[tex]T = temperature[/tex]
so,
[tex]T = 4700/(1.5 * 2.3 * 8.31k)[/tex]
∵ [tex]T = 163.94 K[/tex]
Gas B
Given that,
Number of moles [tex]= 2.6 mol[/tex]
Initial thermal energy [tex]= 8500 J[/tex]
[tex]T = 8500/(1.5 * 2.6 * 8.31 * T)[/tex]
∵ [tex]T = 262.27 K[/tex]
Thus, gas B has a higher temperature.
To determine final thermal energy, the equilibrium temperature would be determined:
[tex]T = naTa + nbTb / (na + nb )[/tex]
[tex]T = [2.3(163.94) + 2.6(262.27)]/(2.3 + 2.6)[/tex]
∵ [tex]T = 216.12 K[/tex]
1). Final thermal energy of gas A
[tex]= 1.5 * 2.3 * 8.314 * 216.12[/tex]
[tex]= 6,199 J[/tex]
2). Final thermal energy of gas B
[tex]= 1.5 * 2.6 * 8.314 * 216.12[/tex]
[tex]= 7,008 J[/tex]
Learn more about "Thermal Energy" here:
brainly.com/question/16961806
