Respuesta :
Answer:
a) 1:1
Explanation:
By the ideal gas law:
PV = nRT
Where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is temperature.
Both ballons are at the same conditions, so the gases have the same temperature and pressure. The number of moles is the mass(m) divided by the molar mass (Mr). The molar masses are:
Mr(Ne) = 20 g/mol
Mr(Ar) = 40 g/mol
Calling 1 for Ne, and 2 for Ar:
P1*V1 = (m1/20)*R*T1
m1 = 20P1V1/RT1
P2*V2 = (m2/40)*R*T2
m2 = 40P2V2/RT2
V1 = 2V2
m1/m2 = (20P1V1/RT1)/(40P21V2/RT2)
P1 = P2, T1 =T2 so they can be canceled, such as the R:
m1/m2 = 20V1/40V2
m1/m2 = 20*2V2/40V2
m1/m2 = 40V2/40V2
m1/m2 = 1/1
m1:m2 = 1:1
The mass ratio of Ne:Ar in the balloons is:
a) 1:1
Ideal gas law:
PV = nRT
where,
- P is the pressure,
- V is the volume,
- n is the number of moles,
- R is the gas constant, and
- T is temperature.
The gases will have same pressure and temperature since both balloons are under same conditions,
The number of moles is the mass divided by the molar mass. The molar masses are:
M(Ne) = 20 g/mol
M(Ar) = 40 g/mol
We are taking 1 for Ne and 2 for Ar.
[tex]P_1*V_1 = (m_1/20)*R*T_1\\\\m_1 = 20*P_1V_1/RT_1[/tex]....................(1)
[tex]P_2*V_2 = (m_2/40)*R*T_2\\\\m_2 = 40P_2V_2/RT_2[/tex]...................(2)
Given: The orange balloon has twice the volume of the blue balloon.
Thus, [tex]V_1 = 2V_2[/tex]
Dividing equation 1 by 2:
[tex]\frac{m_1}{m_2} = \frac{(20P_1V_1/RT_1)}{(40P_2V_2/RT_2)}[/tex]
Since, the balloons are under same conditions.
Thus
[tex]\frac{m_1}{m_2} = \frac{20V_1}{40V_2}\\\\\frac{m_1}{m_2} = \frac{20*2V_2}{40V_2}\\\\\frac{m_1}{m_2} = \frac{40V_2}{40V_2}\\\\\frac{m_1}{m_2} = \frac{1}{1}\\\\m_1:m_2=1:1[/tex]
So, the mass ratio of Ne: Ar in the balloons is: 1:1.
Thus, correct option is a.
Find more information about Ideal gas here:
brainly.com/question/25290815
