Respuesta :
Answer : The correct option is, (A) 0.42 moles
Explanation :
Using ideal gas equation:
[tex]PV=nRT[/tex]
where,
P = pressure of gas = 125000 Pa = 125 kPa
conversion used : (1 kPa = 1000 Pa)
V = volume of gas = [tex]0.01m^3=10L[/tex]
conversion used : [tex](1m^3=1000L)[/tex]
T = temperature of gas = 357 K
n = number of moles of gaseous mixture = ?
R = gas constant = 8.314 kPa.L/mol.K
Now put all the given values in the ideal gas equation, we get:
[tex](125kPa)\times (10L)=n\times (8.314kPa.L/mol.K)\times (357K)[/tex]
[tex]n=0.42mole[/tex]
Therefore, the number of moles of an ideal gas is 0.42 mole.
The correct answer is A. 0.42 moles.
Further Explanation
The Ideal Gas Equation states the relationship among the pressure, temperature, volume, and number of moles of a gas.
The Ideal Gas Equation is:
where:
P - pressure (in Pa)
V - volume (in m³)
n - amount of gas (in moles)
R - universal gas constant (8.314 Pa·m³/mol·K)
T - temperature (in K)
In the problem, we are given the values:
P = 125,000 Pa (3 significant figures)
V =0.01 m³ (1 significant figure)
n = ?
T = 357 K (3 significant figures)
Solving for n using the Ideal Gas Equation:
[tex]PV = nRT[/tex][tex]n = \frac{PV}{RT}\\n = \frac{125,000 \ Pa \times 0.01 \ m^3}{8.314 \frac{Pa-m^3}{mol-K} \times 357 \ K}\\n = \frac{1250 \ Pa-m^3}{2968 \frac{Pa-m^3}{mol}}\\\\\boxed {n = 0.42116 \ mol}[/tex]
The least number of significant figures is 1, therefore, the final answer must have only 1 significant figure:
[tex]\boxed {\boxed {n = 0.4 \ mol}}[/tex]
Since this is not available, the closest answer is option A. 0.42 moles.
Learn More
1. Learn more about Boyle's Law brainly.com/question/1437490
2. Learn more about Charles' Law brainly.com/question/1421697
3. Learn more about Gay-Lussac's Law brainly.com/question/6534668
