What is the pressure of 0.8 moles of Neon gas that occupies a volume of 8.5 L at a temperature of 350 K. given R= 0.0821 L atm/ mol K. a 2.7 atm b 0.59 atm c 17.0 atm d 0.37 atm
To find the pressure, we can use the ideal gas law equation:
PV = nRT
where:
P = pressure
V = volume
n = moles
R = ideal gas constant
T = temperature
Plugging in the given values:
n = 0.8 moles
V = 8.5 L
T = 350 K
R = 0.0821 L atm/mol K
P(8.5) = (0.8)(0.0821)(350)
P = (0.8)(0.0821)(350) / 8.5
P ≈ 0.326 atm
Therefore, the pressure of 0.8 moles of Neon gas is approximately 0.37 atm (option d).
To find the pressure of the gas, we can use the ideal gas law equation: PV = nRT.
Where:
P = pressure
V = volume
n = number of moles
R = gas constant
T = temperature
We are given:
n = 0.8 moles
V = 8.5 L
T = 350 K
R = 0.0821 L atm/ mol K
Now, we can substitute the values into the ideal gas law equation and solve for P:
P * 8.5 = 0.8 * 0.0821 * 350
P * 8.5 = 22.772
P = 22.772 / 8.5
P ≈ 2.68 atm
Therefore, the pressure of the Neon gas is approximately 2.68 atm.
However, none of the provided answer options match this value exactly.
To find the pressure of a gas, we can use the ideal gas law equation:
PV = nRT
Where:
P = pressure
V = volume
n = number of moles
R = ideal gas constant
T = temperature in Kelvin
In this case, we are given the following values:
n = 0.8 moles
V = 8.5 L
T = 350 K
R = 0.0821 L atm/mol K
Now we can substitute these values into the equation and solve for P:
P * 8.5 = 0.8 * 0.0821 * 350
First, multiply 0.8 by 0.0821 and then multiply the product by 350. This will give you 22.856.
Now we divide both sides of the equation by 8.5 to solve for P:
P = 22.856 / 8.5
Solving this division gives you a value of approximately 2.689.
Rounding this answer to the nearest hundredth, the pressure of 0.8 moles of Neon gas in a volume of 8.5 L at a temperature of 350 K is approximately 2.69 atm.
Therefore, the correct answer choice from the provided options is a) 2.7 atm.