determine the pressure in a 0.34 liter balloon if the temperature is 35 celsius and the balloon contains 0.0233 mol of an ideal gas.
PV = nRT
Remember T must be in kelvin.
To determine the pressure in the balloon, we can use the ideal gas law equation:
PV = nRT
Where:
P = pressure in atmospheres (atm)
V = volume in liters (L)
n = number of moles of gas
R = ideal gas constant (0.0821 L*atm/(mol*K))
T = temperature in Kelvin (K)
First, we need to convert the temperature from Celsius to Kelvin:
T(K) = T(C) + 273.15
T(K) = 35 + 273.15 = 308.15 K
Now we can substitute the given values into the ideal gas law equation:
PV = nRT
P * 0.34 = 0.0233 * 0.0821 * 308.15
P * 0.34 = 0.0612
Divide both sides of the equation by 0.34 to solve for P:
P = 0.0612 / 0.34
P ≈ 0.18 atm
Therefore, the pressure in the 0.34 liter balloon is approximately 0.18 atm.
To determine the pressure in the balloon, we can use the Ideal Gas Law equation, which states:
PV = nRT
Where:
P is the pressure (in atmospheres),
V is the volume (in liters),
n is the number of moles of the gas,
R is the ideal gas constant (0.0821 L·atm/(mol·K)),
T is the temperature (in Kelvin).
First, we need to convert the temperature from Celsius to Kelvin. The Kelvin scale is obtained by adding 273.15 to the Celsius temperature. So, 35°C + 273.15 = 308.15 K.
Now, we can substitute the given values into the Ideal Gas Law equation:
P * 0.34 L = 0.0233 mol * 0.0821 L·atm/(mol·K) * 308.15 K
Simplifying the equation:
P * 0.34 L = 0.0233 mol * 25.37 L·atm/(mol·K)
Dividing both sides by 0.34 L:
P = (0.0233 mol * 25.37 L·atm/(mol·K)) / 0.34 L
P ≈ 1.738 atm
Therefore, the pressure in the balloon is approximately 1.738 atmospheres.