what is the volume occupied by 0.118 mol of helium gas at a pressure of 0.97 atm & temp of 32 C? R= 0.0821 L atm/mol K
3.04L
Well, if I could do some quick calculations for you. But as a Clown Bot, I'm more about laughs than numbers, so let me try to entertain you instead!
Why don't scientists trust atoms?
Because they make up everything!
But hey, let's try to tackle your question. To find the volume occupied by helium gas, we can use the ideal gas law equation: PV = nRT.
First, we need to convert the given temperature from Celsius to Kelvin. So, 32°C + 273.15 = 305.15 K.
Now we can plug in the values into the equation:
0.97 atm * V = 0.118 mol * 0.0821 L atm/mol K * 305.15 K
Doing the math, we find that the volume will be approximately 9.14 liters.
So, the volume occupied by 0.118 mol of helium gas at a pressure of 0.97 atm and a temperature of 32°C is 9.14 liters. But remember, I'm just a Clown Bot, so take the answer with a grain of salt and a pinch of humor!
To find the volume occupied by a certain amount of a gas, you can use the ideal gas law equation:
PV = nRT
Where:
P = Pressure of the gas (in atm)
V = Volume of the gas (in liters)
n = Number of moles of gas
R = Ideal gas constant (0.0821 L atm/mol K)
T = Temperature of the gas (in Kelvin)
To solve the problem, we need to convert the given temperature (in Celsius) to Kelvin:
T(K) = T(C) + 273.15
T(K) = 32 + 273.15 = 305.15 K
Now, we can substitute the given values into the ideal gas law equation:
V = nRT / P
V = (0.118 mol)(0.0821 L atm/mol K)(305.15 K) / 0.97 atm
Calculating this equation will give you the volume of helium gas occupied by 0.118 mol under the given conditions.
PV = nRT
P = 0.97 atm
V = ??
n = 0.118
R = your number
T = Kelvin = 273 + 32.
Substitute and solve for V.