What volume in liters does 0.136 g of O2 occupy at 20.0 degree C and 748 torr?
The number of moles in that sample can be first calculated using the molar mass of oxygen.
Now enter all of your values into the ideal gas law formula, remembering to convert to degrees Kelvin and torr to atm.
The response, rounded to three sig figs, is
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To find the volume of 0.136 g of O2 at 20.0°C and 748 torr, we can use the ideal gas law equation: PV = nRT.
First, we need to find the number of moles of O2 using its molar mass (32.00 g/mol).
n = mass / molar mass n = 0.136 g / 32.00 g/mol n ≈ 0.00425 mol
Next, we rearrange the ideal gas law equation to solve for volume (V):
V = nRT / P
Substitute the known values: n = 0.00425 mol R = 0.0821 L·atm/(K·mol) (the ideal gas constant) T = 20.0°C + 273.15 = 293.15 K P = 748 torr
V = (0.00425 mol) * (0.0821 L·atm/(K·mol)) * (293.15 K) / (748 torr)
Now, solve for V:
V ≈ 0.174 L
Therefore, 0.136 g of O2 occupies approximately 0.174 liters at 20.0°C and 748 torr.
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
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