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Answer :
The molar mass of the gas is approximately 184.3 g/mol.
To find the molar mass of the gas, we can use the ideal gas law equation: PV = nRT. Where: P = pressure (in atm)
V = volume (in liters)
n = number of moles
R = ideal gas constant (0.0821 L·atm/(mol·K))
T = temperature (in Kelvin)
First, we need to convert the given temperature from Celsius to Kelvin:
T(K) = T(°C) + 273.15. T = 25°C + 273.15 = 298.15 K. Next, let's rearrange the ideal gas law equation to solve for the number of moles: n = PV / RT Plugging in the values:
P = 1.54 atm
V = 2.92 L
R = 0.0821 L·atm/(mol·K)
T = 298.15 K
n = (1.54 atm * 2.92 L) / (0.0821 L·atm/(mol·K) * 298.15 K)
Calculating the expression: n = 0.197 mol. Now, we can find the molar mass (M) of the gas by dividing the mass (m) by the number of moles (n):
M = m / n M = 36.3 g / 0.197 mol Calculating the expression: M ≈ 184.3 g/mol Therefore, the molar mass of the gas is approximately 184.3 g/mol.
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