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At what temperature (in Celsius) will 0.0705 moles of Chlorine gas (Cl2) exert a pressure of 1.19 atm at a volume of 0.750L?

a) 45.6°C
b) 56.3°C
c) 34.8°C
d) 62.1°C

1 Answer

2 votes

Final answer:

Using the Ideal Gas Law and given values, the temperature was calculated to be -118.932°C after converting from Kelvin to Celsius, which does not match any of the provided options, suggesting there might be an error in the question or calculations.

Step-by-step explanation:

To find the temperature at which 0.0705 moles of Chlorine gas (Cl2) exert a pressure of 1.19 atm at a volume of 0.750L, we can use the Ideal Gas Law which is PV = nRT, where P is pressure, V is volume, n is moles of gas, R is the gas constant, and T is temperature in Kelvin.

First, rearrange the Ideal Gas Law to solve for T (Temperature):
T = PV/(nR).

Plugging in the known values we get T = (1.19 atm)(0.750 L) / (0.0705 moles)(0.0821 L*atm/mol*K). Please note that R (the ideal gas constant) is 0.0821 L*atm/mol*K.

After solving, convert the temperature from Kelvin to Celsius by subtracting 273.15 from the Kelvin temperature.

Now we'll plug in the values and calculate:
T = (1.19 atm * 0.750 L) / (0.0705 moles * 0.0821 L*atm/mol*K) = (0.8925 L*atm) / (0.00578805 mol*K) = 154.218 K.
Converting to Celsius: 154.218 K - 273.15 = -118.932 °C. This temperature is not listed in the provided options, indicating there may have been a mistake either in the question setup or the calculation.

User Mbernasocchi
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