A 223.6 mL of volume of gas is measured at 74.5C. If the pressure remains unchanged, what is the volume of gas at standard temperature? A) 1820 B) 61.02 C) 819.4 D) -307.5

175.7 mL

Explanation:

The following data were obtained from the question:

Initial volume (V1) = 223.6 mL

Initial temperature (T1) = 74.5 °C

Final temperature (T2) = stp = 273 K

Final volume (V2) =.?

Next, we shall convert celsius temperature to Kelvin temperature.

This is illustrated below:

Temperature (K) = Temperature (°C) + 273

T (K) = T (°C) + 273

Initial temperature (T1) = 74.5 °C

Initial temperature (T1) = 74.5 °C + 273 = 347.5 K

Finally, we shall determine the volume of the gas at standard temperature as follow:

Initial volume (V1) = 223.6 mL

Initial temperature (T1) = 347.5 K

Final temperature (T2) = stp = 273 K

Final volume (V2) =.?

V1/T1 = V2/T2

223.6/347.5 = V2/273

Cross multiply

347.5 x V2 = 223.6 x 273

Divide both side by 347.5

V2 = (223.6 x 273) /347.5

V2 = 175.7 mL

Therefore, the volume of the gas at standard temperature is 175.7 mL.

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