I have a few questions. 1. Suppose the thermometer is miscalibrated to read 0.3

Question

I have a few questions.

1. Suppose the thermometer is miscalibrated to read 0.3 oC higher than actual. Does this error in calibration result in the molar mass of the vapor in the flask being reported as too high or too low or as unaffected? Explain.

2. If the volume of the flask is assumed to be 125mL instead of the measured volume, would the calculated molar mass of the unknown liquid be too high or too low or as unaffected by this experimental error? Explain.

3. The pressure reading from the barometer is recorded higher than it actually is. How does this affect the reported molar mass of the liquid: too high, too low, or unaffected? Exlplain.

Explanation / Answer

n = m/M where m is mass and M is molar mass PV = nRT = mRT/M M = mRT/PV 1. M is directly proportional to T. If T is low, that means that molar mass will be low, since they are directly related. 2. M = mRT/PV Need to know what the volume of the flask was, which is information you still haven't given. If V is bigger than 125, then M will be too high; if V is small than 125, then M will be too low. M is inversely related to V, so as V is reduced, M gets bigger, and as V increases, M gets smaller. 3. M = mRT/PV M is inversely proportional to P. If P is too high, then M will be too low.

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