The reaction of the alloy with the acid is exothermic. If the hydrogen gas released is...

The reaction of the alloy with the acid is exothermic. If the hydrogen gas released is warmer than the water temperature and you use the incorrect low temperature, how would this effect your calculated %Al result (high or low)? Explain.

A student performs three runs of the experiment using pure aluminum and determines an average N_H2 of 0.01156 mol/g and a standard deviation of 0.00001 mol/g. What do these results tell you about the random and systematic errors present in his analysis?

Expert Solution

Reaction of alloy containing aluminium with the acid is an exothermic reaction.

If the hydrogen gas released is warmer than the water temperature and we use the incorrect low temperature.

This error would result in higher %Al calculated as the temperature is inversely proportional to the moles of aluminium and hence the mass of aluminium.

When a student perfoms three runs of the experiment, using pure aluminium and determines average NH2 of 0.01156 mol/g with a standard deviation of 0.000001 mol/g.

This result tells us that we are working with systematic error in the experiment which gives us a low standard deviation for the given experiment.

queen_honey_blossom answered 2 years ago

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