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You are asked to calibrate a 25 mL volumetric pipet. You determine that the temperature of your distilled water is exactly {T} degrees Celsius. You carefully determined the mass of a clean dry beaker and found that it was {m1} g. You pulled water up to the mark and transferred this to the beaker and found that the new mass was {m2} g. What is the actual volume of the pipet? The density of water at {T} degrees Celsius is {D} g/mL. Your answer should have 6 significant figures

You calibrated a volumetric pipet and determined its volume to be {v1} mL. You then use it to determine the density of an unknown liquid. You use a fresh clean dry beaker with an initial mass of {m1} g. You pull the unknown liquid up to the mark in the pipet and transfer this to the beaker. The new mass of the beaker and liquid is {m2} g. What is the density of the unknown liquid? Report 3 significant figures

1.68 x 1023 atoms of Ni represents how many grams (report 3 significant figures) _______ grams.

In the reaction  how many moles of ammonia (NH3) will be produced from 1.30 mol of hydrogen gas and excess nitrogen gas? (report 3 significant figures) _______ moles

The number 0.00003009 expressed in exponential notation is

A hydrocarbon has the formula C5H12. What is the percent by mass of carbon in the compound?

Elements that are in the same ________  have a tendency to have very similar properties .

When chlorine undergoes the reaction Cl ® Cl – , which of the following statements is true.

A compound has a molar mass of 42.0 g/mol and the emperical formula is CH2{“version”:”1.1″,”math”:”2″}. What is the molecular formula?

A 52.8 g gold nugget is dropped into a graduated cylinder containing 50.00 mL of water and the level of the water rises to 52.80 mL. What is the density of the gold? (use the correct number of significant figures) _______ g\mL