How would I determine the formula of butane as they ask in question #7? I've found that the molar mass of butane gas is 0.574 g/mol by dividing the mass of butane (0.1027 g) by the number of moles of butane (0.179 mol).

In chemistry, what is meant by the term mole? What is the importance of the mole concept?

Uranium is used as a fuel, primarily in the form of uranium(IV) oxide, in nuclear power plants. This question considers some uranium chemistry. (a) A small sample of uranium metal (0.169 g) is heated to between 800 and 900 C in air to give 0.199 g of a dark green oxide, UxOy How many moles of uranium metal were used? What is the empirical formula of the oxide, UxOy? What is the name of the oxide? How many moles of UxOy must have been obtained? (b) The naturally occurring isotopes of uranium are 234U, 235U, and 238U. Knowing that uraniums atomic weight is 238.02 g/mol, which isotope must be the most abundant? (c) If the hydrated compound UO2(NO3)2 z H2O is heated gently, the water of hydration is lost. If you have 0.865 g of the hydrated compound and obtain 0.679 g of UO2(NO3)2 on heating, how many waters of hydration are in each formula unit of the original compound? (The oxide Ux, Oy is obtained if the hydrate is heated to temperatures over 800C in the air.)

Give the name and value of the number associated with the mole.

Is there a difference between a homogeneous mixture of hydrogen and oxygen in a 2:1 mole ratio and a sample of water vapor? Explain.

Without using a calculator, which has the greater mass: One mole of carbon atoms or one mole of chlorine atoms? Explain your reasoning. What is the benefit of using moles when working with atoms and molecules in a lab setting? How does this relate to the concept of molarity?

Consider a sample of carbon tetrafluoride that contains 1.09 × 10²⁴ atoms of fluorine. 1.) Using the formula CF₄, how many moles of fluorine are present? 2.) Determine how many moles of carbon tetrafluoride are present 3.) Determine the molar mass of carbon tetrafluoride. 4.) What is the mass in grams of carbon tetrafluoride that are present?

A sample of NH3 has a mass of 84.06 grams.   Calculate the moles of NH3 in the sample.   Calculate the number of NH3 molecules in the sample.   Calculate the moles of H in the sample.