<p>Ch100: Fundamentals for Chemistry 1 Moles Worksheet 4/29/2018</p><p>1. You have a 26.98 g piece of aluminum. a) How many moles are in 26.98 g of Al?</p><p> b) How many atoms are in 26.98 g of Al?</p><p> c) How many moles are in 5.00 g of Al?</p><p> d) How many atoms are in 5.00 g of Al?</p><p>2. You have a 20.00 g sample of chlorine gas.</p><p> a) How many moles of Cl2 are in the 20.00 g sample?</p><p> b) How many molecules are in 20.00 g of Cl2?</p><p> c) How many Cl atoms are in 20.00 g of Cl2?</p><p> d) How many moles of Cl2 are in a 5.00 g sample?</p><p> e) How many molecules of Cl2 are in 5.00 g? Ch100: Fundamentals for Chemistry 2 Moles Worksheet 4/29/2018</p><p>3. You have a sample containing 10.00 g of AlCl3?</p><p> a) What is the molecular mass of AlCl3?</p><p> b) How many moles of AlCl3 are in the sample?</p><p> c) How many moles of Al3+ are in the sample?</p><p> d) How many moles of Cl- are in the sample?</p><p> e) How many grams of Al3+ are in the sample?</p><p> f) How many grams of Cl- are in the sample?</p><p>4. You dissolve 25.00 g of AlCl3 in 1.0 L of de-ionized H2O.</p><p> a) How many moles of AlCl3 are dissolved?</p><p> b) How many molecules of AlCl3 are dissolved?</p><p> c) Using the information above, calculate how much volume of this solution you would </p><p> need to get 5.00 g of AlCl3. Ch100: Fundamentals for Chemistry 3 Moles Worksheet 4/29/2018</p><p>5. You have a flask containing 150. g of H2O (volume is 150. mL).</p><p> a) How many moles of H2O are in 150. g?</p><p> b) How many molecules of H2O are 150. g?</p><p> c) What is the mass percent of H and O, respectively, in H2O?</p><p> d) How much water (in grams) is needed to have obtain 10.0 grams of oxygen?</p><p>6. In the chemistry lab, you produce 10.0 grams of hydrogen gas from the following chemical reaction:</p><p>2HCl (aq) + Zn (s)  H2 (g) + ZnCl2 (aq)</p><p> a) What is the molar mass of H2?</p><p> b) How many moles of H2 are in 10.0 g?</p><p> c) How many moles of Zn are needed to produce 10.0 g of H2?</p><p> d) How many grams of Zn are needed to produce the 10.0 g of H2? Ch100: Fundamentals for Chemistry 4 Moles Worksheet 4/29/2018</p><p>7. Nuclear Chemistry: Nuclear Fusion During a nuclear fusion reaction, 2 nuclei combine to form the larger nucleus of a larger atom; in the process a large amount of heat energy is released. Consider the fusion of hydrogen-1, 1H to form helium-4 (4He), beta particles (+) and gamma photons (): 4 1H  4He + 2 + + 2  a) Calculate the mass of the four hydrogen 1 atoms.</p><p> b) Calculate the total mass of the helium-4 atom and the beta particles. Notes: 1) gamma photons are electromagnetic energy and do not have mass; and 2) beta particles have the same mass as electrons.</p><p> c) Calculate the mass deficit (m) between the reactants (a) and the products (b). This is the lost mass that is released as energy!</p><p> d) According to Einstein’s famous equation, E = (m)c2, where c = 2.998 x 108 m/s (the speed of light in vacuum) and m is the mass deficit (lost mass) during the reaction. Calculate the energy equivalent (in Joules) for the mass deficit in this nuclear fusion reaction; this is the amount of energy released by this nuclear process.</p><p> e) Convert the energy from Joules to calories.</p><p> f) Calculate the energy released per mole of helium-4 produced during this process.</p><p> g) If 1.00 mole of helium-4 is produced by this process, how many grams is it? </p>