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A 4.86 g quantity of solid rubidiummetal is combined with 3.44 g of magnesium chloride crystals according to this chemical reaction: 2 Rb (s) + 1 MgCl2 (s) 1Mg (s) +2 RbCI (s) What quantity of magnesium metal will be produced? _g Mg round your answer using appropriate sig figs The following molar masses may or may not be needed, but are provided to save you time: • molar mass: Rb = 85.47 g/mol • molar mass: MgCl2= 95.21 g/mol • molar mass: Mg = 24.31 g/mol Hiint: Start with the number of grams of Rubidium

Please write the chemical reaction exactly as described below. The products are one mole of liquid water, one mole of carbon dioxide gas, and two moles of aqueous potassium chloride. The reactants are one mole of solid potassium carbonate and two moles of aqueous hydrochloric acid. Use the editor to format your answer

A student needs to produce 19.09 grams of nitrogen gas (N2) for a lab experiment. How many grams of ammonia (NH3) will be required to produce this amount of nitrogen? Round your answer to the nearest 0.01 and remember to include units and substance! NH3 --> N2 + H2

Relate the model to Chemistry: The balanced chemical reaction for producing water is: 2 H2 + 1 O2 → 2 H2O. Predict which reactant amounts (of the three examples shown below) would get the most water with the least amount of leftovers. Explain how your understanding of Limiting Reactant helped you figure this out.

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13. Aluminum metal (Al) reacts with sulfur (S) to produce aluminum sulfide (ALS) according to this balanced chemical equation: 2 Al(s) + 3 S(s) → AlS(s) How many atoms of aluminum will react completely with 1.33 x 10 atoms of sulfur?

How many kilograms of C3H6 are needed along with an excess of ammonia to react with 1.31 x 103 g of O2 in the following reaction? Use the drop down menus in each section of the grid to select the best quantity to go in that section of the grid. Use the drop down menu in the answer box to select the best answer. 2 C3H6(g) + 2 NH3(g) + 3 O2(g) → 2 C3H3N(g) + 6 H20(g)

A materials scientist has created an alloy containing aluminum, copper, and zinc, and wants to determine the percent composition of the alloy. The scientist takes a 12.849 g sample of the alloy and reacts it with concentrated HCl. The reaction converts all of the aluminum and zinc in the alloy to aluminum chloride and zinc chloride in addition to producing hydrogen gas. The copper does not react with the HCl. Upon completion of the reaction, a total of 10.4 L of hydrogen gas was collected at a pressure of 724 torr and a temperature of 27.0 °C. Additionally, 2.836 g of unreacted copper is recovered. Calculate the mass of hydrogen gas formed from the reaction. mass: ----- g Calculate the mass of aluminum in the alloy sample. mass: ---- g What is the mass percent composition of the alloy? Cu: -----% Zn: ----% Al: -----%

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