2. Magnesium nitride can be prepared by the direct reaction of the elements, as shown by the equation Mg(s) + N2(g) → Mg3N2(s) How many grams of magnesium nitride can be produced from the following amounts of reactants? a. 10.0 g of Mg and 10.0 g of N2 b. 20.0 g of Mg and 10.0 g of N2 c. 30.0 g of Mg and 10.0 g of N2 С.

2. Magnesium nitride can be prepared by the direct reaction of the elements, as shown by the equation Mg(s) + N2(g) → Mg3N2(s) How many grams of magnesium nitride can be produced from the following amounts of reactants? a. 10.0 g of Mg and 10.0 g of N2 b. 20.0 g of Mg and 10.0 g of N2 c. 30.0 g of Mg and 10.0 g of N2 С.

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter3: Stoichiometry

Section: Chapter Questions

Problem 124E: DDT, an insecticide harmful to fish, birds, and humans, is produced by the following reaction: In a...

See similar textbooks

Similar questions

DDT, an insecticide harmful to fish, birds, and humans, is produced by the following reaction: In a government lab, 1142 g of chlorobenzene is reacted with 485 g of chloral. a. What mass of DDT is formed, assuming 100% yield? b. Which reactant is limiting? Which is in excess? c. What mass of the excess reactant is left over? d. If the actual yield of DDT is 200.0 g, what is the percent yield?
3.81 The particulate scale drawing shown depicts the products of a reaction between H2 and O2 molecules. (a) Draw a similar representation for the reactants that must have been present before the reaction took place. (b) Write a balanced chemical equation for the reaction, using the smallest possible whole number coefficients.
One way to remove nitrogen oxide (NO) from smoke-stack emissions is to react it with ammonia. 4NH3(g)+6NO(g)5N2(g)+6H2O(l) Calculate (a) the mass of water produced from 0.839 mol of ammonia. (b) the mass of NO required to react with 3.402 mol of ammonia. (c) the mass of ammonia required to produce 12.0 g of nitrogen gas. (d) the mass of ammonia required to react with 115 g of NO.
In an experiment designed to produce calcium oxide by the chemical reaction 2Ca + O2 2CaO 177.2 g of CaO was obtained out of a possible 203.9 g ofCaO. a. What is the theoretical yield of CaO? b. What is the actual yield of CaO? c. What is the percent yield of CaO?
Citric acid (C6H8O7) is made by fermentation of sugarssuch as sucrose (C12H22O11) in air. Oxygen is consumedand water generated as a by-product. (a) Write a balanced equation for the overall reaction thatoccurs in the manufacture of citric acid from sucrose. (b) What mass of citric acid is made from 15.0 kg sucrose?
If baking soda (sodium hydrogen carbonate) is heated strongly, the following reaction occurs: :math>2NaHCO3(s)Na2CO3(s)+H2O(g)+CO2(g) lculate the mass of sodium carbonate that will remain if a 1.52-g sample of sodium hydrogen carbonate is heated.
Methanol, CH3OH, can be prepared from carbon monoxide and hydrogen. CO(g) + 2 H2(g) CH3OH(l) What mass of hydrogen is required to produce 1.0 L of CH3OH (d = 0.791 g/mL) if this reaction has a 74% yield under certain conditions?
You have seven closed containers, each with equal masses of chlorine gas (Cl2) . You add 10.0 g of sodium to the first sample, 20.0 g of sodium to the second sample, and so on (adding 70.0 g of sodium to the seventh sample). Sodium and chlorine react to form sodium chloride according to the equation 2Na(s)+Cl22NaCl(s) After each reaction is complete, you collect and measure the amount of sodium chloride formed. A graph of your results is shown below. Answer the following questions: a. Explain the shape of the graph. b. Calculate the mass of NaCl formed when 20.0 g of sodium is used. c. Calculate the mass of Cl2 in each container. d. Calculate the mass of NaCl formed when 50.0 g of sodium is used. e. Identify the leftover reactant, and determine its mass for parts b and d above.
ou know that chemical A reacts with chemical B. You react 10.0 g A with 10.0 g B. What information do you need to know to determine the amount of product that will be produced? Explain.
Determine the number of moles of compound and the number of moles of each type of atom in each of the following: 25.0 g of propylene, C3H6 3.06103 g of the amino acid glycine, C2H5NO2 25 lb of the herbicide Treflan, C13H16N2O4F (1 lb = 454 g) 0.125 kg of the insecticide Paris Green, Cu4(AsO3)2( CH3 CO2)2 325 mg of aspirin, C6H4(CO2H)(CO2CH3)
Write the balanced chemical equation for the complete combustion of heptene, C7H14. In combustion, hcpLcnc reacts with oxygen to produce carbon dioxide and water. What is the mole ratio that would enable you to calculate the number of moles of oxygen needed to react exactly with a given number of moles of heptene? What mole ratios would you use to calculate how many moles of each product form from a given number of moles of heptene?