Where stated, classify reactions both by the key reaction event (PPT, A/B, R/O) and bychanges in composition (COM, DEC, SDP, DDP).5. _ Mg(N3)2(s) → _ M93N2(s) + _ N2(g)balance, then classify:-Calculate the following, with proper number of significant figures:When 0.057 moles of N2 form,moles of Mg;N2 form also.To make 92.0 moles of Mg3N2,moles of Mg(N3)2 need to react.To make 0.48 grams of N2,moles of Mg(N3)2 need to react.When 24.5 grams of Mg(N3)2 react,grams of M93N2 are made.To make a count of 5.62x1020 of Mg3N2 units,grams of Mg(N3)2 need to react.

Answered: Image /qna-images/answer/1b1589ed-3ee8-4913-bd58-5e55bf1616fc.jpg

Where stated, classify reactions both by the key reaction event (PPT, A/B, R/O) and by changes in composition (COM, DEC, SDP, DDP).| 5. Mg(N3)2(s) →– Mg3N2(s) + N2(g) balance, then classify: Calculate the following, with proper number of significant figures: When 0.057 moles of N2 form, moles of Mg3N2 form also. To make 92.0 moles of Mg3N2, moles of Mg(N3)2 need to react. To make 0.48 grams of N2, moles of Mg(N3)2 need to react. When 24.5 grams of Mg(N3)2 react, grams of Mg3N2 are made. To make a count of 5.62x1020 of Mg3N2 units, grams of Mg(N3)2 need to react.

Where stated, classify reactions both by the key reaction event (PPT, A/B, R/O) and by changes in composition (COM, DEC, SDP, DDP).| 5. Mg(N3)2(s) →– Mg3N2(s) + N2(g) balance, then classify: Calculate the following, with proper number of significant figures: When 0.057 moles of N2 form, moles of Mg3N2 form also. To make 92.0 moles of Mg3N2, moles of Mg(N3)2 need to react. To make 0.48 grams of N2, moles of Mg(N3)2 need to react. When 24.5 grams of Mg(N3)2 react, grams of Mg3N2 are made. To make a count of 5.62x1020 of Mg3N2 units, grams of Mg(N3)2 need to react.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

H2SO4(aq) + Pb(C2H3O2)2(aq) -> PbSO4(s) + 2 HC2H3O2(aq) Solutions of sulfuric acid and lead (II) acetate react to form solid lead (II) sulfate and a solution of acetic acid. If 11.7 g of sulfuric acid and 13.2 g of lead (II) acetate are mixed, calculate the number of grams of sulfuric acid, lead (II) acetate, lead (II) sulfate, and acetic acid present in the mixture after the reaction is complete. Which chemical is the limiting reactant? Select an answer How many grams of sulfuric acid are leftover? grams How many grams of lead (II) acetate are leftover? grams How many grams of lead (II) sulfate are produced? grams How many grams of acetic acid are produced? grams
The balanced chemical equation for the reaction between calcium hydroxide and hydrochloric acid is: Ca(OH)2 ( aq) + 2 HC1 ( aq )→ CaCl2 ( aq ) + 2 H,0 (1) We can interpret this to mean: 1 mole of calcium hydroxide and |mole(s) of hydrochloric acid React to produce: | mole(s) of calcium chloride and |mole(s) of water
Yeast converts glucose (C6H1206) into ethanol (d = 0.789 g/mL) in a process called fermentation. An unbalanced equation for the reaction can be written as follows: CH₁206(aq) C₂H₂OH(1) + CO₂(g) - Balance this fermentation reaction by adding the missing coefficients. X X₁ He d. 1 C6H₁2O6(aq) - 2_C₂H₂OH(1)+ 2_CO₂(g) If 350.0 g of glucose yields 142.0 mL of ethanol, what is the percent yield for the reaction? % See Periodic Table See Hint
[References] Use the References to access important values if needed for this question. For the following reaction, 27.8 grams of sodium chloride are allowed to react with 66.9 grams of silver nitrate. sodium chloride ( aq ) + silver nitrate ( aq) → silver chloride ( s) + sodium nitrate ( aq ) What is the maximum amount of silver chloride that can be formed? grams What is the FORMULA for the limiting reagent? What amount of the excess reagent remains after the reaction is complete? grams Visited Submit Answer Try Another Version 1 item attempt remaining Show Hint
Sulfuric acid dissolves aluminum metal according to the following reaction: 2A1(s) + 3H;SO, (aq) → AL (SO,)s (aq) + 3H2(g) Part A Suppose you wanted to dissolve an aluminum block with a mass of 18.1 g- What minimum mass of H2SO4 (in g) would you need? Express your answer in grams to three significant figures. Submit Requeet Anewer Part B What mass of H2 gas (in g) would be produced by the complete reaction of the aluminum block? Express your answer in grams to three significant figures.
In one experiment, 12.0 g of PCl5 was slowly added to 15.0 g of H2O according to the following balanced chemical equation: Pcl5(s)+4H2O(l) ---> H3PO4 (aq) + 5HCl (g) The molar masses for each compounds in the equation are as follows; PCl5: 208.224 g/mol H2O: 18.015 g/mol H3PO4: 97.994 g/mol HCl; 36.45 g/mol What is the limiting reagent in this scenario? Your answer should be an explanation! You're not solving anything. Note! Make an accurate claim: The limiting reagent in this scenario is _____. Provide additional details and use subject specific language. Cite evidence from what's given to you in the problem that supports your answer, hint: look at that equation!. Lastly! Fully connect the evidence to the claim/your answer to the question. Include subject specific language in your reasoning. The two images attached are examples of how your response SHOULD look.
Zinc sulfide reacts with oxygen according to the reaction2ZnS(s) + 3O2 (g)› 2ZnO(s) + 2SO2 (g)A reaction mixture initially contains 4.8 mol ZnS and 8.9mol O2Once the reaction has occurred as completely as possible, what amount (in moles) of the excess reactant remains? Express your answer using two significant figures.
When calcium carbonate is added to hydrochloric acid, calcium chloride, carbon dioxide, and water are produced. CaCO₂ (s) + 2HCl(aq) →→→ CaCl₂ (aq) + H₂O(l) + CO₂(g) How many grams of calcium chloride will be produced when 30.0 g of calcium carbonate is combined with 13.0 g of hydrochloric acid? mass of CaCl₂: Which reactant is in excess? CaCO, HCI How many grams of the excess reactant will remain after the reaction is complete? mass of excess reactant: g g
The Apollo 13 mission astronauts are running out of oxygen and need to get rid of the excess carbon dioxide. You know that sodium hydroxide can remove carbon dioxide from the spacecraft cabin. The filter which they had been using is fully saturated and no longer works. The astronauts have a 5 kg container of sodium hydroxide on the ship. The reaction to neutralize the air, remove carbon dioxide with sodium hydroxide is shown below CO2(g) + 2NaOH(s) ⟶⟶ Na2CO3(aq) + H2O(l) The astronauts have 2 days left before they land on earth. You know that there are three astronauts, and each astronaut emits roughly 500. g of carbon dioxide each day. Is there enough sodium hydroxide in the cabin to cleanse the cabin air of the carbon dioxide, or are the astronauts doomed? Calculate how much sodium hydroxide is required to remove all the carbon dioxide from the three astronauts. Be sure to show all your work!
6. Consider the following chemical reaction: 2 Cr(OH)3(aq) >Cr₂O3(s) + 3H₂0(1) 12.00 moles of chromium (III) hydroxide is decomposed. Calculate moles of the water produced. O 18.00 moles O 1.500 moles O 4.00 moles O 12.00 moles
Epsom salts, a strong laxative used in veterinary medicine, is a hydrate, which means that a certain number of water molecules are included in the solid structure. The formula for Epsom salts can be written as MgSO4⋅xH2OMgSO4⋅xH2O, where xx indicates the number of moles of H2OH2O per mole of MgSO4MgSO4. When 7.592 gg of this hydrate is heated to 250 ∘C∘C, all the water of hydration is lost, leaving 3.708 gg of MgSO4MgSO4. What is the value of x?
Epsom salts, a strong laxative used in veterinary medicine, is a hydrate, which means that a certain number of water molecules are included in the solid structure. The formula for Epsom salts can be written as MgSO4⋅xH2OMgSO4⋅�H2O, where x� indicates the number of moles of H2OH2O per mole of MgSO4MgSO4. When 5.061 gg of this hydrate is heated to 250 ∘C∘C, all the water of hydration is lost, leaving 2.472 gg of MgSO4MgSO4.