1) The decomposition of lithium azide, LIN,(s) is used to inflate airbags. On impact, the LIN,(s) is ignited by an electrical spart, producing N,(g) and Li(s). The N,() inflates the air bag. a) Write a balanced chemical equation for the decomposition of Lithium azide, using the smallest whole-number coefficients. b) What is the number of moles present in a 82.0 gram sample of LiN.(s)? Show all steps

1) The decomposition of lithium azide, LIN,(s) is used to inflate airbags. On impact, the LIN,(s) is ignited by an electrical spart, producing N,(g) and Li(s). The N,() inflates the air bag. a) Write a balanced chemical equation for the decomposition of Lithium azide, using the smallest whole-number coefficients. b) What is the number of moles present in a 82.0 gram sample of LiN.(s)? Show all steps

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

1. Write the correct chemical equation for the following reaction: when beryllium chloride reacts with silver (I) nitrate, beryllium nitrate and silver (I) chloride are formed 2. Write the correct skeleton equation for the following: fluorine gas reacts with calcium metal to form solid calcium fluoride
A common demonstration in chemistry courses involves adding a tiny speck of magnesium(IV) oxide to a concentrated hydrogen peroxide H2O2 solution Hydrogen peroxide is unstable and it decomposes quite spectacularly under these conditions to produce get oxygen gas and steam magnesium (IV) oxide is a catalyst for the decomposition of hydrogen peroxide and is not consumed in the reaction she was the balance equation for the decomposition reaction of hydrogen peroxide
Click in the answer box to activate the palette. Balance the equation representing the reaction between iron(II) oxide, Fe;Or, and carbon monoxide (CO) to yield iron (Fe) and carbon dioxide (Co,). Do not include the states of matter.
For the following, (1) predict the products, (2) write the balanced equation with formulas, (3) determine if it is a synthesis, decomposition or combustion reaction. 1. Dihydrogen Monoxide produces (SECOND HINT, THINK DIATOMICS) Synthesis, Decomposition or Combustion? Balanced Chemical Equation. and (HINT: 2 gases) Beryllium and Chlorine yield Synthesis, Decomposition or Combustion? Balanced Chemical Equation. Butane (C,H,,) and Oxygen produce Synthesis, Decomposition or Combustion? Balanced Chemical Equation. and
3. A student mixes 100.0 mL of a 0.100 M solution of potassium phosphate with 100.0 mL of a 0.125 M solution of copper (II) sulfate and obtains a blue solid. (a) Write the balanced chemical equation for the reaction including physical states. (b) Determine the limiting reagent. (c) Calculate the number of moles of the excess reagent after the reaction is completed. Record servation
What is the term for the substance in a chemical reaction that controls the maximum amount of product? A) limiting reactant B) limiting product C)maximum product
Question 6 of 21 Pure magnesium metal is often found as ribbons and can easily burn in the presence of oxygen. When 4.78 g of magnesium ribbon burns with 7.61 g of oxygen, a bright, white light and a white, powdery product are formed. Enter the balanced chemical equation for this reaction. Be sure to include all physical states. equation: What is the limiting reactant? O oxygen magnesium The reaction goes to completion, but in the process of recovering the product, some of it was lost. The the percent yield for the reaction is 82.8%. How many grams of product are recovered? mass of product recovered: g How many grams of the excess reactant remain? Assume the reaction goes to completion. mass of excess reactant:
A common method for analyzing the nickel content of a sample is to use a precipitation reaction Adding the organic compound dimethylglyoxime to a solu containing Ni* ions precipitates a red solid. Given that the sample contain, Ni-20.315%,C-33.258%,H-4884%,0-22.151%, and N-19.392%, a Calculate the number of moles of each elenment? Ni, C, H, b. Which element has the lowest number of moles? c. What is the empirical formula of the compound
A solution containing 1.50 g of iron (III) chloride reacts with a solution containing 3.00 g sodium phosphate use the Solubility Table provided to (A) determine to the balanced conventional chemical equation (do not forget the subscript defining the state of compounds). (B) Determine the net ionic equation (C) What is the limiting reactant? (D) How much in grams of the precipitant that will be produced?
MN.39.
Transfer the following into chemical equations and balance them.(i) Hydrogen gas combines with nitrogen to from ammonia.(ii) Hydrogen sulphide gas burns in air to give water and sulphurdioxide.(iii) Potassium metal reacts with water to give potassium hydroxide and hydrogen gas.
Aluminum metal reacts with aqueous iron(i) oxide to form aqueous aluminum oxide and iron metal. Write a balanced chemical equation for the above reaction State what type of reaction it is