1. Ammonium sulfate is used as a source of nitrogen in some fertilizers. It reacts with sodium hydroxide to produce sodium sulfate, water and ammonia, NH3. What mass of sodium hydroxide is required to react completely with 15.4 g of ammonium sulfate? 2. Iron (III) oxide, rust, can be removed from iron by reacting it with hydrochloric acid, HCI, to produce iron (III) chloride and water. What mass of hydrogen chloride is required to react with 100 g of rust? 3. Dinitrogen pentoxide is a white solid. When heated it decomposes to produce nitrogen dioxide and oxygen. How many grams of oxygen gas will be produced in this reaction when 2.34 g of NO2 are made?

1. Ammonium sulfate is used as a source of nitrogen in some fertilizers. It reacts with sodium hydroxide to produce sodium sulfate, water and ammonia, NH3. What mass of sodium hydroxide is required to react completely with 15.4 g of ammonium sulfate? 2. Iron (III) oxide, rust, can be removed from iron by reacting it with hydrochloric acid, HCI, to produce iron (III) chloride and water. What mass of hydrogen chloride is required to react with 100 g of rust? 3. Dinitrogen pentoxide is a white solid. When heated it decomposes to produce nitrogen dioxide and oxygen. How many grams of oxygen gas will be produced in this reaction when 2.34 g of NO2 are made?

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

Consider the copper thermite reaction, a reaction between two solids that can be initiated with strong heating: 3 CuO(s) + 2 Al(s) → 3 Cu(s) + Al2O3(s) 25.0 g of copper(II) oxide are combined with 25.0 g of Al , and the mixture is heated strongly to react. molar masses (g/mol): CuO - 79.55 Al - 26.98 Cu - 63.55 What is the chemical formula or elemental symbol for the limiting reactant? What is the chemical formula or elemental symbol for the excess reactant?
The useful metal manganese can be extracted from the mineral rhodochrosite by a two-step process. In the first step, manganese(II) carbonate and oxygen react to form manganese(IV) oxide and carbon dioxide: 2MnCO,(G) + 0,(g) 2M1O,(G) + 2C0, (g) In the second step, manganese(IV) oxide and aluminum react to form manganese and aluminum oxidide: 3 MnO, (s) + 4Al(s) 3 Mn(s) + 2 Al,O3 (s) Suppose the yield of the first step is 95.% and the yield of the second step is 84.%. Calculate the mass of manganese(II) carbonate required to make 10.0 kg of manganese. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits. olo
In a reaction, 1 mole of silver nitrate combines with 1 mole of sodium chloride. AgNO3 + NaCl Which statement about the product is justified by the law of conservation of mass? There will be five atoms in the product. There will be two molecules in the product. There will be 1 mole of silver (Ag) in the product. There will be 2 moles of sodium (Na) in the product.
13. Suppose 90.0 g of Iron (III) chloride reacts with 17g of water? What is the limiting reagent? How much (in grams) will the products produce and how much of the excess reactant will remain after the reaction is complete?( Write the complete balanced reaction along with it states)
2. When a student reacted 66.8 grams of solid potassium metal with excess phosphoric acid only 1.18 grams of gas (H₂) were produced. Assumed this reaction occurs because potassium is more reactive than hydrogen. What is the percent yield of the student's reaction?
90. Phosgene (COCI,) reacts with ammonia (NH,), as shown in this reaction. If 1.2 grams of COCI, are added to 10.5 grams of NH,, what is the limiting reagent? What mass of CH,N,0 can be produced in this reaction? COCI, (g) + 2 NH3 (g) → CH,N,0 (g) + 2 HCI (g)
a. According to the following reaction, how many moles of mercury will be formed upon the complete reaction of 31.8 grams of mercury(II) oxide?2HgO (s) 2Hg (l) + O2 (g)____moles mercury b.According to the following reaction, how many grams of water are necessary to form 0.295 moles phosphoric acid?P2O5 (s) + 3H2O (l) 2H3PO4 (aq)______grams water
The reaction of carbon and water at a high temperature produces a mixture of hydrogen and carbon monoxide gases. This mixture is known as synthesis gas (or syngas). How many grams of hydrogen gas can be formed from the reaction of 125 g of water with excess carbon?
A chemist goes into the lab and performs an experiment in which a mixture of 8.47 grams of Zn and 6.03 g of sulfur are reacted. Before starting the experiment they perform the following calculations to predict the maximum (theoretical) yield of zinc sulfide that could be produced. They obtain an actual yield of 8.25 grams of zinc sulfide. Calculate their percent yield to one decimal place.
11. Elemental phosphorus, P4, reacts vigorously with oxygen to give P4O10. What is the mass of P4O10 that can be produced if 3.75 g of P4 is reacted with 6.55 g of oxygen? If any reagent was in excess, how much of it will be leftover when the reaction is finished?
Antimony is alloyed with lead to increase the rigidity of components used in the construction of lead storage batteries.3.061 g of a particular metallic alloy, compounded of only Pb and Sb, can be quantitatively converted into a 3.557-g mixture of the oxides PbO2 and Sb2O4.What was the percentage (by mass) of antimony in the alloy?
When ammonia is mixed with hydrogen chloride (HCl), the white solid ammonium chloride (NH4Cl) is produced. Suppose 10.0 g ammonia is mixed with the same mass of hydrogen chloride. What substances will be present after the reaction has gone to completion, and what will theirmasses be?