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My teacher hates kids that play sports. I have asked about these chem questions but she doesnt seem to care.? 1.The acid contained in storage batteries is acetic hydrochloric nitric sulfuric _______ 2.Hydrogen sulfide forms a white precipitate when passes into a solution of Cd(NO3)2 Pb(NO3)2 CuCl2 ZnSO4 ______ 3.A sulfur compound that will readily dissolve sulfur is H2SO4 SO2 CS2 H2S _____ 4.When sulfur reacts with oxygen, heat is neither liberated nor absorbed absorbed liberated sometimes liberated and sometimes absorbed ______ 5.Sulfur dioxide is used in commercial refrigerators because the gas is easily liquified dissolves in water is cold _____ 6.If the volume of sulfuric acid in an uncovered beaker increased gradually during a perios of several weeks, the increase was probably due to the absorption of carbon dioxide nitrogen oxygen water _____ Yes this is my homework. It is not graded and there are only 6 questions. ... (Asked by Joe)
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you're teacher seriously won't help? I would talk to the principal of the school (or the dean or whoever). It is the teacher's job to help you!...(Answered by poohb2878)

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A chemistry question.? I need some help with this kind of chemistry question:(Note: Please simplify your answer so I can understand it, and also show all work.) Magnesium reacts with sulfuric acid according to the following equation. How many moles of H2 are produced by the complete reaction of 230mg of Mg with sulfuric acid. Mg + H2SO4----> MgSO4+H2 Thanks so much. ... (Asked by trinitarianwiccan)
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The number of moles of H2 liberated is equal to the number of moles of Mg involed in the reaction, provided the sulphuric acid is in excess. let the molar mass of Mg be x. then , no. of moles of H2 liberated=no. of moles of Mg reacted=230/x...(Answered by panther)

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more chemistry and enthalpy? part 1: An industrial process for manufacturing sulfuric acid, H2SO4, uses hydrogen sulfide, H2S, from the purification of natural gas. In the first step of this process, the hydrogen sulfide is burned to obtain sulfur dioxide, SO2. 2H2S(g) + 3O2(g) ==> 2H2O(l) + 2SO2(g); DeltaHo = -1125 kJ The density of sulfur dioxide at 25oC and 1.00 atm is 2.62 g/L, and the molar heat capacity is 30.2 J/(mol x oC). How much heat (in kJ) would be evolved in producing 1.00 L of SO2 at 25oC and 1.00 atm? part 2: Suppose heat from this reaction is used to heat 1.00 L ... (Asked by teenie263)
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I ll be glad to discuss live over voice n whiteboard but cannot type out the whole thing .IM me I am free now...(Answered by raindrops on a leaf)

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Molality of the acid produced by the dilution? Approximately 2.29 mL of concentrated sulfuric acid (specific gravity is 1.84 is added to water. The dilute sulfuric acid is titrated against NaOH and the concentration of H2SO4 is 0.184 mol dm^-3. How do I calculate the molality of the acid produced by the dilution? ... (Asked by sky_blue)
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Essentially, you're given the molarity of the dilute acid, from which you can deduce the molality by finding the weight of the water in 1 L of solution. Step 1: Find out the mass of acid in 1 L of solution. mass = .184 moles * molecular mass of H2SO4 2 H (1) + 4 O (16) + S (32) = 96 g/mol .184 mol * 96 g/mol = 17.664 g H2SO4 / L Step 2: Using the mass and specific gravity, find the volume of acid. 17.664 g / 1.84 g/cm^3 = 9.239 cm^3 of acid Step 3: Given the volume of acid, and 1 liter ...(Answered by ³√carthagebrujah)

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2 science homework questions, please help!!! All it is is a list, PLEASE HELP!!!? I need some help with this, I would REALLY appreciate it if you guys helped me, PLEASE and THANKS!!! Please list 4 examples of items that have sulfuric acid in them, or are made with sulfuric acid. Please list 6 foods that have a sour/tingy taste because of hydrogen ions. PLEASE HELP!!! THANKS!!! I only need 2 items for the sulfuric acid question now. SOMEBODY PLEASE HELP!!! Now I only need an answer for the list of 6 foods, PLEASE!!! Thanks to the two ladies who have helped so far! Now all I need is 3 more foods that have a sour/tingy taste to them. I ... (Asked by ii'M tRaPp3d iiN Mii LiiF3)
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Here is some with sulfuric acid: Acid Rain Producing Iron and Steel Ammonium Sulfate (nitrogen fertilizer) Papermaker's Alum Nylon Sour/Tingy Taste: Curdled Milk (EWWW) Vinegar Lemon Juice Orange Juice...(Answered by Simply Me)

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Which planets atmosphere is characterized by the presence of carbon dioxide and sulfuric acid? ... (Asked by )
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go to cosmeo.com and sign up for a free 30-day trial. it is really helpful! This site is dedicated to helping students with their homework and increasing grades. There are videos, articals, places where they show you how to do the math problem... just check it out.. it is pretty cool....(Answered by mrsmorales541)

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Question about REDOX? Is this reaction a redox reaction? Is there any change in oxidation numbers? Aluminium nitrate + concentrated sulfuric acid I heard that concentrated sulfuric acid acts differently from the dilute acid. What are the properties of the concentrated acid? ... (Asked by formystudies5)
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http://www.efma.org/publications/NitricAcid/Section03.asp...(Answered by Farkette at ♥)

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Chemistry... Atmosphere/Pressure/Gas Laws? Write reactions to show how nitric acid and sulfuric acid are produced in the atmosphere. Oh, and could you explain to me how you found them out? thanks a billion. ... (Asked by :))
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Sulfuric acid is produced in the upper atmosphere of Venus by the sun's photochemical action on carbon dioxide, sulfur dioxide, and water vapor. Ultraviolet photons of wavelengths less than 169 nm can photodissociate carbon dioxide into carbon monoxide and atomic oxygen. Atomic oxygen is highly reactive; when it reacts with sulfur dioxide, a trace component of the Venusian atmosphere, the result is sulfur trioxide, which can combine with water vapor, another trace component of Venus' atmosphere, to yield sulfuric acid. CO2 → CO + O SO2 + O → SO3 SO3 ...(Answered by farah_727rash)

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Which one of the foloowing statement about sulfuric acid is correct? a) sulfuric acid ia a known muriatic acid b) sulfuric acid is a strong oxidizing agent c) sulfuric acid has a little effect on metals d) sukfuric acid is dangerous to living organisms ... (Asked by tillie)
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It is a strong oxidizing agent....(Answered by R@inY)

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Zn reacts with 100.0 mL of 6.00 M sulfuric acid through single replacement? 1. how many grams of zinc sulfate can be produced? 2. How many liters of hydrogen gas could be released as STP? please explain step by step and provide answer :]] ... (Asked by arg.jew.)
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First write the balanced equation: Zn + H2SO4 -> ZnSO4 + H2 Now find the number of moles of H2SO4 used in the reaction: 100 mL = 0.1L 6.00M = 6.00 moles/L 6.000.1 = 0.6 moles of H2SO4 used in the reaction mole ratio from the balanced equation: 1 mole H2SO4 / 1 mole ZnSO4 = 0.6 moles H2SO4 / x moles ZnSO4 This means that 0.6 moles of ZnSO4 are produced. Find the molar mass of ZnSO4: Zn = 65.38 g/mol S= 32.06 g/mol O=15.9994 g/mol ZnSO4 = 65.38 + 32.06 + 415.9994 = 161.4376 g/mol 161.4376 g/mol * 0.6 moles 96.86 g ZnSO4 produced For part 2, find the mole ratio of H2SO4 ...(Answered by Jenelle)

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Zn reacts with 100.0 mL of 6.00 M sulfuric acid through single replacement? 1. how many grams of zinc sulfate can be produced? 2. How many liters of hydrogen gas could be released as STP? please explain step by step and provide answer :]] ... (Asked by arg.jew.)
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First write the balanced equation: Zn + H2SO4 -> ZnSO4 + H2 Now find the number of moles of H2SO4 used in the reaction: 100 mL = 0.1L 6.00M = 6.00 moles/L 6.000.1 = 0.6 moles of H2SO4 used in the reaction mole ratio from the balanced equation: 1 mole H2SO4 / 1 mole ZnSO4 = 0.6 moles H2SO4 / x moles ZnSO4 This means that 0.6 moles of ZnSO4 are produced. Find the molar mass of ZnSO4: Zn = 65.38 g/mol S= 32.06 g/mol O=15.9994 g/mol ZnSO4 = 65.38 + 32.06 + 415.9994 = 161.4376 g/mol 161.4376 g/mol * 0.6 moles 96.86 g ZnSO4 produced For part 2, find the mole ratio of H2SO4 ...(Answered by Jenelle)

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