3:19 AM Wed Jan 2959% 4www-awn.aleks.comAAfe mass - Google SearchALEKS - Camille Johnson - LearnAnswered: Measurements show that unknown compound... | bartlebyO STOICHIOMETRYCamilleElemental analysis of binary compoundsMeasurements show that unknown compound X has the following composition:elementmass %25.9%nitrogen74.0%охудеnWrite the empirical chemical formula of X.olo18ArCheckExplanation© 2020 McGraw-Hill Education. All Rights Reserved. Terms of Use | Privacy

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Living by Chemistry

2nd Edition

ISBN:9781464142314

Author:Angelica M. Stacy

Publisher:Angelica M. Stacy

ChapterU4: Toxins: Stoichiometry, Solution Chemistry, And Acids And Bases

Section: Chapter Questions

Problem 20STP

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A 13.2010g sample of hydrated zinc sulfate, ZnSO4 • xH2O), was strongly heated until no further change in mass was recorded. The final mass of solid product was found to be 7.3997g. On heating, all of the water of crystallization had evaportaed, as shown by the equation: ZnSO4 • xH2O -> ZnSO4 + xH2O Calculate the number of moles of water of crystallization in the sample. Write in a padpaper and show the complete solution
A compound consists of 65.45% C, 5.492% H,and 29.06% O on a mass basis and has a molarmass of 110 g/mol. Determine the molecularformula of the compound.
Write the empirical formula for the hydrated KAl(SO4)2, based on moles of anhydrous KSI(SO4)2= 0.046 mol molar mass of H2O= 18g/ mol moles of H2O= 0.0444mol ratio pf moles H20 to moles of anhydrous KAI(SO4)2= 9.65/1 . Show all work including units. Hint: if the ratio of moles of H2O to moles of anhydrous KAl(SO4)2 was 4, then the empirical formula would be: KAl(SO4)2•4H2O.
Sulfur can be recovered from the hydrogen sulfide removed from crude oil deposits, a process known as sweetening, by roasting in air and using the sulfur dioxide initially formed to push the reaction to the final product: H2S(g) + O2(g) --> H2O(g) + SO2(g) H2S(g) + SO2(g) --> H2O(g) + S(s) The maximum number of kilograms of sulfur that can be isolated per kilogram of hydrogen sulfide entering the process is __________.
The hydrated salt, MY3·xH2O, was heated strongly in a crucible to remove all the watermolecules of crystallization.The data are for this experiment are given in the table below.Mass of empty crucible and cover 29.73 gMass of crucible, cover, and hydrated salt 32.72 gMass of crucible, cover, and anhydrous salt 31.52 gMolar mass of anhydrous salt 241.88 g/mol(i) Calculate the % composition by mass of water in the hydrated salt.(ii) Determine the value of x.(iii) M is in Period 4 of the Periodic Table of the Elements.If Y = NO3–, identify the element M.(iv) What is the name of this hydrated salt? ___
Mass of oxygen = 0.49g- 0.33g= 0.16gNumber of moles = given mass / molar massNumber of moles of oxygen = 0.16/ 16 = 0.01 molMolar Mass of magnesium = 24.3gMoles of magnesium = 0.33g / 24.3g = 0.0135 mol Moles of magnesium 0.0135 1.35 3 4------------------------ = _____________ = ____________ x ________ = ___Moles of oxygen 0.01 1 3 3 The ratio between the moles of magnesium used and the moles of oxygen uses is 4/3. Based on your experimental data, write the empirical formula for magnesium oxide. Is this the molecular formula or the simplest formula? Explain how you know this.
Mass of sample: 0.60g Mass of top of funnel + filter paper: 14.72g Mass of top of funnel + filter paper + MgNH4PO4.6H2O: 16.07g What is: Mass of MgNH4PO4.6H2O Molar Mass of MgNH4PO4.6H2O Moles of MgNH4PO4.6H2O Molar Ratio MgNH4PO4.6H2O : P Moles of P Mass of P in the original sample of plant food % of P in the original sample of plant food Moles of P Molar ratio P2O5 : P Moles of P2O5 Molar Mass of P2O5 Mass of P2O5 in the original sample of plant food % of P2O5 in the original sample of plant food
Given the unbalanced equation: C6H6 + O2 ---> H2O + CO2. When properly balanced, the coefficient of H2O is:
Iron(II) sulfate forms several hydrates with the general formula FeSO4·xH2O, where x is an integer. If the hydrate is heated, the water can be driven off, leaving pure FeSO4 behind. Suppose a sample of a certain hydrate is heated until all the water is removed, and it's found that the mass of the sample decreases by45.%. Which hydrate is it? That is, what is x?
At the end of this, how did we go from a 5 to 1 ratio moles to 2CO2 and 3H2O?
GivenRaw Materials: 500 g calcium polysulphide and 1.5 kg hydrochloric acid Actual Yield: 343.4g precipitated sulfurWhereas the balanced chemical reaction, as given in the problem is: CaS5+2HCl => 4S + CaCl2 + H2Sa. Find the Mass to Mass Stoichiometry Calculation b. Upon solving A, find the LIMITING REAGENT, EXCESS REAGENT and the AMOUNT IN EXCESSc. Find the Percentage Yield from Problem Ad. Find the number of dosage form and packaging that can be produced from the stoichiometric calculation based on Problem A
For the reaction C2H4 + 3O2 ---> 2CO2 + 2H2O, does this mean that ten (10) grams of CO2 produced reuired 0.345 mol O2?

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