VIDEO solution: Determine the volumes of the pure liquids required to make up 100.0 cm³ of a solution of CH₃CH₂OH and H₂O with a mole fraction of x(CH₃CH₂OH) = 0.090. The partial molar volumes of the solution at this mole fraction are: V(CH₃C (2024)

`); let searchUrl = `/search/`; history.forEach((elem) => { prevsearch.find('#prevsearch-options').append(`

${elem}

`); }); } $('#search-pretype-options').empty(); $('#search-pretype-options').append(prevsearch); let prevbooks = $(false); [ {title:"Recently Opened Textbooks", books:previous_books}, {title:"Recommended Textbooks", books:recommended_books} ].forEach((book_segment) => { if (Array.isArray(book_segment.books) && book_segment.books.length>0 && nsegments<2) { nsegments+=1; prevbooks = $(`

  • ${book_segment.title}
  • `); let searchUrl = "/books/xxx/"; book_segment.books.forEach((elem) => { prevbooks.find('#prevbooks-options'+nsegments.toString()).append(`

    ${elem.title} ${ordinal(elem.edition)} ${elem.author}

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Make an ajax call to the server and get the search database. let databaseUrl = `/search/whiletype_database/`; let resp = single_whiletyping_ajax_promise; if (resp === null) { whiletyping_database_initial_burst = whiletyping_database_initial_burst + 1; single_whiletyping_ajax_promise = resp = new Promise((resolve, reject) => { $.ajax({ url: databaseUrl, type: 'POST', data:{csrfmiddlewaretoken: "YJCSStFKADuWtHFvd2YNb3oJkwhrei6IWS5p6AJ4ARXMbeF7dnvHB2dOSm4QISob"}, success: function (data) { // 3. verify that the elements of the database exist and are arrays if ( ('books' in data) && ('curriculum' in data) && ('topics' in data) && Array.isArray(data.books) && Array.isArray(data.curriculum) && Array.isArray(data.topics)) { localforage.setItem('whiletyping_last_success', (new Date()).getTime()); localforage.setItem('whiletyping_database', data); resolve(data); } }, error: function (error) { console.log(error); resolve(null); }, complete: function (data) { single_whiletyping_ajax_promise = null; } }) }); } return resp; } return Promise.resolve(null); }).catch(function(err) { console.log(err); return Promise.resolve(null); }); } function get_whiletyping_search_object() { // gets the fuse objects that will be in charge of the search if (whiletyping_search_object){ return Promise.resolve(whiletyping_search_object); } database_promise = localforage.getItem('whiletyping_database').then(function(database) { return localforage.getItem('whiletyping_last_success').then(function(last_success) { if (database==null || (new Date()) - (new Date(last_success)) > 1000*60*60*24*30 || (new Date('2023-04-25T00:00:00')) - (new Date(last_success)) > 0) { // New database update return get_whiletyping_database().then(function(new_database) { if (new_database) { database = new_database; } return database; }); } else { return Promise.resolve(database); } }); }); return database_promise.then(function(database) { if (database) { const options = { isCaseSensitive: false, includeScore: true, shouldSort: true, // includeMatches: false, // findAllMatches: false, // minMatchCharLength: 1, // location: 0, threshold: 0.2, // distance: 100, // useExtendedSearch: false, ignoreLocation: true, // ignoreFieldNorm: false, // fieldNormWeight: 1, keys: [ "title" ] }; let curriculum_index={}; let topics_index={}; database.curriculum.forEach(c => curriculum_index[c.id]=c); database.topics.forEach(t => topics_index[t.id]=t); for (j=0; j

    Solutions
  • Textbooks
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  • Solutions ${viewAllHTML}
  • `); let questionUrl = "/questions/xxx/"; let askUrl = "/ask/question/xxx/"; solution_search_result.forEach((elem) => { let url = ('course' in elem)?askUrl:questionUrl; let solution_type = ('course' in elem)?'ask':'question'; let subtitle = ('course' in elem)?(elem.course??""):(elem.book ?? "")+"    "+(elem.chapter?"Chapter "+elem.chapter:""); solutions_section.find('#whiletyping-solutions').append(` ${elem.text} ${subtitle} `); }); $('#search-solution-options').empty(); if (Array.isArray(solution_search_result) && solution_search_result.length>0){ $('#search-solution-options').append(solutions_section); } MathJax.typesetPromise([document.getElementById('search-solution-options')]); } } function build_textbooks() { $('#search-pretype-options').empty(); $('#search-pretype-options').append($('#search-solution-options').html()); if (Array.isArray(textbook_search_result)) { var books_section = $(`
  • Textbooks View All
  • `); let searchUrl = "/books/xxx/"; textbook_search_result.forEach((elem) => { books_section.find('#whiletyping-books').append(` ${elem.title} ${ordinal(elem.edition)} ${elem.author} `); }); } if (Array.isArray(textbook_search_result) && textbook_search_result.length>0){ $('#search-pretype-options').append(books_section); } } function build_popup(first_time = false) { if ($('#search-text').val()=='') { build_pretype(); } else { solution_and_textbook_search(); } } var search_text_out = true; var search_popup_out = true; const is_login = false; function pretype_setup() { $('#search-text').focusin(function() { $('#search-popup').addClass('show'); resize_popup(); search_text_out = false; }); $( window ).resize(function() { resize_popup(); }); $('#search-text').focusout(() => { search_text_out = true; if (search_text_out && search_popup_out) { $('#search-popup').removeClass('show'); } }); $('#search-popup').mouseenter(() => { search_popup_out = false; }); $('#search-popup').mouseleave(() => { search_popup_out = true; if (search_text_out && search_popup_out) { $('#search-popup').removeClass('show'); } }); $('#search-text').on("keyup", delay(() => { build_popup(); }, 200)); build_popup(true); let prevbookUrl = `/search/pretype_books/`; if (is_login) { $.ajax({ url: prevbookUrl, method: 'POST', data:{csrfmiddlewaretoken: "YJCSStFKADuWtHFvd2YNb3oJkwhrei6IWS5p6AJ4ARXMbeF7dnvHB2dOSm4QISob"}, success: function(response){ previous_books = response.previous_books; recommended_books = response.recommended_books; build_popup(); }, error: function(response){ console.log(response); } }); } else { let prebooks = null; try { prebooks = JSON.parse(localStorage.getItem('PRETYPE_BOOKS_ANON')); }catch(e) {} if (prebooks && 'previous_books' in prebooks && 'recommended_books' in prebooks) { anon_pretype(); } else { $.ajax({ url: prevbookUrl, method: 'POST', data:{csrfmiddlewaretoken: "YJCSStFKADuWtHFvd2YNb3oJkwhrei6IWS5p6AJ4ARXMbeF7dnvHB2dOSm4QISob"}, success: function(response){ previous_books = response.previous_books; recommended_books = response.recommended_books; build_popup(); }, error: function(response){ console.log(response); } }); } } } $( document ).ready(pretype_setup); $( document ).ready(function(){ $('#search-popup').on('click', '.search-view-item', function(e) { e.preventDefault(); let autoCompleteSearchViewUrl = `/search/autocomplete_search_view/`; let objectUrl = $(this).attr('href'); let selectedId = $(this).data('objid'); let searchResults = []; $("#whiletyping-solutions").find("a").each(function() { let is_selected = selectedId === $(this).data('objid'); searchResults.push({ objectId: $(this).data('objid'), contentType: $(this).data('contenttype'), category: $(this).data('category'), selected: is_selected }); }); $("#whiletyping-books").find("a").each(function() { let is_selected = selectedId === $(this).data('objid'); searchResults.push({ objectId: $(this).data('objid'), contentType: $(this).data('contenttype'), category: $(this).data('category'), selected: is_selected }); }); $.ajax({ url: autoCompleteSearchViewUrl, method: 'POST', data:{ csrfmiddlewaretoken: "YJCSStFKADuWtHFvd2YNb3oJkwhrei6IWS5p6AJ4ARXMbeF7dnvHB2dOSm4QISob", query: $('#search-text').val(), searchObjects: JSON.stringify(searchResults) }, dataType: 'json', complete: function(data){ window.location.href = objectUrl; } }); }); });
    VIDEO solution: Determine the volumes of the pure liquids required to make up 100.0 cm³ of a solution of CH₃CH₂OH and H₂O with a mole fraction of x(CH₃CH₂OH) = 0.090. The partial molar volumes of the solution at this mole fraction are: V(CH₃C (2024)

    FAQs

    What is the volume of 1 mole of gas at 1 atm? ›

    Molar volume is the volume occupied by 1 mol of any (ideal) gas at standard temperature and pressure (STP: 1 atmospheric pressure, 0 °C). Show that it is 22.4 litres.

    How to calculate the volume of 1 mole? ›

    At standard Temperature and Pressure (STP) the molar volume (Vm) is the volume occupied by one mole of a chemical element or a chemical compound. It can be calculated by dividing the molar mass (M) by mass density (ρ). Molar gas volume is one mole of any gas at a specific temperature and pressure has a fixed volume.

    What are the partial molar volumes of water and ethanol? ›

    The partial molar volumes of water and ethanol in a solution with x H 2 , o = 0.45 at 25 ∘ C are 17.0 and 57.5 cm 3 mol − 1 , respectively.

    What is the molar volume of water at 25 C? ›

    At 25∘C and 1bar, the molar volume of pure water is V∗m,A=18.07cm3 mol−1 and that of pure methanol is V∗m,B=40.75cm3 mol−1.

    What volume of O2 measured at 1 atm? ›

    = 0.025*22.4 L = 0.56 L of O2.

    What is the volume of 1.0 mol of a gas at 1 atm and 00 C? ›

    What is the volume of 1 mole of an ideal gas at STP (Standard Temperature and Pressure = 0 °C, 1 atm)? So, the volume of an ideal gas is 22.41 L/mol at STP. This, 22.4 L, is probably the most remembered and least useful number in chemistry.

    What is the formula for volume? ›

    Volume Formulas of Various Geometric Figures
    ShapesVolume FormulaVariables
    Rectangular Solid or CuboidV = l × w × hl = Length w = Width h = Height
    CubeV = a3a = Length of edge or side
    CylinderV = πr2hr = Radius of the circular base h = Height
    PrismV = B × hB = Area of base, (B = side2 or length.breadth) h = Height
    6 more rows
    Oct 12, 2020

    How to calculate volume of water? ›

    Formula:
    1. Formula:
    2. L x W x D. = Cubic Feet.
    3. Cubic ft x 7.47. = Gallons.

    What is the formula for volume of water? ›

    It's a simple calculation you just multiply the average length x width x depth to calculate the cubic meters (M3). You then multiply this by 1000 to work out how many litres of water your pond system holds. In the below example we have an average length of 2m with an average width of 1.5m and an average depth of 1.2m.

    What is the formula for partial volume? ›

    Partial Molar Volume:

    (5.33) V = n1V1 + n2V2. The units of partial molar volumes are the same as molar volumes. The relationship between the two, i.e., partial molar volume and the molar volume is a subtle but important one. be identical to the molar volume of the pure substance in the absence of the other component.

    How to determine excess volume? ›

    Calculate the difference between the theoretical and the measured volume average for each mixture. This number represents the excess volume of your mixture. Subtract the measured average volume from the theoretical volume for each mixture.

    What is the unit of molar volume? ›

    It is equal to the molar mass (M) divided by the mass density (ρ). It has the SI unit cubic meters per mole (m3/mol), and often practical to use the units cubic decimeters per mole (dm3/mol) for gases and cubic centimeters per mole (cm3/mol) for liquids and solids.

    What is the molar volume of water at 4 C density of water at 4 C is 1 g cc? ›

    Answer. Answer: Thus, the molarity of pure water at a temperature of 4 degrees celsius is equal to 55.56 moles per litre.

    What is the volume at 25 C and 1 atm? ›

    Molar volume at 25°C and 1 atm

    Now, we can calculate the molar volume of an ideal gas at 25°C and 1 atm: V = 1 × 0.0821 × 298.15 1 = 24.465 L / m o l So, the molar volume of an ideal gas at 25°C and 1 atm pressure is approximately 24.465 L/mol.

    What is the volume of a certain amount of a gas at 25 C? ›

    The volume of a certain amount of a gas at 25∘C and at 100 cm pressure is 80 mL.

    What is the volume of a gas at atm? ›

    The volume of 1.00mol of any gas at STP (Standard temperature, 273.15 K and pressure, 1 atm) is measured to be 22.414L. We can substitute 101.325kPa for pressure, 22.414L for volume, and 273.15K for temperature into the ideal gas equation and solve for R.

    What is the volume of 1 mole of any gas at? ›

    One gram mole of a gas at STP occupies 22.4L volume.

    What is the gas constant at 1 atm? ›

    The value of R at atm that is at standard atmospheric pressure is R = 8.3144598 J.

    What is the volume of 0.5 mole of gas at 1 atm pressure and 273? ›

    pressure and 273 K is. 22.4 litres.

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