2.4 How many moles of gas would be produced if this amount of sodium bicarbonate reacted completely with acetic acid, which you added as vinegar? Jdeal Gas law Re 0.0821Lat m mol.k. PV- nRT P= 1.013x 105 Molar mass of MaHCOB Na HCO8 OBRD 84.00 glmol %3D 2.5 What volume would this amount of gas occupy at room temperature (25.0 °C)? At refrigerator temperatures (4.0 °C)? Or at freezer temperature (-20.0 °C)? 2 1.013x 105 ppessre

2.4 How many moles of gas would be produced if this amount of sodium bicarbonate reacted completely with acetic acid, which you added as vinegar? Jdeal Gas law Re 0.0821Lat m mol.k. PV- nRT P= 1.013x 105 Molar mass of MaHCOB Na HCO8 OBRD 84.00 glmol %3D 2.5 What volume would this amount of gas occupy at room temperature (25.0 °C)? At refrigerator temperatures (4.0 °C)? Or at freezer temperature (-20.0 °C)? 2 1.013x 105 ppessre

Chemistry & Chemical Reactivity

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ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter20: Environmental Chemistry-earth's Environment, Energy, And Sustainability

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Problem 41PS

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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.
7. Given that the kf of water in a car radiator filled with liquid in the ratio of 62 g of ethylene glycol (HOCH₂ CH₂OH) in 500 g of water is.... (A) -0.93 °C (B) -1.86 C (C) -3.73 C (D) -7.64 °C (E) -5.58 C
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? ___
Consider Palmitic acid C16H32O2, a common fatty acid used in the manufacture of soap. A solution of palmitic acid is prepared by mixing 112 g palmitic acid with 725 mL of benzene C6H6. The density of the resulting solution is 0.902 g/mL. Palmitic acid (molar mass = 256 g/mol and density = 0.852 g/mL); Benzene (molar mass = 78 g/mol and density = 0.879 g/mL) A. What is the %m/m of the solution? B. What is the molarity of the solution? C. What is the mole fraction of the solvent?
Give the theoretical yield, in moles, of CO2 from the reaction of 0.60 moles of C8H18 with 40.00 moles of O2. 2C8H18+25O2 ---> 16CO2 + 18H2O
Consider Palmitic acid C16H32O2, a common fatty acid used in the manufacture of soap. A solution of palmitic acid is prepared by mixing 112 g palmitic acid with 725 mL of benzene C6H6. The density of the resulting solution is 0.902 g/mL. Palmitic acid (molar mass = 256 g/mol and density = 0.852 g/mL); Benzene (molar mass = 78 g/mol and density = 0.879 g/mL) 1. What is the % m/m of the solution? 2. What is the mole fraction of the solvent? 3. What is the molarity of the solution? Based from the calculated molarity of the solution in #3, you are to prepare 250 mL of the said molar concentration. If you have an available 2M stock solution of Palmitic acid, How many mL of the 2M palmitic acid stock solution will you need? and; 4. How many mL of solvent do you need to add to the amount gotten from the 2M Palmitic acid stock solution in order to prepare 250 mL total volume of your desired solution?
A crime scene analyst found out a 10 mm thick metal plate was penetrated by 10 bullets that caused a severe but clean volumetric defect in the form of 10 holes with a diameter of 10 mm each. If the theoretical density of the metal plate is 10 g/cm3, how many metal atoms have been removed from the plate due to the impact? Assume a solid structured metal, with an atomic weight of 100 g/mol, Given the Avogadro constant as 6 × 1023 atom/mol and π = 3.14.
18.2 Balance the following chemical equation for the stoichiometric combustion of methane with oxygen. ____ CH4(g) + ______O2(g) ⟶ ______ CO2(g)+ ______H2O(g) What are the coefficients for O2(g) and CO2 (g)?
A hydrate [hydrates have the general formula AB • xH2O] is found to have the percentcomposition: Na = 19.17%, C = 10.00%, H = 4.17% and O = 66.6%. After heating to 100 oC todrive off the water of hydration, the percent composition is found to be: Na = 27.38%,C = 14.28%, H = 1.19% and O = 57.15%. From this data, determine the probable molecularformula for the hydrate if the molecular weight = 120 amu.
If the empirical formula of a compound is found to be CH2, which of the following value is a plausible molecular mass for the compound? The answer is 70.15. How did you get that?
A mixture weighing 9.25 mg contained only cyclohexane, C6H12 (FM 84.159), and oxirane, C2H4O (FM 44.053). When the mixture was analyzed by combustion analysis, 20.87 mg of CO2 (FM 44.010) were produced. Find the weight percent of oxirane in the mixture.
what is the coefficient in front of the O2 when the equation is balanced (using only whole numbers abs the lowest whole number ratio) C2H6O(g)+O2(g)>CO2(g)+H2O(g)

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