Methane CH is a simple organic molecule that is used as a fuel—it is the major component of natural gas. The bottom of the ocean contains large amounts of methane hydrate (also called methane ice or methane clathrate), enough that it has been suggested as a major source of fuel. The methane hydrate contains 6 moles water for each mole of methane. What percentage of methane hydrate is methane? What percentage is water?

Methane CH is a simple organic molecule that is used as a fuel—it is the major component of natural gas. The bottom of the ocean contains large amounts of methane hydrate (also called methane ice or methane clathrate), enough that it has been suggested as a major source of fuel. The methane hydrate contains 6 moles water for each mole of methane. What percentage of methane hydrate is methane? What percentage is water?

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter2: Chemical Formulas, Equations, And Reaction Yields

Section: Chapter Questions

Problem 46AP

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Methane CHis a simple organic molecule that is used as a fuel—it is the major component of natural gas. The bottom of the ocean contains large amounts of methane hydrate (also called methane ice or methane clathrate), enough that it has been suggested as a major source of fuel. The methane hydrate contains 6 moles water for each mole of methane.What percentage of methane hydrate is methane? blank1 - Numeric Answer % What percentage is water? blank2 - Numeric Answer %
Initial Temp of HCl: 22.96 C Final Temp of HCl: 28.30 C Moles of HCl: .05 moles Moles of NaOH: .05 moles Cs water: 4.184 J/g C Accepted delta Hrxn: -55.8 kJ/mol 1. what is the qwater. pls include formula. 2. calculate delta Hrxnn using the moles, temp and cswater 3. calculate delta Hrxn % error
Show work using conversion factors Answer key: #37d 1.250 moles CO2 #37e 4.92 mole HCl #37f 7.1422 moles HCl ( fixed 10/14/2020) #37g 143 g CO2
Show work using conversion factors Answer Key:#37a CaCO3 + 2HCl --> CaCl2 + H2O + CO2 #37b 36.46 g/mol HCl #37c 100.09 g/mol CaCO3 #37d 1.250 moles CO2 #37e 4.92 mole HCl #37f 7.1422 moles HCl ( fixed 10/14/2020) #37g 143 g CO2
One quick follow up...this works well with adding 13 moles. Do you use the same math if fewer or more moles were added? For exampl, what if 5 moles of AB2+ were added? Or 20 moles of AB 2+ were added?
What is ΔHof of Al2S3(s)? 2Al2S3(s) + 9O2(g) → 2Al2O3(s) + 6SO2(g) ΔHo = -3684.2 kJ ΔHof Al2O3(s) = -1675.7 kJ/mol ΔHof SO2(g) = -296.8 kJ/mol
(atk) Solve all with the appropriate number of sigfigs 1) 10−10.14/4.37 2) ln(27.9) 3) (30.45 + 43.249) × (0.0261 − 0.007) 4) (102.33 atm)(6.91 L)/(8.206×10−2 L⋅atmK⋅mol)(376.0 K) into __________ moles
For the following table fill in the missing values and calculate the theoretical yield. A + 2B à C moles 0.00242 0.00242 ?_________ MW ?_________ 98.06 164.16 g ?_________ ?__0.00002467_______ ?_________ mL 0.20 d(g/mL) 0.80
So for the question below, I have the answer worked out from class but I don't understand certain steps. For example, why does KiCi+KaCa / KaCa = 4.50 become KiCi/KaCa + KaCa/KaCa = 4.50 ? Where does the second KaCa come from? Next, you cancel values and get 1 + Ka,i(Ci/Ca) = 4.50 -- in this step where does the one come from? Glutathione is an important antioxidant found in plants and animals. You are measuring glutathione in blood, but the analysis is complicated by many potential interferents including ascorbic acid. In one of your studies, you analyze a solution of 10.0 ppb glutathione and 1.5 ppb ascorbic acid, the signal was 4.50 times greater than the signal you measured for sample containing only 10.0 ppb glutathione. What is the selectivity coefficient for this analysis?
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.
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.
On strong heating ammonia dissociates into nitrogen and hydrogen, all in a gaseous state. When 0.350 mol of NH3 is heated in a closed 10.0 L vessel, the fraction of dissociation is 0.400. (ensure all calculation have 3 decimal places. a. Calculate moles of NH3dissociated? b. Calculate moles N2 formed? c. Calculate moles H2 Formed?