The equation that shows the formation of water from the elements that makes it up supports the law of conservation of massbecause...2 H₂(g) + O₂(g) → 2 H₂O(g)A the number of moles of hydrogen and oxygen is equal to the number of moles of water.B atoms of the elements hydrogen and oxygen react to form molecules of the compound water.C) atoms of the elements hydrogen and oxygen are in the reactants and also in the products.D) the mass of the hydrogen and oxygen is equal to the mass of water.Ethe same number of moles of elements, six, is on both sides. A sample of carbon dioxide is analyzed and determined to be 27.3% by mass carbon. If a 50.0 g sample of carbon dioxide isanalyzed, how many grams should be carbon?A 27.3 gB 22.7C) 36.3 gDE13.7 gnot enough information to determine

Consider a compound AB Percent of A = (Mass of A/Mass of AB) x 100 Law of conservation of mass:…

A sample of carbon dioxide is analyzed and determined to be 27.3% by mass carbon. If a 50.0 g sample of carbon dioxide is analyzed, how many grams should be carbon? (A) 27.3 g B) 22.7 C) 36.3 g (D) 13.7 g E not enough information to determine

A sample of carbon dioxide is analyzed and determined to be 27.3% by mass carbon. If a 50.0 g sample of carbon dioxide is analyzed, how many grams should be carbon? (A) 27.3 g B) 22.7 C) 36.3 g (D) 13.7 g E not enough information to determine

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Which of the following is a molecular compound? (a)NaCl (b) NaOH (c) FePO4 (d) LiF (e) H2O
Which of the following samples of matter would have the largest mass (grams)? Highlight the letter of your answer. Support your answer with calculations. a) 1.25 x 1023 molecules of Br, b) 48.0 Liters of C,0 gas c) 0.478 moles of XeF, gas
2. 5.88 g of hydrated calcium chloride CaCl,•xH,O is treated with excess K2SO4 in a double replacement reaction to yield 5.44 g anhydrous CaSO4 after heating. a) Write down the balanced double replacement reaction. (Refer to question 1a.) b) Calculate the number of moles of anhydrous CaSO4 produced. c) Calculate the number of moles of CaCl,•XH2O used. d) Calculate the molar mass of CaCl2•xH2O. e) Determine the value of x in CaCl,*XH2O.
9)
6) Chlorophyil has the formula Cs5 H72 Mg N4 O5. How many grams of carbon are required to combine with 0.0011g of Mg? ?[ Mg = 24.3, C = 12.0 g/mol]
A 1.95 mg sample of a compound containing carbon, hydrogen, and oxygen underwent combustion producing 4.42 mg of CO₂ and 1.81 mg of H₂O. What is the empirical formula of the compound? (Type your answer using the format CxHyOz for the compound CxHyO₂) CH20 HopHelpCh3N7 (b) A compound is composed of elements C, H, and N. A 6.300-mg sample of the unknown compound was combusted, producing 17.090 mg of CO₂ and 4.900 mg of H₂O. What is the empirical formula for this compound? (Type your answer using the format CxHyNz for the compound CxHyNz) HopHelpCh3N8 If the compound has a molar mass of 160 ± 5 g/mol, what is its molecular formula?
2.5 66 y 46 Hydrates 4) A 5.000 g sample that contained NaCl and BaCl2 2H20 was heated. After heating the sample had a weight of 4.588 g. What is the percent Nacl in the sample?
H. H. Three moles of the compound in the figure above would weigh how many grams? (The atomic masses, in daltons, are approximately 12 for carbon, 1 for hydrogen). O=U エーO CH
9. What is the amount of oxygen in 200.0 mg of an unknown compound, if 100.0 g of the compound contains 49.93 g O? (A) 0.02497 g (C) 24.98 g (B) 0.09986 g (D) 99.86 g 10. What is the thickness of 5.79-mg of gold leaf evenly spread over an area of 44.6 cm² ? (Density of gold is 19.3 g/cm³.) (A) 6.73 x 10-6 cm (C) 6.73 x 10³ cm (B) 1.20 × 10³ cm (D) 2.78 x 102 cm
A hydrocarbon has a MW of 114 g/mol and has a composition of carbon 84.06% and hydrogen 15.94%. What is its (a) empirical formula (b) true formula? Enter the empirical formula in the first box and the molecular formula in the second box. Enter the elements in the order of CH with the appropriate number for each element. If only 1 of an element is necessary leave the 1 off. Example: C6H12O6 If only one of a particular element is needed DO NOT type 1. Example: CO2 NOT C102
Consider a 101.3 g sample of the compound manganese(IV) perchlorate. (d)Using the formula Mn(ClO₄)₄ (MM = 452.74), what is the percent by mass of Cl in the compound? (e)how many moles of manganese perchlorate are in 101.3g? (f)How many moles of oxygen are in 101.3 g of manganese perchlorate
A 3.000 g sample of a gaseous compound was found to contain 2.560 g of carbon and 0.440 g of hydrogen. A) What is the simplest formula of the compound (Write C first and then H)? You won't be able to make the numbers a subscript. For instance, for MgCl2 enter MgCl2. B) The molar mass of the compound was found to be 42.08 g/mol. What is the molecular formula of the compound? You won't be able to make the numbers a subscript. For instance, for MgCl2 enter MgCl2.