This data table is given find the atoms of each element and the total number of atoms in each substance. Data Table   H2O(l) NaCl(s) CaCO3(s) Name of substance Water  Sodium Chloride  Calcium Carbonate Mass of substance (g) 4.19g 8.11g 2.69g Molar mass (g/mol) 18g 58g 100g Moles of each compound 0.23 0.13 0.0269 Moles of each element H=0.46 O=0.23 Na=0.13 Cl=0.13 Ca= 0.269 C=0.0269 O=0.807 Atoms of each element     Total number of atoms in a substance

Aqueous hydrobromic acid (HBr) reacts with solid sodium hydroxide (NaOH) to produce aqueous sodium bromide (NaBr) and liquid water (H₂O). If 1.90 g of water is produced from the reaction of 35.6 g of hydrobromic acid and 7.39 g of sodium hydroxide, calculate the percent yield of water. Round your answer to 3 significant figures. ☐% X

How many grams of NaCl can be produced from 9 grams of Na? • 2Na + Cl2 –> 2NACI Calculate the final answer using the set up. (Hint: Multiply the fractions) 9g Na x 58.949 Nacl Imoi NaCl I mol Na 2 mol Nacl %3D 22.99g Na 2 mol Na O 1051.92 g O 9g O 58.44 g O 22.87 g

9.00 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar mass of 150. g/mol, is burned completely in excess oxygen, and the mass of the products carefully measured: product carbon dioxide 13.20 g 5.40 g Use this information to find the molecular formula of X. 10 mass water 00 S

0₂ Use the References to access important values if needed for this question. Sample Molecular formula: Furnace H₂O absorber CO₂ absorber A 8.946 gram sample of an organic compound containing C, H and O is analyzed by combustion analysis and 11.35 grams of CO2 and 3.098 grams of H₂O are produced. In a separate experiment, the molar mass is found to be 104.1 g/mol. Determine the empirical formula and the molecular formula of the organic compound. (Enter the elements in the order C, H, O.) Empirical formula:

O Chemical Reactions Theoretical yield of chemical reactions 1/3 Gaseous methane (CH4) reacts with gaseous oxygen gas (O2) to produce gaseous carbon dioxide (CO2) and gaseous water (H2O). What is the theoretical yield of water formed from the reaction of 0.48 g of methane and 0.60 g of oxygen gas? Round your answer to 2 significant figures. A g X

Identify which of the following substances has the amount equivalent to ONE mole. O 6.22 x 1023 oxygen atoms O 58.93 g copper metal O 28.02 g nitrogen gas O 24.31 g manganese O 10.00 g of water

For the following balanced equation:  CH4 + 4 Cl2 ==> CCl4 + 4 HCl Determine the number of moles of HCl that  can be made from 6.80 moles of CH4? Answer to 2 decimal places.

Gaseous methane CH4 reacts with gaseous oxygen gas O2 to produce gaseous carbon dioxide CO2 and gaseous water H2O. If 4.36g of water is produced from the reaction of 8.82g of methane and 10.6g of oxygen gas, calculate the percent yield of water. Be sure your answer has the correct number of significant digits in it.

Stoichiometric coefficients are used to describe the mole ratio. 3 ny O True = False