5.If.you have 632.grams.of.sugar how.many.moles do yau have?. C2. Hz2 O 6. How many grams do you have of Fe (Iron) if you have 12 moles of Iron? 7.lf you have 15 moles of Fe2 O3 How many molecules do you have? 8. If you have 9.22 x 102 molecules of H20 how many moles do you have ?
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A: 1 mole hydrogen atoms contains 6.023 x 1023 atoms of hydrogen.
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- 2 SO2 + O2 -> 2 SO3 If you have 12.5 grams SO2 and 2.50 grams O2, then calculate the nunber of moles of SO2 using the sample and calculate the number of O2 in the sample. Use dimensional analysis.Calculate the percent by mass of S in each of the following compounds Part A. C2H6SO, dimethylsulfoxide, topical anti- inflammatory Part B. C10H10N4O2S, sulfadiazine, antibacterial Express your answer using four significant figures.Calculate the mass in grams for each of the following Part A. 6.40x1022 molecules of dinitrogen trioxide, N2O3. Express your answer to three significant figures and include appropriate units. Part B 3.68x1021 formula units of potassium dichromate, K2Cr2O7.
- A hydrated salt is 21% water (anhydrous formula weight is 136.1). a. How many grams of water would be in 100 g of the hydrate? b. How many grams of anhydrous salt would be in 100 g of the hydrate? c. How many moles of the anhydrous salt would be in 100 g of the hydrate?Calculate the percent by mass of S in each of the following compounds Part A. Na2SO4, sodium sulfate Part B. Li2S, lithium sulfide Part C. SO, sulfur monoxide Part D. C2H6SO, dimethylsulfoxide, topical anti-inflammatory Part E. C10H10N4O2S, sulfadiazine, antibacterial Express your answer using four significant figures.How many moles of Zn(NO3)2 are produced from 32.20 grams of AgNO3 and excess Zn? Round your answer to three digits after the decimal point. Zn + 2 AgNO3 à 2 Ag + Zn(NO3)2
- The mole is a counting number that allows scientists to describe how individual molecules and atomsreact. If one mole of atoms or molecules is equal to 6.022 × 1023 atoms or molecules, how many moleculesare in a 23.45 g sample of copper (II) hydroxide, Cu(OH)2? (MM of Cu(OH)2 is 97.562 g/mol) Expressyour answer to the correct number of significant figures and you must show all work in the form ofdimensional analysis as shown in Lesson 4. You must solve the problems as they are taught in the course. 4.2 Counting particles of matter. Grams to moles of Copper Hydroxide to molecules of Copper Hydroxide.A compound is 40.0% C, 6.70% H, and 53.3% O by mass. Assume that we have a 100.-g sample of this compound. The molecular formula mass of this compound is 240 amu . What are the subscripts in the actual molecular formula? Enter the subscripts for C, H, and O, respectively, separated by commas (e.g., 5,6,7).C5H12(l) + 8 O2 (g) --> 6 H2O (g) + 5 CO2 (g) How many moles of CO2 will be produced by 53.9 grams of C5H12 ? Round your answer to 2 decimal places.
- Aluminum hydroxide is used as a deodorant and sometimes an antacid (something that prevents acid build up in the stomach). A tablet of antacid is found to have 4.33 x 1023 atoms of oxygen in the tablet, how many grams of aluminum hydroxide do you have? So I can understand properly, answer using the COAST template as follows (I will upvote). Collect and Organize What are you solving for? What should be the units of your final answer? Insert answer here. What information are you given? Insert answer here Analyze What information do you need? Insert conversion factors/ equations here How will you connect the information you have and the information you need to solve this problem? (Provide a unit plan) Insert unit plan here Solve Solve the problem. Be sure to show all units and write clearly. Insert answer here. Think Does your answer make sense? How do you know? Insert answer here Thank youHow many grams of Al2(CrO4)3 (HINT: F.M. = 401.96) would be required to obtain 12.00 g of oxygen?Place your answer in the box. For your calculation, use molar masses that have been rounded to the closest hundredths of a gram (two places to the right of the decimal point). Express your answer using only a number or numbers without text. Report your result in decimal notation and to the proper number of significant figures. All numbers are measured.Use the information and examples provided in the Exploration to calculate how many moles of CaCl2•2H2O are present in 1.50 g of CaCl2•2H2O and then calculate how many moles of pure CaCl2 are present in the 1.50 g of CaCl2•2H2O. Record the answers in Data Table 1. Use the information and examples provided in the Exploration (and values input into Data Table 1, in step 8) to determine how many moles of Na2CO3 are necessary to reach stoichiometric quantities. From that calculation, determine how many grams of Na2CO3are necessary to reach stoichiometric quantities.