Experiment 2 Determination of a Chemical Formula(1) (2)

How do you solve question 2?

50 Name: Date lab performed: Partner(s) name: Date due: Balancing Chemical Reactions A. BALANCING EQUATIONS: Balance each of the chemical equations. Coefficients of 1 shouldn't be written. 1. C6H14 CO: +_H:0 2. CoH O2 CO 3. Zn + _HCI +_ZnClz +_H: 4. P. +_Cl2 PCl, PCI3 5. NaHCO, _Na:CO +_CO: CO: H20 6. ΗΝΟ, NO2 _H2O O2 7. Fe + Fe;O3 8. _CaC: Ca(OH): + C;H; 9. _MgiN: H:0 NH Mg(OH): 10. CaCO, _HCI CaCl; + CO: : +H;O H:0 11. Zn + H,PO. → Znj(PO.): H2 12. AGNO +_ +ABCI + _Ca(NO:)a 51 13. Al:O H2SO4 Al:(SO)) H:SO. _H:0 14. Fe + Brz FeBr 15. Al(OH)s + H;SO. Al:(SO.)s H:0 16. C:H: CO: H20 -> 17. Li:0 + _H:0 LIOH 18. NH _H:CO (NH.):CO, 19. C:HSOH + O: CO: +_H:0 20. H3PO, + Ca(OH): → Cas(PO4): H:0

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I'm stuck on step 3. find the formula - Divide each by the smallest number to get while number ratio for the formula  With the information I've provided under attachments can you help? I don't know how to calculate the smallest number to get the ratio for the formula.

ure X R Module 7B - Stoic x G molar mass of cal X O stemble O Learning why can X O Clear Oval Hous es/228/assignments/389/tasks/302 ps 8/18 tasks attempted Determine the molecular and empirical formulae for the two molecules shown below: CI Cl H. H H–Si- Si-H H-C H H H H H. Please Note: Chemical notation is case sensitive Please Note: Chemical notation is case sensitive Molecular Formula Enter your chemical notation here Enter your chemical notation here Please Note: Chemical notation is case sensitive Please Note: Chemical notation is case sensitive Empirical Formula Enter your chemical notation here Enter your chemical notation here SAVE RESPONSE 1 2 3 16 17 18

People Tab Window Help /0/index.html?deploymentld%=55750828934189288909969212&elSBN=978130565 NDTAP Use the References to access important values if needed fo An experiment requires that enough PNF, be used to yield 19.0 g of fluorine. How much PNF, must be weighed out? g Submit Answer 5 question attempts remaining

What is the answer for question 9?

Could you please help me with this question? It is broken up into 3 parts and I’m having a hard time. I have attached a picture below.

Use the References to access important values if needed for this question. Determine the molecular and empirical formulas for the substance shown in the ball-and-stick model below. C = black H=gray Molecular Formula In progress Empirical Formula Submit Answer Retry Entire Group 3 more group attempts remaining Previous Email Instructo Cengage Learning | Cengage Technical Support Q Search Bing %24 % & 5 7 8. R Y U F.

marks Profiles Tab Window Help X Worl X v.pdf Para X Gran X eAssignment/takeCovalentActivity.do?locator=assignment-take Submit Answer My x SEP 14 Use the References to access important values if needed for this question. OWL X How many grams of Se are there in a sample of Se that contains the same number of moles as a 65.8 gram sample of Sn? grams of Se Retry Entire Group tv How X I BWha X GWhax + ₁ 口 9 more group attempts remaining Previous Next Show All X C

mmunity College X x || X D2L ALEKS Learning Module 8 (due A X A ALEKS- Jessica Sceusa - Learn X G Write the empirical formula for a x + www-awu.aleks.com/alekscgi/x/Isl.exe/1o_u-IgNslkr7j8P3jH-lvWyv8WYLP6W0cqJcWJdIACROQwyw24GWHInCX70-Q0WaoxQiZ3DF-1EgBJkRS45QbFh_mdu6pQMT19A08TrT_6p5Ces O ||| O STATES OF MATTER Using the combined law gas Student - Home kPa For many purposes we can treat ammonia (NH3) as an ideal gas at temperatures above its boiling point of -33. °C. Suppose the temperature of a sample of ammonia gas is lowered from 19.0 °C to -25.0 °C, and at the same time the pressure is changed. If the initial pressure was 0.30 kPa and the volume decreased by 40.0%, what is the final pressure? Round your answer to 2 significant digits. Explanation Check X10 X K 0/5 © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Cent

Part C A sample of propane, C3 H8, contains 15.8 moles of carbon atoms. How many total moles of atoms does the sample contain? Express the total number of moles of carbon and hydrogen numerically. View Available Hint(s) VAD ? moles Submit Provide Feedback Next> P Pearson cation Inc. All rights reserved. | Terms of Use Privacy Policy I Permissions | Contact Us II F8 F9 F11 F6 F7 F10 F12 ) & 9 7 8 1 delete { U P enter K

Results table. To clean up, zoom out from the balance and drag the sample to the red disposal container. Repeat with ammonium chloride (NH4Cl), located on the Salts shelf.                                     C12H22O11                                              NH4ClMass (g)                        1.0481 g                                                  1.0444g  Molar Mass (g/mol)MolesMoles of each elementAtoms of each element Much like the previous calculation, you will use the periodic table to determine the molar massof the compound. The example shown is for sodium chloride, NaCl. The molar mass is the massof 1 sodium (22.98g/mole) and 1 chlorine (35.45g/mole) added together, 58.43g/mole. If theformula shows multiple atoms, as in sugar, you must take that into account. For sugar, it will be12 times the mass of a carbon atom plus 22 time the mass of hydrogen atom, plus 11 times themass of oxygen atoms.The calculation of moles will be similar to that done in the previous…

Help me find the Molar Mass, please?

Sofia 1.00 completely in excess oxygen, and the mass of the products carefully measured: of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar mass of 44. g/mol, is burned product mass carbon dioxide 3.00 g water 1.64 g Use this information to find the molecular formula of X. X Check Tems of Use Explanation O 2019 McGraw-Hill Education. All Rights Reserved. e 99+ Type here to search hp

ents/271356/variants/271356/take/12 Question 11 Fe,0 How many moles of CO will react with 1.75 moles of 2 3? Turn on Show numerical result. Were you correct? Answer in a complete sentence. Problems solved: 0 Show units Show numerical result Flip tile Reset 1.75 mot-Feg0s 3 mol CO = mol CO 1 mot-Fe03 E A H. B IUS

R %S4 Question 11 How many moles of nitrogen are in 267.78 g dinitrogen tetroxide. * Previous LNe Not saved Sub Questions OCT 8. esc F1 .. F2 000 000 F4 .... F3 .... .... F5 .... .... 23 2.

Use the References to access important values if neec A compound is found to contain 46.75 % silicon and 53.25 % oxygen by mass. What is the empirical formula for this compound? To answer the question, enter the elements in the order presented above. Submit Answer Retry Entire Group 3 more group attempts remaining Cengage Learning | Cengage Technical Support

Solve correctly please. Need all a to d parts. (Gpt/ai wrong answer not allowed)

PLS HELP ASAP ON ALL AND SHOW ALL WORK

%30&daunchu h 3, 31-36 3 attempts left Check my work Be sure to answer all parts. The density of water is 1.00 g/mL at 4°C. How many water molecules are present in 2.46 mL of water at this temperature? x 10 molecules Enter your answer in scientific notation. < Prev

Dokmarks * Co Profiles Tab Window Help 3.1 Electrome X 6.2 Determin X Desmos | Scir X Question 8.d of 46 Feet to Mete: X formula for v % Ne A paraffin wax candle is 6.25 inches tall and 1.50 inches in diameter. How many mL of paraffin wax would it take to make a candle of this size, with a volume of 11.0 in ?

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Course X ✓ Macmillan: X Course Mod X ack o/index.html?deploymentid=5735112480241329813180832311&elSBN=9781305862883&id=1707786042&snap: - D 1. How many MOLECULES of xenon trioxide, XeO3, are present in 6.25 grams of this compound? Sections 51 X 2. How many GRAMS of xenon trioxide are present in 4.41x1022 molecules of this compound? Juv References Submit Answer Use the References to access important values if needed for this question. E✓ ✓ ✓ A✓ V ass/Number of Formula Units or Molecules of Compound: This is group attempt 1 of 10 HOMEWORK X 6 3 0 2. How many formula units of potassium nitrite are present in 8.65 grams of this compound? 1: How many GRAMS of potassium nitrite, KNO₂, are present in 2.22x1022 formula units of this compound? Autosaved at 8:07 PM molecules grams MindTap - C Done grams formula units

Chemistry Question 4 of 10 View Policies Show Attempt History Current Attempt in Progress Your answer is partially correct. Calculate the percent composition by mass for Fe(NO3)3. Use the molecular weights to two decimal places in your calculations. a) %Fe - 23.09 b) %N-i 5.718 c)%0- 19.83 eTextbook and Media Hint Save for Later Attempts: 5 of 10 u

be Maps Netflix in other Co... Nhttps://lms.naz.ed... Rochester to Seat... rus What is the mass of one formula unit of calcium cyanide, Ca(CN)2? amu Question #6 t How would you calculate (see below) the number of formula units of Ca(CN)2 of in 7 moles of Ca(CN)2? C V port 7 x formula mass (A) 7 x molar mass (B) 7 x Avogardro's Number (C) 7 7 formula mass (D) molar mass (E) Submit Answers 7 Avogardro's Number (F) McKee Next Previous 60

Part D-Yield Calculations Which of the following errors could cause your percent yield to be falsely high, or even over 100%? Select ALL that apply. Taking the mass of all samples with the lid included. Handling the crucible directly with your hands. Taking the mass of the empty crucible without the lid, but including the lid in all other mass measurements. Heating the sample too vigorously. Failing to completely decompose the sodium bicarbonate sample. Submit Previous Answers Request Answer X Incorrect; Try Again; One attempt remaining Provide Feedback

ople Tab WindoVW p/index.html?deploymentld%355750828934189288909969212&elSBN=97813056575 DTAP Use the References to access important values if needed for A compound is found to contain 43.64 % phosphorus and 56.36 % oxygen by weight. What is the empirical formula for this compound? To answer the question, enter the elements in the order presented above. Submit Answer 5 question attempts remaining

a.) What is the percent composition by mass of each compound? b.) Mass to Mass Stoichiometry Calculation c.) Limiting Reagent d.) Excess Reagent e.) Amount in grams of the excess reagent f.) Percent Yield g.) Number of dosage form and packaging that can be produced from stoichiometric calculation

Quantity 1. Mass of crucible + cover 2. Mass of crucible + cover + Magnesium 3. Mass of Magnesium 4. Mass of crucible + cover + magnesium oxide 5. Mass of magnesium oxide 6. Mass of oxygen that combined with the magnesium 7. Atomic mass of magnesium 8. Atomic mass of oxygen 9. Moles of magnesium 10. Moles of oxygen Subtract # 2 - #1 Subtract #4 - #1 Subtract #4 - #2 From the periodic table From the periodic table Divide #3/#7 (In other words, divide the grams of magnesium by 24.3 to get the moles of magnesium) Your value Find the simplest whole number ratio 11. Empirical formula of magnesium between #9 and # 10. Those whole oxide based on this data numbers become of the subscripts of the formula* 20.00 g 24.86 g 28.06 g 24.3 16.0 moles of Mg Divide #6/#8 (In other words, divide the moles of moles of O oxygen by 16.0 to get the moles of oxygen *For example, if the moles of Mg were found to be 2.0 moles, and the moles of O were found to be 6.0 moles, then you would write the following:…

Part D Calculate the moles of C2 H6 in 3.76x1023 molecules of C2 H6. Express your answer using three significant figures. moles of C2 H6 Submit Previous Answers Request Answer X Incorrect; Try Again; 4 attempts remaining Provide Feedback < Previous

10) Calculate the moles of magnesium ( Show your calculation)

1 How many atoms of vanadium are in 1.28 grams of vanadium? ADD FACTOR x( ) 7.71 x 1023 50.94 3.93 x 1025 g V/mol 6.022 x 10²3 1.28 atoms V gV ANSWER 6.022 x 1024 1000 0.0251 1.51 x 102² mol V kg V RESET 2 1.51 x 1023