ally.* Question Completion Status:QUESTION 1During the experiment, the mass of original sample of compound was 2.965 g, and the mass of copper obtained was 1.006 g.Based on these numbers, calculate the mass of chlorine in the original sample in grams. Include the unit and three decimal places in your answer.QUESTION 26.If 1.045 g of copper was obtained in the experiment, how many moles (mol) of copper is this?Include the unit and five decimal places in your answer.QUESTION 3During the experiment, a student calculated the mass of chlorine in the compound to be 1.186 g. How many moles (mol) of chlorine are in theSave All AnswersClick Save and Submit to save and submit. Click Save All Answers to save all answers.DELLII Ch xyA compound is composed of 39 X b mass of aluminum - Bingtps://blackboard.indstate.edu/webapps/assessment/take/launch.jsp?course_assessment_id%3 397704 1&course_id%3 175505_1&content_id%3D 5438547 18&s... * @* Question Completion Status:QUESTION 4A compound containing copper and chlorine contains 0.01047 moles of copper and 0.01802 moles of chlorine. Calculate the ratio of moles of4 pointsSave Answerchlorine to moles of coppermol CImol CuRound your answer to two decimal places. Do NOT include units. Your number should be greater than 1.QUESTION 54 pointsSave Answermol CIAssume that the ratio of moles of Cl to moles of Cuis equal to 3.09.mol CuIf we represent the formula by CuCly, what is the value for x?Round your answer to the nearest whole number. Do NOT include units. For example, if you determine the formula is CuCle6, enter "6"6 pointsSave AnswerQUESTION 6Assume the copper was not thoroughly dried in Step 7.How will the following measurements/calculations be affected?The mass of copper (measured in Step 9) will be too low or too high (type in the correct answer).The calculated moles of copper will be too low or too high (type in the correct answer).Save and SubmtThe calculated mass of chlorine will be too low or too high (type in the correct answer).Save All Answers540 PM10/7/2020Click Save and Submit to save and submit. Click Save All Answers to save all answers.

Since,Mass of original sample of compound = mass of copper obtained +mass of chlorine in the…

QUESTION 1 During the experiment, the mass of original sample of compound was 2.965 g, and the mass of copper obtained was 1.006 g. Based on these numbers, calculate the mass of chlorine in the original sample in grams. Include the unit and three decimal places in your answer. QUESTION 2 If 1.045 g of copper was obtained in the experiment, how many moles (mol) of copper is this? Include the unit and five decimal places in your answer.

QUESTION 1 During the experiment, the mass of original sample of compound was 2.965 g, and the mass of copper obtained was 1.006 g. Based on these numbers, calculate the mass of chlorine in the original sample in grams. Include the unit and three decimal places in your answer. QUESTION 2 If 1.045 g of copper was obtained in the experiment, how many moles (mol) of copper is this? Include the unit and five decimal places in your answer.

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter3: Molecules, Moles, And Chemical Equations

Section: Chapter Questions

Problem 3.112PAE: 3.112 In one experiment, the burning of 0.614 g of sulfur produced 1.246 g of sulfur dioxide as its...

See similar textbooks

Similar questions

Zinc and magnesium metal each reacts with hydrochloric acid to make chloride salts of the respective metals, and hydrogen gas. A 10.00-g mixture of zinc and magnesium produces 0.5171 g of hydrogen gas upon being mixed with an excess of hydrochloric acid. Determine the percent magnesium by mass in the original mixture.
Which of the postulates of Dalton’s atomic theory explains why we can calculate a theoretical yield for a chemical reaction?
(For Exercises 4546) Solutions containing nickel(II) ion are usually bright green in color. When potassium hydroxide is added to such a nickel(II) solution, a pale-green fluffy solid forms and settles out of the solution. The fact that a reaction takes place when potassium hydroxide is added to a solution of nickel(II) ions is an example of a properly. . The fact that a solution of nickel(II) ion is bright green is an example of a property.
The Statue of Liberty in New York harbor is made of 2.00 105 lb copper sheets bolted to an iron framework. Calculate the mass and the amount of copper in the statue (1 lb = 454 g).
3.112 In one experiment, the burning of 0.614 g of sulfur produced 1.246 g of sulfur dioxide as its only product. In a second experiment run to verify the outcome of the first, a sample was burned and 0.813 g of sulfur dioxide was obtained, but the student running the experiment forgot to determine the initial mass of sulfur burned. Describe how the data already obtained could be used to calculate the initial mass of the sulfur burned in the second experiment.
Consider the equation 2A + B . A2B. If you mix 1.0 mole of A with 1.0 mole of B, what amount (moles) of A2B can be produced?
29. For items 29 - 32, please refer to the following chemical equation:CuC12 + 2 NaNO3 - Cu(NO3)2 - 2 NaCI. If 12 grams of copper (II) chloride react with 20 grams of sodium nitrate how much sodium chloride can be formed? A. 10 g NaCi B. 11 g NaCI C. 15 g NaCl D. 20 g Naci 30. For items 29 - 32, please refer to the following chemical equation:CuC12 + 2 NaNO3 - Cu(NO3)2 - 2 NaCI. What is the limiting reagent? * O A. Copper (Il) chloride B. Copper (II) nitrate C. Sodium chloride D. Sodium nitrate 31. For items 29 - 32, please refer to the following chemical equation:CuC12 + 2 NANO3 - Cu(NO3)2 - 2 Naci. What is the excess reagent? A. Copper (II) chloride B. Copper (II) nitrate C. Sodium chloride D. Sodium nitrate 32. For items 29 - 32, please refer to the following chemical equation:CuCi2 + 2 NANO3 - Cu(NO3)2 - 2 Nacl. How much of the excess reagent is left over in this reaction? O A. 3 g В. 5g C.79 D. 8 g
An unknown compound comprised of osmium and chlorine is 40.11% osmium by mass. a. If you assume 100.0 g of the compound, what is the mass in grams of osmium that are present in the compound? b. How many moles of osmium are present in 100.0 g of the compound? c. If you assume 100.0 g of the compound, what is the mass in grams of chlorine that are present in the compound? d. How many moles of chlorine are present in 100.0 g of the compound? e. Determine the empirical formula of the unknown compound. f. What is the IUPAC name of the compound?
The amounts of two elements X and Y in three samples of an unknown substance are as follows: 10.0 g X and 10.0 g Y in Sample 1 18.0 g X and 12.0 g Y in Sample 2 6.0 g X and 2.0 g Y in Sample 3 What is this substance? Hint: Compare the percentages of Y (or X) in each sample. Are these percentages of Y the same or different? I will say that in sample 1 the percentage of Y is 50 %. likely a mixture likely a compound likely an element either a compound or an element, but cannot be a mixture
1.308g of an organic compound containing carbon, hydrogen, and oxygen was analyzed by combustion analysis. 1.797g of carbon dioxide and 1.471g of water vapor were produced. What is the compound's empirical formula? Enter a number in each space. Answers must be numerical - for example, enter "1" not "one".
B. TRUE OR FALSE: Read each statement carefully. Write TRUE if the statement is correct and FALSE if the statement is incorrect. 6. It is important to know the chemical formula of compound in order to calculate its percentage composition _7. Percentage composition describes the actual number of atoms of each element in a given compound _8. The percent by mass of a compound can be computed using this formula, (mass of an element per mole/molar mass of compound) x 100 _9. You can use percent composition to get the number of grams in a given compound. 10. Percent composition determine the amount (in percent) of each element present in a compound. C. Solve the given problem. Write your calculations on the provided answer sheet. Paracetamol (C3H,NO2) an organic compound made up of C, H, O and N. It is a common medicine to treat fever and pain because it is an anti-inflammatory drug. Determine the elemental percentage composition of a paracetamol.
35. Calculate the mass in grams of each of the following samples. a. 1.25 moles of aluminum chloride b. 3.35 moles of sodium hydrogen carbonate c. 4.25 millimoles of hydrogen bromide (1 millimole = 1/1000 mole) d. 1.31 × 10–3 moles of uranium e. 0.00104 mole of carbon dioxide f. 1.49 × 10² moles of iron