Kami Export - Postlab Lab 9

8.The number of moles of each compound in a chemical reaction is represented by a ______ a.Supercript b.Subscript c.Coefficient d.Element Symbol

reactant controls the amount of product formed in a chemical reaction? A. excess reactant B. mole ratio C. composition reactant D. Jimiting reactant h of the following would be investigated in composition stoichiometry? A. the volume of neon gas equivalent to a specific number of atoms of neon gas B. the masses of hydrogen and oxygen in water the mass of potassium required to produce a known mass of potassium chloride D. the types of bonds that break and form when acids react with metals 4 L sample of which of the following substances, at STP, would contain Avogadro's number of particles? A. phosphorus B. mercury C) sodium D. nitrogen termination of the amount of sulfur and oxygen in the compound sulfur dioxide would be involved in which of calculation? A reaction stoichiometry B. percent composition C. limiting reactant D. composition stoichiometr ch of the following would NOT be studied in the branch of chemistry called stoichiometry? A. the mole ratio of aluminum and chlorine in…

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The subscripts in a chemical formula are the number of A. reactants © B. molecules C. atoms D.moles of a particular atom in one mole of the molecule.

B. Formula of a Hydrate 23.43 29.24 26.31 26.28 1. Mass of crucible 2. Mass of crucible and hydrate 3. Mass of crucible and anhydrate 3a. Mass of crucible and anhydrate (second heating) Calculations 4. Mass of hydrate 5. Mass of anhydrate 6. Mass of water lost

help  please answer in text form with proper workings and explanation for each and every part and steps with concept and introduction no AI no copy paste remember answer must be in proper format with all working

expected mass calcium carbonate? percent yield??

A 1.00 g sample of potassium bicarbonate is decomposed by heating. If the resulting potassium carbonate weighs 0.735 g and the calculated yield is 0.690 g, what is the percent yield? General Exercises Percent yield= ____%

Which reactant controls the amount of product formed in a chemical reaction? A. Actual yield  B. Excess reactant  C. Limiting reactant  D. Mole ratio

Directions: Read and understand each item and choose the letter of the correct answer. Use separateanswer sheet of paper. 1. Which of the following is TRUE of a balanced equation?A. The total number of atoms remains the same.B. The kinds of atoms remain the same.C. The total number of molecules remains the same.D. The number of atoms of each element remains the same. 2. Which of the following is true of a chemical reaction?A. Only physical changes occur. C. Only changes of state occur.B. New substances must form. D. Chemical properties remain the same. 3. Which is not a type of chemical reaction?A. Combination C. decompositionB. Substitution D. evaporation 4. The electrolysis of water into hydrogen and oxygen is an example of ______ reaction.A. Combination C. double replacementB. Decomposition D. single replacement 5. What scientific law is explained using balanced chemical equations?A. Law of chemical reactions C. law of conservation of massB. Law of conservation of energy D. law of…

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Use your data to determine the experimental mole-to-mole ratio between sodium carbonate and sodium chloride. Show your work for each step a)Convert the mass of sodium carbonate used to moles. b) Convert the mass of sodium chloride collected to moles. c) Divide both of your results from the preceding two steps by the lower mole value to determine the simplest mole-to-mole ratio between sodium carbonate and sodium chloride. Simplest mole ratio before rounding _____________________moles Na2CO3 : _________________ moles NaCl Simplest whole number mole ratio after rounding ____________________moles Na2CO3 : _________________moles NaCl

1. A student collected the following data during Lab: Mass of MgCO3 hydrate = 0.9987 g. Constant mass of anhydrous MgCO3 = 0.4831 g How many moles of water were in the MgCO3 hydrate?  2. A student uses gravimetric determination to find the water of hydration of a hydrated sample of cobalt (II) sulfate. The student’s sample contained 0.0098459 moles of anhydrous cobalt(II) sulfate (CoSO4) and 0.068921 moles of water (H2O). What is the formula of the cobalt(II) sulfate hydrate?  3. A student has a sample of CaSO4 hydrate and it weighs 0.4813 grams. He heats it strongly to drive off the water of hydration, and after subsequent heatings, the student finds the anhydrous compound has a constant mass of 0.3750 grams. Find the formula of the hydrate.

Percent Yield

Stoichiometry Instructions: Complete the following questions and hand in at the start of your lab period or when instructed by your instructor. Show your work with units and correct significant figures for all questions that involve a calculation. 1. Calculate the molecular weights of all the compounds in the reaction we are doing in this lab (and copy them onto your procedure... they will be helpful!): a. NaHCO3 b. HCI c. NaCl d. H₂O e. CO2 2. The following is some example data for the lab. Use the data to answer the following questions. Mass of test tube and boiling chip Mass of test tube, boiling chip and NaHCO3 Mass of test tube, boiling chip and NaCl a. How much NaHCO3 was added to the test tube? 14.123 g 14.724 g 14.496 g b. How many grams NaCl was produced from the experiment? c. Using the balanced chemical equation, the amount of limiting reactant calculated above, and molar masses from question 1, how many moles of NaCl should the experiment have produced? d. Calculate the…