CALCULATIONS Answer the following in Question 1-2 involves the same process three different times. Questions 3-9 are four-fold repetitive. Repeat these calculations for each of the four individual trials. Because of the repetition, you should collect your work in the data tables provided. Make sure to show all your work and label all calculations carefully. 1. Convert the mass of NaHCO3 in each test tube of the Avogadro's Law experiment into moles of NaHCO3. 2. How many moles of CO₂ gas are expected to form from each of the balloon reactions? Hint: HC₂H302(aq) + NaHCO3(s) → NaC₂H302(aq) + H₂O(1) + CO₂(g) 3. Use Table 3 of the partial pressures from page 4 of the introduction in the student handout and the temperature of the lab to find the PH₂O. 4. Use Dalton's Law of partial pressures, the barometric pressure, and the PH₂O to calculate the PH₂. [PH₂= Ptotal - PH₂0] 5. Use the Ideal Gas Law with PH2, VH2, TH₂ and the gas constant R to calculate the moles of hydrogen, n H₂. 6. Us

CALCULATIONS Answer the following in Question 1-2 involves the same process three different times. Questions 3-9 are four-fold repetitive. Repeat these calculations for each of the four individual trials. Because of the repetition, you should collect your work in the data tables provided. Make sure to show all your work and label all calculations carefully. 1. Convert the mass of NaHCO3 in each test tube of the Avogadro's Law experiment into moles of NaHCO3. 2. How many moles of CO₂ gas are expected to form from each of the balloon reactions? Hint: HC₂H302(aq) + NaHCO3(s) → NaC₂H302(aq) + H₂O(1) + CO₂(g) 3. Use Table 3 of the partial pressures from page 4 of the introduction in the student handout and the temperature of the lab to find the PH₂O. 4. Use Dalton's Law of partial pressures, the barometric pressure, and the PH₂O to calculate the PH₂. [PH₂= Ptotal - PH₂0] 5. Use the Ideal Gas Law with PH2, VH2, TH₂ and the gas constant R to calculate the moles of hydrogen, n H₂. 6. Us

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Hello can you please help me answer this
Assume that your empty crucible weighs 15.98 g, and the crucible plus the sodium bicarbonate sample weighs 18.56 g. After the first heating, your crucible and contents weighs 17.51 g. After the second heating, your crucible and contents weighs 17.50 g. Answer the following questions based on this information.
Completion Your answers are saved automatically. Remaining Time: 22 minutes, 58 seconds. v Question Completion Status: A Moving to another question will save this response. Question 10 Consider the combustion of propane (C3H3), shown in the chemical equation below: 1 C3H3 + 502 → 3 CO2 + 4 H,0 How many molecules of 02 are needed to fully react with 97 molecules of propane? A Moving to another question will save this response. tech.edu/webapps/blackboard/content/listContent.jsp?course_id%=_455765_1&content_id=_17790076_1&mode=reset M
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Thank you for your explanation, I'm however confused by the multiplication of each. For example, the first one mentions x 3 to CuBr2 and x 2 to AlBr3, this process of cancelling out to create even moles is the balancing? I also wanted to know what the proper classification was for those three you answered? I felt like I had the first two wrong, I wasn't sure if they were single or double replacement.
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LAB 8 Pre-Lab Questions portions of lab adapted from various online and reference sources 1. Fill in the missing parts of this chemical equation. Remember that a chemical with a dot in the middle is called a hydrate. The arrow means that heat will be applied, which will drive off the water from the hydrate. No physical states needed, but your final answer should be balanced. CuSO4.5H2O -> CUSO4 + 2. Calculate the molar mass of the hydrate ZnSO4.7H₂O. 3. A student took 4.92 g of hydrated magnesium sulfate crystals (MgSO4 xH₂O), but didn't write down how many water molecules were attached, hence "x." a. Write a balanced chemical equation that shows a decomposition of this molecule if we were to apply heat. No physical states needed, but your final answer should be balanced (you can use x in balancing). b. The student heated the hydrate. Once heating was complete, the dish had 2.40 g of dried magnesium sulfate. How much water in grams did the student drive off from heating? Show work. c.…
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Consider the reaction below. A student takes 53.12 grams of Fe and mixes it with 37.12 grams of S – then they heat the mixture to cause the reaction to occur. Use math and words to prove which of these reagents is the limiting reagent in that reaction.