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

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.

What factors during the reducing bezil experiment caused the percent yield to be different than 100%? What impurities may be present in the final product and how does that effect the percent yield determination?

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.…

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.

Write a balanced chemical equation for each of the following.  Express your answer as a chemical equation. Identify all of the phases in your answer.   a. Solid lead(II) sulfide reacts with aqueous hydrochloric acid to form solid lead(II) chloride and dihydrogen sulfide gas. b. Gaseous carbon monoxide reacts with hydrogen gas to form gaseous methane (CH4) and liquid water.         c.Solid iron(III) oxide reacts with hydrogen gas to form solid iron and liquid water.         d.Gaseous ammonia (NH3) reacts with gaseous oxygen to form gaseous nitrogen monoxide and gaseous water.

5 g of hydrated barium chloride is heated in a crucible until the mass of the sample no longer changes. The mass of the sample after heating is 4.26 g. Assume that the mass lost during the heating is solely due to the loss of water from the sample. What percentage of water was contained in the barium chloride hydrate?

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.

Predict the products of the reaction below. That is, complete the right-hand side of the chemical equation. Be sure your equation is balanced. HI + NaOH → I Don't Know 1841 Submit 3 E 5 T 6 G 0-0 X S stv♫ 5 © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Cer A all 9 zoom

Calculate the percentage by mass of magnesium in magnesium sulphate (MgSO4). 24 +32 + 16 x4 = 120. %3D