Find the mistake. A student calculated their answer to a gas law problem as shown in the image below. Their answer is incorrect. Review their work and find the mistake the student made in their calculation. The question is typed in the upper left corner. Hint: There is only 1 step that is incorrect and the issue IS NOT related to significant figures! Click here for the Gas Laws Formula Sheet. Click here for the Periodic Table. Calcium carbonate decomposes when heated to form calcium oxide and carbon dioxide according to the following chemical equation: 75.0y | Iml Cal3/1mol Coz Ime Catos =0.7493 mol 100.099 CaCO3 - Ca0 + CO2 What volume of carbon dioxide can be produced from 75.0 g of calcium carbonate at a temperature of 25 degrees C and a pressure of 1.25 atm? G-n-0.7493mol, P=1.25 atm, T-ス5C+スフ3こス98R R-8.314 LokPa/mal.K %3D Looking for liters? Start with stoich. E PV =nRT →V= nRT P く,V= 07493 mad L8 3146i と Palmot K) (298K) 1.25 atm S:V-1485,21L

Find the mistake. A student calculated their answer to a gas law problem as shown in the image below. Their answer is incorrect. Review their work and find the mistake the student made in their calculation. The question is typed in the upper left corner. Hint: There is only 1 step that is incorrect and the issue IS NOT related to significant figures! Click here for the Gas Laws Formula Sheet. Click here for the Periodic Table. Calcium carbonate decomposes when heated to form calcium oxide and carbon dioxide according to the following chemical equation: 75.0y | Iml Cal3/1mol Coz Ime Catos =0.7493 mol 100.099 CaCO3 - Ca0 + CO2 What volume of carbon dioxide can be produced from 75.0 g of calcium carbonate at a temperature of 25 degrees C and a pressure of 1.25 atm? G-n-0.7493mol, P=1.25 atm, T-ス5C+スフ3こス98R R-8.314 LokPa/mal.K %3D Looking for liters? Start with stoich. E PV =nRT →V= nRT P く,V= 07493 mad L8 3146i と Palmot K) (298K) 1.25 atm S:V-1485,21L

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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Please help with question d
Calcium metal reacts with phosphoric acid. What mass of precipitate is produced when 29.3 g of calcium reacts with excess phosphoric acid?Hint: Write a balanced chemical reaction equation first.Do not show your work in the space provided.Record only your final answer with the correct number of significant digits and the proper units.
Below is a picture of a 10-fold dilution series. What is the dilution factor of tube # 3? Write as both a fraction and scientific notation. i mL EC 9 mL 9 mL 9 mL HIO 9 mL ecterial Sampie TLbe #1 Tube e2 Tube #3 Tube #4
Find the mistake. A student calculated their answer to a gas law problem as shown in the image below. Their answer is incorrect. Review their work and find the mistake the student made in their calculation. The question is typed in the upper left corner. Hint: There is only 1 step that is incorrect and the issue IS NOT related to significant figures! Click here for the Gas Laws Formula Sheet. Click here for the Periodic Table. A sample of oxygen gas is stored in a 500.0mL flask at 108 kPa and 10 degrees C. The gas is transferred to a 750.0 mL flask at 75 kPa. What is the temperature inside the second flask? G:Vi=500mL Pi=108kla, Ti=10°c Vz= 30ML P2:75kPa → T2 = P3 V2 T, P.V, Pz Vz S:T= 754 Pa(750mL)( 10°C) 1as kPa (500 mL) ST2=10.42°C BI U
A chemist adds 1.70 L of a 0.39 mol/L barium chloride (BaCl) solution to a reaction flask. Calculate the millimoles of barium chloride the chemist has added to the flask. Round your answer to 2 significant digits. manol O.P X
* Question Completion Status: A Moving to another question will save this response. Question 26 SHOW WORK Given the following reaction: CaC 2(s) + 2H 20 - C2H 2(g) + Ca(OH) 2(aq) Assume that you place 1.85 g of calcium carbide in excess water and collect the acetylene gas over water. Calculate the maximum amount of gas that should be produced in grams round answer to 3 decimal places omit trailing zeroes The actual volume of acetylene and water vapor collected is 810 ml at 30.5°C with a pressure of 557.524 mmHg. Calculate the actual amount of gas collected(in grams) round answer to 3 decimal places omit trailing zeroes The vapor pressure of water at 30.5°C is 32.35 mmHg. Calculate the percent yield of acetylene. round answer to 2 decimal places omit trailing zeros A Moving to another question will save this response.
11. Radon gas produces radioactive particles and in high concentrations can result in lung cancer in humans. The radon gas level inside a basement is measured at 4.5 × 10ª Curies/cm³. How many picoCuries of radon are present in the room if the room's dimensions are 7.2 m × 8.5 m × 4.0 m?
> Question 7 A container of O₂ gas at 75 °C has a volume of 3.5 liters at 1.3 atm. What is the new volume of the gas if the pressure is reduced to 0.80 atm with the temperature staying at 75 °C? (K="C + 273) (Hit Remember that all the temperatures in your calculation must be in Kelvin K O 5.7 Iters O 2.2 ters Ⓒ 4.6 Iters 0.30 liters Question 9 What is the volume, in liters, of 45.0 g of N₂ gas at STP? (1 mole of gas at STP -22.4 L of gas (The molar mass of the nitrogen atom. N. is 14.01 g/mole. 72.0 Ster 36.0 ters O 1000 liters O 00717 ters
Part A. State a number of molecules for 1 mol of nitrogen, N2. Part B. State a mass for 1 mol of nitrogen, N2. Express your answer to two decimal places and include the appropriate units. Part C State the volume at STP for 1 mol of nitrogen, N2. Express your answer to three significant figures and include the appropriate units
An IV bag contains 0.4979 mol of NaCl and a total volume of 2.974 L. What is the concentration of the IV in mass per volume (m/v) percentage? Be sure to express your answer to the correct number of sig figs and include units.
If 2.85 L of nitrogen gas and 2.1 L of hydrogen gas were allowed to react, how many liters of ammonia gas could form? Assume all gases are at the same temperature and pressure. Enter to 2 decimal places.
Hydrogen gas has a density of 0.090 g/L, and at normal pressure and - 2.78 °C one mole of it takes up 22.4 L. How would you calculate the moles in 990. g of hydrogen gas? Set the math up. But don't do any of it. Just leave your answer as a math expression. Also, be sure your answer includes all the correct unit symbols. moles = x10 degreenobox