In this experiment, you will determine the molar volume of a gas by conducting a chemical reaction that produces a gas, as shown in the reaction equation below. Mg(s) + 2 HCI(aq) → MgCl2(aq) + H2(g) DATA: Trial 1 Trail 2 Trail 3 Mass of Mg (g) 0.012 0.013 0.014 Vol of flask (mL) 139.5 139.5 139.5 Max Pressure (atm) 1.0431 1.0293 1.0530 Initial Pressure (atm) 0.9425 0.9309 0.9560 Pressure change,A P (atm) 0.1006 0.0984 0.0970 Temperature (K) 294.00 294.70 293.55 Calculate the volume of hydrogen gas (molar volume) at STP (T2, P2). Use the Combined Gas Law. trial 1: trial 2: trial 3:

In this experiment, you will determine the molar volume of a gas by conducting a chemical reaction that produces a gas, as shown in the reaction equation below. Mg(s) + 2 HCI(aq) → MgCl2(aq) + H2(g) DATA: Trial 1 Trail 2 Trail 3 Mass of Mg (g) 0.012 0.013 0.014 Vol of flask (mL) 139.5 139.5 139.5 Max Pressure (atm) 1.0431 1.0293 1.0530 Initial Pressure (atm) 0.9425 0.9309 0.9560 Pressure change,A P (atm) 0.1006 0.0984 0.0970 Temperature (K) 294.00 294.70 293.55 Calculate the volume of hydrogen gas (molar volume) at STP (T2, P2). Use the Combined Gas Law. trial 1: trial 2: trial 3:

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...

See similar textbooks

Similar questions

Consider the following chemical reactions: KClO3 (s) ----------> KCl(s) + O2(g) NaNO3(s) ---------> NaNO2(s) + O2(g) 5.0000 g mixture of potassium chlorate and sodium nitrate is decomposed and the mass of residuals is 3.8600 g. The oxygen gas is collected in 359. mL. container at 25 oC by water displacement technique. Calculate the total pressure in mmHg. the vapor pressure of H2O at 25oC is 18.3 mmHg. K = 39.10 g/mole, Cl = 35.45 g/mole, Na = 22.99 g/mole, N = 14.00 g/mole and O = 16.00 g/mole
+ Chemistry 20 Midterm Equation Sheet (Click to open) Nitric acid is a potentially dangerous strong acid that must be handled with great care. A laboratory technician is asked to dilute a sufficient quantity of stock 15.4 mol/L nitric acid to produce 1.50 L of a 0.220 mol/L solution. Calculate the volume of concentrated nitric acid needed to prepare this diluted solution. XQ F1 BI E E F2 2 E E F3 % F4 F5 U S X₂ x² E F6 II Proctorio is sharing your screen. Ⓡ F7 = I Stop sharing DO LL F8 5 C H Hide + F9 ✓ C F10
What volume of NH3 is produced in the following reaction when 3.0 L N₂ reacts with 4.0 L of H₂? N₂(g) + 3H₂(g) →→→ 2NH3(g) Files Accepted file types All file types H 4 You can drag and drop files here to add them. a ⠀⠀⠀
When solutions of silver nitrate and sodium chloride are mixed, silver chloride precipitates out of solution according to the equation AGNO3 (aq) + NaCI(aq)→AgCl(s) + NaNO3(aq) Part A What mass of silver chloride can be produced from 1.69 L of a 0.214 solution of silver nitrate? Express your answer with the appropriate units. • View Available Hint(s) ? mass of AgCl = Value Units Submit Part B The reaction described in Part A required 3.48 L of sodium chloride. What is the concentration of this sodium chloride solution? Express your answer with the appropriate units. • View Available Hint(s) HA ? Value Units Submit
Part A What is the minimum amount of 6.1 M H2SO4 necessary to produce 27.1 g of H2 (g) according to the following reaction? 2Al(s) + 3H2S04(aq) → Al½(SO4)3 (aq) + 3 H2(g) Express your answer using two significant figures. • View Available Hint(s) ? V = L
A student prepares phosphorous acid by reacting solid phosphorous triiodide with waterPI₃(s) + 3 H₂O(l) → H₃PO₃(s) + 3 HI(g)The student needs to obtain 0.359 L of phosphorous acid (d=1.651g/mL). The procedure calls for a 43.3 % excess of water and a yield of 70.8%. How much phosphorous triiodide should be weighed out?
Need these
2. Sodium nitrate decomposes into sodium nitrite and oxygen gas with heat. When 0.123 g of sodium nitrate was heated, it produced 16.2 mL of oxygen collected over water. The room temperature and pressure are 22.5°C and 758 torr, respectively. The water over which the gas was collected had a temperature of 20.0°C. Calculate the theoretical amount of oxygen in grams which should have been produced. What is the percent yield? Theoretical yield oxygen: Actual yield oxygen: bg Percent yield:
Here is a yıaph of the molarity of acetonitrile (CH3 CN) i in a reaction vessel during a certain chemical reaction. Use this graph to answer the questions in the table below. 0.30 0.25 0.206, M 0.1544 0.10+ 0.07872- 0.05+ 130 150 25,265.1 50 100 200 seconds O created Is CH,CN being created or destroyed by the chemical O destroyed reaction? O neither created nor destroved If CH, CN is being created or destroyed, what is the rate at which it is being created or destroyed 130 seconds after the reaction starts? Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. If CH, CN is being created or destroyed, what is the average rate at which it is being created or destroyed during the first 130 seconds of the reaction? olo
Here is a graph of the molarity of ethanol (C₂H5OH) in a reaction vessel during a certain chemical reaction. Use this graph to answer the questions in the table below. M reaction? 0.003 0.00197 0.001 0 y 5 10 15 seconds Is C₂H5OH being created or destroyed by the chemical 20 25 created destroyed 30 neither created nor destroyed X 5 x10 010 X G