Calculations for experimentally determining R   Trial 1 Trial 2 Mass of Mg ribbon (g) 0.033 0.039 Temperature of H2(g) (°C) 23.5 23.7 Volume of H2 collected (mL) 33.80 38.97 Atmospheric pressure (torr) 758 758 Vapor pressure of water (torr)     Volume of H2 gas in liters (L)     Temperature of H2 gas in Kelvin (K)     Moles of H2 gas (mol)     Pressure of H2 gas in atmospheres (atm)     Experimental value of R (L·atm/(mol·K))       Average value of R (L·atm/(mol·K)):   Percent error (%)Use 0.08206 L·atm/(mol·K) for the theoretical value of R:   The hydrogen generated in this lab was a product of the reaction between magnesium and hydrochloric acid. Which of these reactants is the limiting reactant?: Magnesium or Hydrochloric Acid? Explain reasonsing.

the atmospheric pressure in inches Hg (inHg) 30.08 Temperature at beginning of measurements (°C) 20.6     Mass added Syringe volume Reading 1 0.0   5.0   Reading 2 0.300   4.5   Reading 3 0.450   4.2   Reading 4 0.650   4.1   Reading 5 0.950   3.6   Reading 6 1.150   3.1   Reading 7 0.200   5.4   Reading 8 0.400   6.7   Reading 9 0.550   7.5   Reading 10 0.700   8.4   Reading 11 0.900   9.3   Temperature at end of measurements (°C) 20.6   PV Measurements and Calculations   Volsyringe (mL) VolT (mL) Mass added (kg) Force (kg·m/s2) Psyr (Pa) PT (Pa) PV (Pa·mL) No mass addedReading 1 5.0     0.000           Increasing the pressureReading 2 4.5     0.300           Reading 3 4.2     0.450           Reading 4 4.1     0.650           Reading 5 3.6     0.950           Reading 6 3.1     1.150           Decreasing the pressureReading 7…

0.374 m3 of hydrogen was observed at −7.0 oC and atmospheric pressure (105 Pa). The relative molecular mass of hydrogen is 2.02 g mol-1 and the gas constant, R, is 8.314 J K−1 mol−1 a) Calculate the number of moles (round to 2 decimal places): b) Calculate the mass of the gas in g (round to 3 significant figures):

In this experiment, we will be using the gas inside of a small hand-held lighter. Before the trial, the lighter weighed 46.747 g. After the trial the mass of the lebter was 31.104 g. what is the mass in grams of the gas used? Enter a numeric answer only. A Moving to another question will save this response. «< Question 6 of 10 8:39 AM search 耳 a 22 4/13/2022 hp insert prt sc delete 144 %24 4 %23 & L. 8 6. %3D backspace hor R T Y U P F G L enter D pause t sh C alt ctri

01 10 11 20 21 22 23 24 25 Question 23 A bottle of concentrated hydrochloric acid is opened and set beside an open bottle of concentrated ammonium hydroxide. A white cloud forms above the opening of the bottles. What is the white cloud? Your answer: O A) ammonium chloride O B) hydrochloride gas C) ammonia gas D) water vapor Clear answer US 8:05

An extended form of the combined gas law can be developed if moles of gas change. In this extended form, only R is constant, so n₁ and n₂ must be included. n₁T₁ T₂ 1 1 22 Based on this gas law, which of the following are correct relationships describing n₁ and n₂? A n ₁ T₁ = ¹₂₁²₂ 1 1 2 (B) E n n 1 2-7 = T T 1 F n P₁"₁=P₂" 2 P₁ P2 == n "₁ ⒸV₁"₁₁=V₂" ₂ V n 1 n 1 == n 2 P₁V₁ P₂V/2 1 1 22 2

eq req < 1req For each of the following sets of volume/temperature data, calculate the missing quantity after the change is made. Assume that the pressure and the amount of gas remain constant. V=2.30 L at 22.0 °C V = 4.98 L at ? °C PC V = 120. mL at 281 K V = ? mL at 386 K mL V=49.7 mL at 37.0 °C V = ? mL at 357 K a. APR 30 b. C. Submit Answer 2 mL Retry Entire Group Show Hint tv [Review Topics] Ⓒ 9 more group attempts remaining [References] SENSA SPREC ********* Previous Next Save and Exit 3

pe here to search ? * 2 1 According to the kinetic theory of gases, the average kinetic energy of the gas particles in a gas sample is directly proportional to the O number of moles of gas. O volume. O pressure. O molar mass. O temperature. eTextbook and Media Save for Later Attempts: 0 of 2 used Submit Answer W insert N 3 @ 2 W S 13 * # X alt 3 E D $ 101 4 C R O E LL F % 5 V T G 6 B Y 4 & H 7 no U N 4+ * 8 fo M a 144 ( 9 K V fo ▶11 ) O L fn > A4 P - ; alt { ? + [ 1 = ( } 个 ctrl 1 pause prt. backs 1 t

11:32 AM Sun Oct 22 Question 21.a of 34 8% 0.5683 g Submit The following reaction can be used to convert carbon dioxide to oxygen gas. 4 KO₂ (s) + 2 CO₂(g) → 2 K₂CO3(s) + 3 O₂(g) What is the mass in grams of oxygen gas that can be produced from 0.371 grams of carbon dioxide?

10001 me r 9 е 9.38 Constants Part A Assuming all gases are at the same temperature and pressure, how many milliliters of hydrogen iodide are produced from 165 mL of H2 ? H2 (g) +I2(g)→2HI(g) Express your answer with the appropriate units. HÁ VHI Value %3D Submit Previous Answers Reguest Answer X Incorrect; Try Again Provide Feedback