The data below is for a sample of gas at 25ºC. Volume Difference in Hg Pressure Px V (mL) Levels (mm) (mm) (mm x mL) 35.6 710 34.9 +15 33.7 +40 31.2 +100 25.3 +290 36.6 -20 38.3 -50 41.4 -100 50.6 -210 Now, calculate the Px V product (this is the proportionality constant, k) for each volume and pressure and fill in the column in the table. Complete the statements below: Statements: 1. The name of the curve you graphed is 2. The mathematical relationship between P and V is 3. The value of the proportionality constant, k, is 4. The volume of this sample of gas at 2.00 atm and 25°C would be (Show your calculation in the space below.)

The data below is for a sample of gas at 25ºC. Volume Difference in Hg Pressure Px V (mL) Levels (mm) (mm) (mm x mL) 35.6 710 34.9 +15 33.7 +40 31.2 +100 25.3 +290 36.6 -20 38.3 -50 41.4 -100 50.6 -210 Now, calculate the Px V product (this is the proportionality constant, k) for each volume and pressure and fill in the column in the table. Complete the statements below: Statements: 1. The name of the curve you graphed is 2. The mathematical relationship between P and V is 3. The value of the proportionality constant, k, is 4. The volume of this sample of gas at 2.00 atm and 25°C would be (Show your calculation in the space below.)

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

lc X LMS Middle tion.com GAS LAW IDEAL GAS LAW CONSTANT INTRODUCTION LABORATORY SIMULATION Water Vapor Pressur ases produced by a chemical reaction can easily be collected over water. To determine the pressure of the dry ga: por pressure of the water at that temperature must be subtracted from the total pressure. ) Consider the following reaction: Mg(s) + 2 HCl(aq) MgCl2(aq) + H2(9) The total pressure of gas collected over water is 785.0 mmHg and the temperature is 24.0°C What is the pressure of hydrogen ormed in mmHg? mmHg Pressure D
Trimix is a general name for a type of gas blend used by technical divers and contains nitrogen, oxygen and helium. In one Trimix blend, the partial pressures of each gas are 55.0 atm oxygen, 90.0 atm nitrogen, and 51.0 atm helium. What is the percent oxygen (by volume) in this trimex blend? % 1 3 4 6. C 7 8. 6. +/- х 100 2.
34.0 mL of 6.0 M sulfuric acid solution is spilled on the floor. The acid is neutralized by pouring sodium hydrogen carbonate on the spilled acid. What is the volume, in L, of the carbon dioxide which is released at 25 deg. C and 1 atm? H2SO4 (aq) + 2NaHCO3 (s) --> Na2SO4 (aq) + 2H2O (l) + 2CO2 (g)
In dry atmospheric air, the four most abundant components are N₂, X = 0.808; O₂, X = 0.1915; Ar, X = 9.34x10-5; and CO₂, X = 4.066x104. Calculate the partial pressure of CO₂, in torr, under standard atmospheric conditions. Submit Answer Tries 0/99 This discussion is closed. M CAL 8:00- 10:50- CI 12:00 Q ! 2 @ W OCT 21 F2 # 3 E 80 F3 $ 4 R 10 Q F4 % 5 T F5 A 6 Y F6 tv A S MacBook Air & 7 8 F7 8 DII FB ( 9 F9 O ) 0 J F10 F11 + F12 Send Feedback
The ideal gas law describes the relationship among the pressure P, volume V, number of moles n, and absolute temperature T of an ideal gas. Here is the relationship expressed mathematically: PV = nRT where R is a proportionality constant. The units of R are determined by the units of pressure and volume used in the equation. When bar used for pressure and L for volume, the appropriate R value is 0.08314 L bar mol-¹ K-¹. Part A How many air molecules are in a 4.05 x 3.66 x 3.05 m³ room? Assume atmospheric pressure of 1.00 bar, a room temperature of 20.0 °C, and ideal behavior. Express your answer using three significant figures. ► View Available Hint(s) VE ΑΣΦ + Review | Constants | molecules
Question 11 (1 point) A scientist isolates a sample of gas that occupies a volume of 678.1 mL at 104.3 kPa and 39.27 °C. If the gas has a molar mass of 81.98 g/mol. Calculate the mass of the sample in grams. Provide your answer to TWO decimals. Your Answer: 9 2 S 3 e d $ 4 f % 5 t 9 DELL Oll 6 b y & 7 h U n * 8 i 9 11.
How many moles of gas must be forced into a 3.1 LL ball to give it a gauge pressure of 8.4 psipsi at 23 ∘C∘C? The gauge pressure is relative to atmospheric pressure. Assume that atmospheric pressure is 14.6 psipsi so that the total pressure in the ball is 23.0 psipsi .
The combined gas law states that for a fixed amount of gas, the quantity PVIT is constant. This is often expressed by the equation P¡V PV2 T2 where P is the pressure, V is the volume, and T is the temperature, and the subscripts 1 and 2 denote two different conditions. Rearrange the combined gas law to solve for Pj. P = A gas with an initial temperature of 271 K and initial volume of 15.0 L is heated to 317 K and compressed to 10.2 L. The final pressure of the gas is 4.28 atm. What was the initial pressure (P¡) of the gas? P1 = atm
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
Find the volume in milliliters of 3.50 mol of an ideal gas at 36°C and a pressure of 1120 torr. Use the ideal gas law and the appropriate R value: R = 0.0821 atm • L/mol • KR = 8.31 kPa • L/mol • KR = 62.4 torr • L/mol • K
Table 1. Pressure vs Volume Data (including the inverse of Pressure). Volume (mL) Pressure (kPa) Inverse Pressure (kPa-1) 250 100 1/100 = 330 75 500 50 1000 25 Draw two graphs: 1) Volume and Pressue 2) Volume and Inverse Pressure
Initial Pressure = 720 torr, Initial Volume = 256 mL, Initial Temperature = 25.0oC, Final Volume = 250 mL and Final Temperature = 50.0oC. Solve for Final Pressure. (x10 due to SF) Answer: x10^ Unit: Blank 1: Blank 2: Blank 3: