E Result List X3 Course Pro XCP Referen XPSY2214-0 XCourse Ho X& Clevela 4A Module 4 Xllege.com/course.html?courseld=16985674&OpenVellumHMAC=d20f081859e6de97f65e31513d4bfdc9#10001Exercise 10.89 Enhanced with FeedbackM Review | ConstaMISSED THIS? Watch IWE 10.14; ReadSection 10.10. You can click on the Review link toaccess the section in your e Text.Part AChlorine gas reacts with fluorine gas to formchlorine trifluoride via the following reaction:Part BCl2 (g) + 3F2(g) → 2CIF3(g)A 1.80 L reaction vessel, initially at 298 K,contains chlorine gas at a partial pressure of 337mmHg and fluorine gas at a partial pressure of827 mmHgDetermine the theoretical yield of CIF3 in grams.Express your answer in grams to three significant figures.gMCIF;SubmitRequest AnswerProvide Feedback

Given, Reaction : Cl2(g) +3F2(g) → 2ClF3(g)Calculations of moles of reactant : (a) moles of Chlorine : ncl=PVRT⇒ncl=337760 atm×1.80 L0.0821 L atm mol K×298 K⇒ncI=0.0325 mol (b) moles of Fluorine : nF=PVRT⇒nF=827760 atm×1.80 L0.0821 L atm mol K×298 K⇒nF=0.080 molAccording to balanced reaction , 1 mol Cl requires 3 mol of F2 , so 0.0325 mol Cl requires 3×0.0325=0.0975 mol F2, but we only have 0.080 mol of F2 So, F2 is the limiting reagent , so moles of ClF3 formed : =23×0.080=0.05332 mol mass of ClF3 formed : = moles ×molar mass=0.05332 mol×92.448 gmol=4.92932 g≈4.93 g { rounding off to 3 sig. figure }

Science

Chemistry

gas chlorine trifluoride via the following reaction: Cl2 (g) + 3F2(g) → 2CIF3 (g) Part B A 1.80 L reaction vessel, initially at 298 K, contains chlorine gas at a partial pressure of 337 mmHg and fluorine gas at a partial pressure of 827 mmHg Determine the theoretical yield of CIF3 in grams. Express your answer in grams to three significant figures. MCIF, = g Submit Request Answer

gas chlorine trifluoride via the following reaction: Cl2 (g) + 3F2(g) → 2CIF3 (g) Part B A 1.80 L reaction vessel, initially at 298 K, contains chlorine gas at a partial pressure of 337 mmHg and fluorine gas at a partial pressure of 827 mmHg Determine the theoretical yield of CIF3 in grams. Express your answer in grams to three significant figures. MCIF, = g Submit Request Answer

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

12b
Using stoichiometry, calculate the volume of O2 gas at 1.25 atm and 18.0 ̊C, which forms when 10.5 g KClO3 decomposes according to the reaction:2 KClO3 → 2 KCl + 3 O2
2H3PO4(s) --> 3 H2(g) + 2 P(s) + 4 O2(g) Using the reaction above, show step by step how many liters of oxygen can be created if I start with 0.7156 grams of H3PO4 solid at STP?
Answer both !
A 0.6333 g sample of a metal carbonate was reacted with hydrochloric acid. The carbon dioxide gas generated was collected over water at a temperature of 26.0°C and pressure of 103.80 kPa. The final volume of carbon dioxide gas collected was 125.0 mL. XCO₃(s) + 2HCl(aq) → XCl₂(aq) + H₂O(l) + CO₂(g) Find the moles of the metal carbonate reacted.
Hydrogen peroxide (34.02 g/mol) decomposes into water and oxygen gas according to the reaction 2 H₂O2 (1) → 2 H2O (l) + O2 (g) A 7.50 g sample of hydrogen peroxide is sealed in a 375 mL container at 350 K. Identify the strategy you would use to determine the pressure of O2 gas produced from the decomposition of the hydrogen peroxide sample. -> grams H2O2 → moles H2O2 → moles O₂ → pressure 02 → moles 02 → pressure O2 → grams H2O2 moles H2O2 pressure 02 → moles 02 → moles H2O2 · →> grams H2O2 moles H2O2 → pressure 02
An old gas cylinder you found lost its label. Lab supervisor is pretty sure that it is either He, Ne, Ar or Kr and you were tasked to figure out which one. What you did was that you transferred some of the gas from the old cylinder into an evacuated 10-L flask until the gauge pressure inside reached 1.00 atm. After sealing it, you carefully weighed the gas-filled flask and figured out that the mass of the gas (excluding that of the flask) was 15 g. If the temperature and barometric pressure in the lab was 27°C and 1 atm, what was the gas?
Pls help ASAP.
Time Left:0:55:00 A student completes the experiment The Universal Gas Constant and obtains the following data for one trial. mass of magnesium (g): Initial gas volume (ml): Final Volume (mL): Temperature (°C): Atmospheric pressure (inHg): Ah (cm of water): F3 80 모 Calculate the partial pressure of hydrogen, PH2, for this trial. Give your answer in torr (mmHg). 1 in Hg = 25.4 mmHg 1 cm water = 0.735559 mmHg 1 mol Mg = 24.305 g Mg TABLE D-4 TEMP 1_DEG₁_C_1 1 3 I 1 1 Q F4 0 1 = 2 3 4 5 6 7 8 10 11 12 13 14 0.0 0.1 0.0326 0.00 35.30 21.3 30.21 16 17.13 F5 6.100 | 6.143 1 6.544 1 6.589 0.2 1 VAPOR PRESSURE OF HATER 0-30 DEG. C IN MM HG 1 4.579 4.612 4.646 | 4.924 | 4.959 4.995 15.291 4.660 4.714 5.0315.068 5.329 5.367 5.406 5.445 4.7484.783 4.818 5.104 | 5.141 | 5.178 5.484 5.523 5.563 5.888 5.930 6.230 16.274 6.318 5.363 15.683 15.723 | 5.764 | 5.8051 5.146 6.186 6.636 5.972 1 6.0141 6.057 1 6.407 1 6.453 6.498 1 6.82 | 6.729 6.776 6.823 | 6.871 | 6.919 | 6.967 1 T T 1 I T I 1 17.0167,064…
The catalytic decomposition of hydrogen peroxide yields oxygen gas and water, according to the reaction given below. In an experiment, the decomposition of hydrogen peroxide yielded 75.3 mL of gas collected over water at 25°C and 0.976 atm. (Pwater = 0.032 atm at 25°C) 2 H2O2(aq) → 2 H2O(l) + O2(g) If the original H2O2 solution had a volume on 500 mL, what was the molar concentration of hydrogen peroxide prior to decomposition? A) 1.8 * 10-4 M B) 0.058 M C) 0.0062 M D) 0.060 M E) 0.012 M
Given the following balanced equation, what volume of hydrogen gas (in liters) would be produced under conditions of STP from the reaction of 0.082 grams of magnesium solid reacting with excess hydrochloric acid solution? Please report your answer WITH the correct number of significant figures, and WITHOUT units. Mg + 2 HCl → MgCl2 + H2
If the reaction below took place at STP, what is the volume of O2(g) required to react with 40.0 grams of ZnS(s)? Show all work and report you final answers to the correct units and significant figures. 2ZnS(s) + 3O2(g) -> 2 ZnO(s) + 2 SO2(g)