Aerosol cans carry clear warnings against incineration because ofthe high pressures that can develop if they are heated. Supposethat a can contains a residual amount of gas at a pressure of 770mmHg and a temperature of 30 °C.lescMother to Son &....pdf!110QAN23²F2WS#3X80F3H1option commandEDWhat would the pressure be if the can were heated to 1255 °C?Express your answer in atmospheres to three significant figures.$4P₂ =SubmitProvide FeedbackR—| ΑΣΦColo 5%FRequest AnswerF51MacBook AirTV^6GF6Y&7BF7H?atm*U8FBN

Answered: Image /qna-images/answer/6a52d04f-e0c6-4635-b0ec-563bdf1e1b73.jpg

Aerosol cans carry clear warnings against incineration because of the high pressures that can develop if they are heated. Suppose that a can contains a residual amount of gas at a pressure of 770 mmHg and a temperature of 30 °C. What would the pressure be if the can were heated to 1255 °C? Express your answer in atmospheres to three significant figures.

Aerosol cans carry clear warnings against incineration because of the high pressures that can develop if they are heated. Suppose that a can contains a residual amount of gas at a pressure of 770 mmHg and a temperature of 30 °C. What would the pressure be if the can were heated to 1255 °C? Express your answer in atmospheres to three significant figures.

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

Pls help ASAP.
A sample of methane occupied 18.95 L at 41.03 °C. When the volume changed to 11.60 L at 16.59 °C, the pressure was 2.044 atm. Calculate the original pressure (atm). Write out the problem on paper in order to answer the questions related to the setup and the calculation for this problem. Identify all of the terms in this problem and enter the numerical values (without units) in the appropriate blanks. Convert temperature(s) to K, and enter with proper s.f. If the term doesn't apply in this problem enter 0. Enter a question mark for the variable being calculated. Do not leave any blank empty. P1 = V1 = T1= n1= P2= V2= T2= n2= Rearrange the gas law equation needed to solve for the variable of interest. Identify which terms are in the numerator and which terms are in the denominator after rearranging. Do not leave any blank empty. Enter a zero "0" if the blank is not needed. Use the following abbreviations: pressures = P1, P2; volumes = V1, V2; temperatures = T1, T2, moles = n1, n2…
A sample of gas has an initial volume of 13.8 L at a pressure of 1.35 atm. If the sample is compressed to a volume of 10.3 L, what is its pressure? Express the pressure in atmospheres to three significant figures.
HCl(g) can be made by the direct reaction of H2 and Cl2 in the presence of light. 6.00 g of H2 and 1.50 x 102 g Cl2 are mixed in a 5.00 L flask at 28.0 °C. What are the partial pressures of gases after the reaction has completed. Given Information: > Temperature and volume remains constant at 28.0 °C > Wavelength of light needed for the reaction is 340 nm.
A hot air balloon is filled with 1.39 × 10° L of an ideal gas on a cool morning (11 °C). The air is heated to 113 °C. What is the volume of the air in the balloon after it is heated? Assume that none of the gas escapes from the balloon. volume: L
Using these formulas pressure at sea level =760 mmHg and P1V1=P2V2
A scuba diver exhales 3.00 L of air while swimming at a depth of 20.0 m, where the sum of the atmospheric pressure and water pressure is 3.50 atm. By the time the exhaled air rises to the surface, where the pressure is 1.00 atm, what is the volume if the temperature of air does not change during its travel. Show your work. Pay attention to significant figures.
SF6 can be synthesized by the reaction: SO2(g) + 3 F2(g) → SF6(g) + O2(g)A 1.25-L reaction vessel, initially at 26°C, contains sulfur dioxide gas at a partial pressure of 184 mmHg and fluorine gas at a partial pressure of 511 mmHg. Identify the limiting reactant and determine the theoretical yield of SF6 in grams.
Please help me solve part A&B. Thank you.
2. Sodium sulfide (0,1159 g) and excess hydrochloric acid were reacted together to form 35.75 mL of an unknown gas. The gas was collected over water when the atmospheric pressure was measured to be 767 mmHg. The temperature of the water was 23.0°C. Determine the molar mass, as well as identity, of the gas. Hint: You will need to reference your textbook for the vapor pressure of water.
A quantity of helium gas is originally held under a pressure of 145 kPa at 18°C. If the volume of the container is tripled, and the temperature is increased to 30°C, what is the resulting pressure in kPa? (Hint, can you make up a volume?) H 322181 Li Na Mg Rb Be Sr Cs Ba Fr 22 Ca Sc Ti Ra Raden Lat 94.5 kPa 46.4 kPa 378.3 kPa 453.9 kPa 50.3 kPa MD 45 83-103 482.2 kPa Zr Hf Atvice Ac Th Series 23 VO Vieta VID 24 2 Ta W Tete 104 105 Rf Db Sg Cr Mn Periodic Table of the Elements VID 75 41. 34445 Nb Mo Tc Ru Rh Pd Ag Cd Abaline Tra Saber 26 27 28 29 30 Fe Co Ni Cu Zn Re Os Symbol S 13 13 FIA B Nawww Al Ga Halagan In La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho D IVA 70 Pt Au Hg Tl Pb B Mar 102108, 109 114 Bh Hs Mt Ds Rg Cn Uut "FI 590 U Np Pu Am Cm Bk Cf Es Sn Sb 14 15 16 17 18 Si CI Ar La 16 3514. Ge As Se Br Kr By 17 VIA 18 VELA He Hek 4000 Ne 62 63 64 SA Te I Xe 16 At Rn Fate Bi Po Uup "Lv Uus Uuo Er Tm Yb Lu C Henan 100 100 Fm Md No L
Hw.75.