(79) Cu)6.0-19) C6.6821)2?)2.970.934SL3A9.) If 3 moles of a gas is in a 50ml gontainer at730 mmHg, What is the temperatureof the gas?NS5oml N2T 2\৭56 02462O.9l0Ta T2if10.)atmospheric pressure is 750mmHg and the vapor pressure of water is 45mmHg at30°C?A gas is collected over water at 30°C. What is the pressure of the gasくレ

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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...

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< A mixture of two gases with a total pressure of 2.48 atm contains 0.70 atm of Gas A. What is the partial pressure of Gas B in atm? + 78°F Mostly cloudy G 2 D S W (ts # 3 E (14 $ 4 101 LL ts D F % R T 5 Q Search 16 ^ G CO 6 4- & Y 7 Question 30 of 33 H 4+ * 8 J 144 ( 9 11011 A ) O U
Oxygen gas can be prepared by heating potassium chloride according to the following equation: 2KClO3(s)--->2KCl(s) + 3O2(g) The product gas, O2, is collected over water at a temperature of 20°C and a pressure of 749mm By. If the wet O2 gas formed occupies a volume of 9.80L, the number of moles of KClO3 reacted was _____ mol. The vapor pressure of water is 17.5 mm By at 20°C.
What is the partial pressure of SO2 in a gas mixture of 9.6 g of SO2 and 6.5 g of C2H4O2 at a total pressure of 6.3 atm? The molar mass of C2H2O2 is 60.02 g/mol and molar mass of SO2 is 64.07 g/mol. Sig figs
Use the ideal gas law to complete the table: PP VV nn TT 2.42 atmatm 1.15 LL ___ 206 KK 512 torrtorr ___ 0.751 molmol 294 KK 0.443 atmatm 0.198 LL 1.41×10−2 molmol ___ ___ 20.8 mLmL 5.74×10−3 molmol 20.3 ∘C∘C Complete the first column of the table.
33
Only 2 and 3
2 3
10. What is P2 If P1 = 200 mmHg, T1 = -73 celsius, T2 = 127 celsius. K = C + 273 The answer is 400 atm. Group of answer choices True False
The following system is used for q7-q9 10.00g of O2 and 15.00g N2 are combined in a 20.0L container at 25.00oC O2 32.00g/mol N2 28.02 g/mol R= 0.08206 L atm/mol K What is the partial pressure (atm) of the N2 in the container above. (3 sig figs)
< 1 4 7 +/- Question 7 of 21 A tank of O₂ shows a pressure of 7.35 atm at a temperature of 30.0 °C. What is the density (in g/L) of the gas? 2 5 8 g/L 3 60 9 O Submit Tap here or pull up for additional resources XU x 100
37. A particular equation of state for 02(g) has the form Pv = RT (1 + 2 + 2) where v is the molar volume, B = -21.89 cm3/mol and C = 1230 cmº/mol?. %3D υ Use the equation to calculate the pressure exerted by 1.00 mol of O2 confined to a volume of 500. cm3 at 273 K. 43.1 atm 22.4 atm 1.00 atm 44.8 atm 2.00 atm
Calcium carbide reacts with water to produce acetylene gas according to the following equation: CaC2(s) + 2H20(1) C,H2(g)+ Ca(OH)2(aq) The product gas, C2H2, is collected over water at a temperature of 20 °C and a pressure of 745 mm Hg. If the wet C,H2 gas formed occupies a volume of 7.88 L, the number of moles of CaC2 reacted was mol. The vapor pressure of water is 17.5 mm Hg at 20 °C.

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