QUESTION 9 How many atm is the partial pressure of carbon dioxide in a container that holds 17.56 moles of CO2, 24.87 moles of N2 and 25.26 mole of H2 and has a total pressure of 1.85 atm? Answer with correct significant figures and unit in abbreviation. QUESTION 10 If I place 37.37 moles of N2 and 21.94 moles of O2 in a 12.8 L container at a temperature of 6 °C, what will the total pressure, in atm, of the resulting gas mixture be? Answer with correct significant figures and unit in abbreviation. R = 0.0821 atm-L-mole-¹.K-1

QUESTION 9 How many atm is the partial pressure of carbon dioxide in a container that holds 17.56 moles of CO2, 24.87 moles of N2 and 25.26 mole of H2 and has a total pressure of 1.85 atm? Answer with correct significant figures and unit in abbreviation. QUESTION 10 If I place 37.37 moles of N2 and 21.94 moles of O2 in a 12.8 L container at a temperature of 6 °C, what will the total pressure, in atm, of the resulting gas mixture be? Answer with correct significant figures and unit in abbreviation. R = 0.0821 atm-L-mole-¹.K-1

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

help
Consider the apparatus shown below with the valve closed. The volume and pressure of each gas is indicated. F2 N2 Valve 3.00 L 6.00 L 2.00 atm 4.00 atm When the valve is opened the two gases mix uniformly. At that point, what is the mole fraction of fluorine in the mixture? none of the answers are correct O 0.333 0.200 O 0.500
A certain gas is present in a 13.0 LL cylinder at 3.0 atmatm pressure. If the pressure is increased to 6.0 atmatm the volume of the gas decreases to 6.5 LL . Find the two constants kiki, the initial value of kk, and kfkf, the final value of kk, to verify whether the gas obeys Boyle’s law by entering the numerical values for kiki and kfkf in the space provided.
Please answer all the parts of the question
A scuba tank contains three gases; oxygen, helium, and nitrogen at a pressure of 85 atm.If the moles of the three gases in the tank are 4.5 mol of O2, 12.0 mol ofN2, and 8.5 mol of He, what are the partial pressures of each gas inside of the tank?
At a temperature of 25°C a bicycle tire has a pressure of 140. psi with 4.09 x 10-2 moles of nitrogen. The pressure needs to be reduced to 130. psi to be safe for riding. How many moles of air need to be removed from the tire? Assume that the volume of the tire remains constant. 2.9 x 103 mol None of the listed choices are correct. 3.80 x 10-2 mol 2.92 x 10-3 mol 3.8 x 10-2 mol 3.79 x 10-2 mol
What will be the new volume (in Liters) of a gas that is initially at a pressure of (6.150x10^0) atm and volume of (7.37x10^0) L if the pressure is changed to (2.3400x10^0) atm?
Help with the following question
Please answer question 9 Part A and B
Assume that the volume and temperature in containers A, B, and C are identical. Assume that container C holds the same contents as containers A and B combined. Container Container Container A B C Pressure 1.51 atm Moles Suppose that container B has 9 times as many moles as container A does. Based on the data provided above, what is the pressure (in atm) in container C? Report your answer to three decimal places.
A gas mixture has a total pressure of 0.51 atm and consists of He and Ne. If the partial pressure of He in the mixture is 0.23 atm, what is the partial pressure of the Ne in the mixture? Enter your answer in the provided box. atm
Calculate each of the following quantities for an ideal gas: a) The volume of the gas in litre, if 2.57 moles have a pressure of 1.86 atm at a temperature of -12ºC. b) The absolute temperature of a gas at which 6.79 X 10 ² moles occupies 164 mL at 893 torr. c) The pressure in atm , if 8.25 X 10 ² moles occupies 255 mL at 15°C. d) If oxygen gas is used, calculate the mass of the oxygen gas in grams, if 5.49 L at 45ºC has a pressure of 11.25 kPa.