Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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- Aluminum reacts with aqueous sodium hydroxide to produce hydrogen gas according to the following equation: 2Al(s) + 2NAOH(aq) + 6H2O(1)-2NAAI(OH)4(aq) + 3H2(g) The product gas, H2, is collected over water at a temperature of 25 °C and a pressure of 759 mm Hg. If the wet H, mol. The vapor gas formed occupies a volume of 7.78 L, the number of moles of Al reacted was pressure of water is 23.8 mm Hg at 25 °C.arrow_forwardPlease help me to give you thumbs uparrow_forwardAnswer part a and barrow_forward
- I only need help with part barrow_forwardPlease do not round off sig figs in calculations until final answer. Thank you.arrow_forwardWhat are the units of a? What are the units of b? For carbon dioxide the numerical value of a is 3.592 and the numerical value of b is 0.0429. atm Use the van der Waals equation to calculate the pressure of a sample of carbon dioxide at 55.0 °C with a molar volume of 0.515 L/mol. Round your answer to 3 significant digits. Use the Ideal Gas Law to calculate the pressure of the same sample under the same conditions. Round this answer to 3 significant digits also. atm Explanation Checkarrow_forward
- The compressibility factor Z = PV/nRT for O2 at -38.6°C and 519.6 atm is 1.60; at 162.8°C and 105.4 atm, it is 0.99. A certain mass of oxygen occupied a volume of 2.10 L at 162.8°C and 105.4 atm. Calculate the volume occupied by the same quantity of oxygen at -38.6°C and 519.6 atm. place the answer rounded to the hundredths place Please provide only typed answer solution no handwritten solution needed allowedarrow_forward11. (a) In a 20.0 L steel container, we have only 77.7 g of CO2(g), 66.6 g of N2(g), and O2(g). The temperature is 25.0 ◦C and the total pressure is 8.88 atm. What mass of O2(g) do we have, and what is its partial pressure? The molar masses of C, N, and O are 12.01, 14.01, and 16.00 g/mol. (b) The density of a sample of pure CH4(g) at a constant pressure of 1.00 atm is 0.666 g/L. What is the average speed, or root mean square speed, of the CH4(g) molecules in this sample? The molar masses of C and H are 12.01 and 1.01 g/mol.arrow_forward10barrow_forward
- Using the ideal gas law, PV = nRT, determine the volume 1000 lbs of oxygen would occupy at 40 degree F and a pressure of 22 psig? R = 10.731 psi.ft3/lb mole.0F, molecular wt. of O2 = 32 lbarrow_forwardThe van der Waals equation of state was designed (by Dutch physicist Johannes van der Waals) to predict the relationship between pressure p, volume V and temperature I for gases better than the Ideal Gas Law does: 72 (V-nb)= nRT The van der Waals equation of state. R stands for the gas constant and n for moles of gas. The parameters a and b must be determined for each gas from experimental data. Use the van der Waals equation to answer the questions in the table below. What are the units of a? What are the units of b? For argon the numerical value of a is 1.337 and the numerical value of b is 0.0320. Use the van der Waals equation to calculate the pressure of a sample of argon at -110.0 °C with a molar volume of 2.98 L/mol Round your answer to the correct number of significant digits. atm Use the Ideal Gas Law to calculate the pressure of the same sample under the same conditions. Round your answer to the correct number of significant digits. atm x10 §arrow_forward
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