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Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Fully discuss dilution and accretion. Illustrate an example.
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- How many moles of water can be formed from 5 moles of oxygen gas?arrow_forward1. Water is formed by burning H2 (g) in the presence of O2 (g): 2H2 (g) + O2 (g) à 2H2O (g) a) If you have 32 g of H2 gas and 32 g of O2 gas, which do you have the most of in terms of moles? Explain your reasoning. b) Starting from the 32 g of H2, how many moles of water can form from the H2 gas? c) Starting from the 32 g of O2, how many moles of water can form from the O2 gas? d) Based on the amounts of water formed in parts b) and c), which is the limiting reactant for this reaction? H2 gas or O2 gas? Explain your reasoning. e) According to the limiting reactant you chose in part d), what is theoretical yield in grams of water that could be produced when 32 g of H2 gas reacts with 32 g of O2 gas?arrow_forward1. Give reasons why the helium atom is smaller than the cesium atom. 2. A student got a problem wrong. They were asked, “How many grams of MgCl2 (molar mass = 95.21 g/mol) are needed to make 3.16 L of a 0.500 M MgCl2 solution?” The correct answer is 150. but the student got 1.58. What mistake did the student make? 3. To solve the following problem what is the reason you must subtract the vapor pressure of water, 24 torr, from the total pressure, 747 torr in order to solve the problem? “A 500.0-mL sample of H2 gas is collected over water at 298 K and 747 torr. What volume would the dry H2 gas occupy at STP? (Given: the vapor pressure of water at 298K is 24 torr).” By the way, the answer is .436 liters. NOTE: I am not asking you to solve this problem. I am asking the reason for subtracting the vapor pressure. If you simply solve the problem, you will get no points.arrow_forward
- A 36.1 mL sample of oxygen gas contains 0.529 mol of oxygen. If enough oxygen is added to the sample to obtain a volume of 50.5 mL, what must the final mass of the sample be? (The pressure and temperature is constant.) 1) 11.8 g 2) 0.740 mol 3) 23.7 g 4) None of the other answers are correct 5) 0.740 garrow_forwardCH3 SH, Br 5)arrow_forward1. Which is larger, 0.45 mol of a material or 2.75 x 10^23 of the same material? Justify your answer.arrow_forward
- Draw the Lewis structure of PBr3 and determine if the molecule is polar or nonpolararrow_forward24. What is the mass of 5.00 moles of water, H₂O?arrow_forward6.00 g of a certain Compound X , known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar mass of 46. g/mol , is burned completely in excess oxygen, and the mass of the products carefully measured: product mass carbon dioxide 11.48g water 7.05g Use this information to find the molecular formula of X .arrow_forward
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