Most of the coal available in the United States is bituminous or "soft" coal, which contains as much as 5% sulfur by weight. When this coal is burned, the sulfur reacts with oxygen to form sulfur dioxide gas. When the sulfur dioxide gas dissolves in raindrops, it forms sulfuric acid. This is how we get acid rain. Here is the reaction that produces sulfur dioxide gas when soft coal is burned: Sg (s)+80,(g) → 880,(g) Suppose an engineer decides to study the rate of this reaction. He prepares four reaction vessels with 112.8 g of solid sulfur and 49.4 g of oxygen gas each. The volume and temperature of each vessel is shown in the table below. olo Arrange the reaction vessels in decreasing order of initial rate of reaction. In other words, select a "1" next to the vessel in which the engineer can reasonably expect the initial rate of reaction to be highest, a "2" next to the vessel in which the initial rate of reaction would be next highest, and so on. initial rate of vessel volume temperature reaction 3.0 L 630. °C ? B 5.0 L 630. °C C 2.0 L 640, °C ? D 3.0 L 640. °C v ? 1 (highest) 2 3 4 (lowest)

Is the reaction endothermic or exothermic? Explain. Co(H,O), (aq) + 4CF (aq) 2 CoCl7 (aq) + 6H;O (1) Is the reaction reactant favored or product favored? Explain.

Sodium hydrogen carbonate NaHCO3, also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid HCl, which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO3 neutralizes excess HCl through this reaction: HCl(aq)+NaHCO3(aq)→NaCl(aq)+H2O(l)+CO2(g)  The CO2 gas produced is what makes you burp after drinking the solution. Suppose the fluid in the stomach of a woman suffering from indigestion can be considered to be 200.mL of a 0.089M HCl solution. What mass of NaHCO3 would she need to ingest to neutralize this much HCl? Be sure your answer has the correct number of significant digits.

A student dissolves 11.6 g of sodium hydroxide (NaOH)in 250. g of water in a well-insulated open cup. He then observes the temperature of the water rise from 23.0 °C to 35.2 °C over the course of 8.9 minutes. Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction: NaOH(s) Na+ (aq) + OH (aq) You can make any reasonable assumptions about the physical properties of the solution. Be sure answers you calculate using measured data are rounded to the correct number of significant digits. Note for advanced students: it's possible the student did not do the experiment carefully, and the values you calculate may not be the same as the known and published values for this reaction. Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in this case. Calculate the reaction enthalpy ΔΗ per mole of NaOH.…