"The dissolving of NH4NO3 is used in chemical cold packs. If 33.7 g NH4NO3 is dissolved in 88.9 mL of water at 20.6°C, what is the final temperature of the solution? The mass of the solution is the mass of the salt and the water together. NH4NO3(s) - → NH4*(aq) + NO3(aq) AHdissolving = 25.7 kJ/mol"

(c) Cl2(g) + KBr(aq) → KCI(aq) + Br2(g) O combination O decomposition O displacement molecular equation Cl2(g) + reducing agent KBr(aq) KCI(aq) + Br2(g) oxidizing agent total ionic equation | Cl2(g) + CI (aq) + net ionic equation K*(aq) + Br (aq) K+(aq) + Br2(g) Cl2(g) + K+(aq) + Br (aq) → K+(aq) + CI (aq) + | Br2(g)

produce carbon dioxide and water, as described in the following reaction: C.H»O, (s) + _ O: (g) → _ H;O (1) + CO; (g) are come

A reaction uses a solution in which solid sodium chloride is dissolved in water. Which symbol designates the physical state of this reactant? O (s) O (I) O (g) O (aq)

esc Phosphoric acid, which is commonly used as rust inhibitor, food additive and etching agent for dental and orthopedic use, can be synthesized using a two-step thermal process. In the first step, phosphorus and oxygen react to form diphosphorus pentoxide: P₁(1)+50₂(g) 2 P₂O(g) In the second step, diphosphorus pentoxide and water react to form phosphoric acid: P₂O(g) + 3 H₂O(1)-2 H₂PO₂(0) 4 Write the net chemical equation for the production of phosphoric acid from phosphorus, oxygen and water. Be sure your equation is balanced. 0 Continue 56°F Clear F1 J F2 @ 2 F3 # 3 Q Search F4 $ 4 F5 % 5 F6 6 0-0 X F7 & 00 7 Ś F8 © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibi M OO DELL F9 prt sc F10 home F11 end 12 F12 0 Submit Assignment J olo 18 Ar insert

Your lab partner accidentally mixed some sodium chloride with your sample of Epsom salts (M9SO,·7H,O). You want to make a standard solution of magnesium ion, and this is the only sample of a magnesium salt you have. To determine the amount of magnesium salt in the mixture, you heat 100.00 g to drive off the water of hydration and find that the anhydrous mixture has a mass of 73.25 g. What is the mass in grams of the original salt mixture that you must add to 1.000L of water to make a 0.1000 M solution of Mg2+ ion?

One way in which the useful metal copper is produced is by dissolving the mineral azurite, which contains copper(II) carbonate, in concentrated sulfuric acid. The sulfuric acid reacts with the copper(II) carbonate to produce a blue solution of copper(II) sulfate. Scrap iron is then added to this solution, and pure copper metal precipitates out because of the following chemical reaction: Fe(s) + CuSO (aq) → Cu(s) + FESO,(aq) Suppose an industrial quality-control chemist analyzes a sample from a copper processing plant in the following way. He adds powdered iron to a 200. mL copper(II) sulfate sample from the plant until no more copper will precipitate. He then washes, dries, and weighs the precipitate, and finds that it has a mass of 64. mg. Ar Calculate the original concentration of copper(II) sulfate in the sample. Round your answer to 2 significant digits. 10

One way the U.S. Environmental Protection Agency (EPA) tests for chloride contaminants in water is by titrating a sample of silver nitrate solution. Any chloride anions in solution will combine with the silver cations to produce bright white silver chloride precipitate. Suppose an EPA chemist tests a 250. mL sample of groundwater known to be contaminated with iron(II) chloride, which would react with silver nitrate solution like this: FeCl₂(aq) + 2 AgNO3(aq) → 2 AgCl(s) + Fe(NO3)₂(aq) The chemist adds 16.0 mM silver nitrate solution to the sample until silver chloride stops forming. She then washes, dries, and weighs the precipitate. She finds she has collected 2.0 mg of silver chloride. Calculate the concentration of iron(II) chloride contaminant in the original groundwater sample. Round your answer to 2 significant digits. mg 0 L x10 X Ś