Part D decreasing the volume of the container The equilibrium concentration of NH, will decrease. The equilibrium concentration of NHg will increase. The equilibrium concentration of NH3 will not change. Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining Part E adding a catalyst O The equilibrium concentration of NH3 will increase. O The equilibrium concentration of NH3 ill decrease. The equilibrium concentration of NH3g will not change.

Part D decreasing the volume of the container The equilibrium concentration of NH, will decrease. The equilibrium concentration of NHg will increase. The equilibrium concentration of NH3 will not change. Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining Part E adding a catalyst O The equilibrium concentration of NH3 will increase. O The equilibrium concentration of NH3 ill decrease. The equilibrium concentration of NH3g will not change.

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...

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Ethanol, C,H,O, is most often blended with gasoline - usually as a 10 percent mix - to create a fuel called gasohol. Ethanol is a renewable resource and ethanol-blended fuels, like gasohol, appear to burn more efficiently in combustion engines. The heat of combustion of ethanol is 326.7 kcal/mol. The heat of combustion of 2-methylheptane, C3H18, is 1.306×10³ kcal/mol. How much energy is released during the complete combustion of 482 grams of 2-methylheptane ? kcal Assuming the same efficiency, would 482 grams of ethanol provide more, less, or the same amount of energy as 482 grams of 2- methylheptane v more less the same amount
One method used in the production of H2 gas is to put the coal into an incomplete combustion reaction with air and water vapor in the combustion chamber (water gas production). A simplified reaction can be written as:2C + 1 H2O + a (O2+3.76N2) = 1C0 + 1CO2 + 1H2 + 3.76·a·N2 Here, 02+3.76N2 represents the amount of air and is multiplied by the coefficient "a".a) The value of the coefficient "a" for this reaction b) The amount of air to be used for 1 kg of pure carbon (C) (total amount of 02 and N2) (kg-air/kg-carbon) Hint: Consider how many kilograms 1 kmol "C" weighs.
heat 2 Al(s) + Fe,O;(s) Al,O,(s) + 2 Fe(l) If 16.3 kg Al reacts with an excess of Fe, O,, how many kilograms of Al, O, will be produced? kg mass of Al, O, produced:
The human body burns glucose (C6H₁2O6) for energy according to this chemical reaction: C6H12O6 +60₂-6CO₂ + 6H₂O The products of the reaction are carbon dioxide (CO₂) and water (H₂O). Interestingly, all of the carbon dioxide and much of the water exits the body through the lungs: on every breath, the average person exhales 500. mL of air, which is typically enriched to 4% CO₂ and 5% water vapor by volume. In short, when a person loses weight by dieting, the weight that is lost actually departs his body as a gas, every time he exhales. Each kilogram of body fat lost requires exhaling about 2.9 kg of carbon dioxide. Calculate how many breaths it takes an average person to "exhale" 1.00 kg of fat. Round your answer to the nearest thousand. You'll need to know that the density of CO₂ is 2.0 kg/m³. 0 ☐ ☐x10 X
1. More than 2000 years ago human cultures figured out a way to produce iron metal from rocks containing iron ores. This iron could be worked by a blacksmith (repeated heating and hammering) to make iron metal pure enough for creating useful tools (even Samurai swords). This direct heating technique was common up until about 200 years ago when people found a better way to obtain iron metal. When hematite, Fe2O3(s), is strongly heated in a blast furnace in the presence of charcoal (carbon), pure iron metal is obtained. Fe2O3() 2 Fe(s) + 3/2 O2 (g) (1) C(s) + O2 (g) → CO2(g) (2) When reaction 1 is coupled to reaction 2, overall chemical equation is Fe2O3() + 3/2 C() 3/2 CO2(g) + 2 Fee) Use the thermodynamic data given below for the following calculations: AG¡ (kJ/mol) | 4H¡ (kJ/mol) | S (J/mol-K) Fe2O3(s) -742.2 -824.2 87.40 Fes) 27.28 CO2(8) -394.36 -393.51 213.74 C (6) 5.74 O2 (2) 205.14 a) Calculate the standard Gibb's free energy change for reaction 1 b) Calculate the standard Gibb’s…
Consider the reaction. heat 2 Al(s) + Fe,0,(s) Al, 0,(s) + 2 Fe(1) If 10.7 kg Al reacts with an excess of Fe, O3, how many kilograms of Al,O, will be produced? mass of Al, O, produced: kg * TOOLS x10
For eac te, click the button under the better solvent. solute Which is the better solvent? :0: || :0: :0: CH,-S CH, НО -С — СH, — CH, — С — ОН CH;CH,OH CH; H C H
Nitric acid is often manufactured from the atmospheric gases nitrogen and oxygen, and hydrogen prepared by reforming natural gas, in a two-step process. In the first step, nitrogen and hydrogen react to form ammonia: N₂(g) + 3H₂(g) 2 NH, (g) In the second step, ammonia and oxygen react to form nitric acid (HNO3) and water: NH₂ (g) + 20₂(g) → HNO3(g) + H₂O (g) Suppose the yield of the first step is 61.% and the yield of the second step is 77.%. Calculate the mass of nitrogen required to make 10.0 kg of nitric acid. Be sure your answer has a unit symbol, if needed, and is rounded to 2 significant digits. 0 Explanation Check. ☐ x10 8 X 09 0.0 S © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center |
6. Write the expression for Kc for the following reactions. In each case indicate whether the reaction is homogeneous or heterogeneous. a. CH4 (g) + H2S (g) → CS2(g) + H2 (g) HF + F¯ (aq) b. (aq) ⇒ H* (aq) c. Ti (s) + Cl2 (g) → TiCl4 (1) d. HCI (aq) + O2 (g) → H₂O (1) + 2 Cl2 (g)
Balance the following reactions. Type a property balance reaction equation.
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: P4(1)+5 0,(g) 2 P,05(g) In the second step, diphosphorus pentoxide and water react to form phosphoric acid: P,0,(g)+3 H,O(1)→2 H,PO,(1) Write the net chemical equation for the production of phosphoric acid from phosphorus, oxygen and water. Be sure your equation is balanced.
15 - Which of the following represents a precipitation reaction?