2NH3(g)+46kJ⇌N2(g)+3H2(g) adding more H2 (g)O The equilibrium concentration of NH3 will increase.The equilibrium concentration of NH, will decrease.The equilibrium ooncentration of NH3 will not change.SubmitRequest AnswerPart Bincreasing the temperature of the reactionO The equilibrium concentration of NH3 will decrease.The equilibrium concentration of NH, will increase.O The equilibrium concentration of NH3 will not change.SubmitReguest AnswerPart Cincreasing the volume of the containerO The equilibrium concentration of NH3 will decrease.O The equilibrium concentration of NH3 will increase.The equilibrium concentration of NH3 will not change.SubmitRequest AnswerPart Ddecreasing the volume of the containerThe equilibrium concentration of NH3 will decrease.O The equilibrium concentration of NH3 will increase.O The equilibrium concentration of NH, willchange.SubmitRequest AnswerPart Eadding a catalystO The equilibrium concentration of NH3 will increase.O The equilibrium concentration of NH, will decrease.The equilibrium concentration of NH3 will not change.

“Since you have posted a question with multiple sub-parts, we will solve first three sub- parts for…

adding more na O The equilibrium concentration of NH3 will increase. The equilibrium concentration of NH, will decrease. O The equilibrium concentration of NH3 will not change. Submit Request Answer Part B increasing the temperature of the reaction O The equilibrium concentration of NH3 will decrease. The equilibrium concentration of NH, will increase. O The equilibrium concentration of NH, will not change. Submit Reguest Answer Part C increasing the volume of the container O The equilibrium concentration of NH, will decrease. O The equilibrium concentration of NH3 will increase. O The equilibrium concentration of NH, will not change.

adding more na O The equilibrium concentration of NH3 will increase. The equilibrium concentration of NH, will decrease. O The equilibrium concentration of NH3 will not change. Submit Request Answer Part B increasing the temperature of the reaction O The equilibrium concentration of NH3 will decrease. The equilibrium concentration of NH, will increase. O The equilibrium concentration of NH, will not change. Submit Reguest Answer Part C increasing the volume of the container O The equilibrium concentration of NH, will decrease. O The equilibrium concentration of NH3 will increase. O The equilibrium concentration of NH, 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...

See similar textbooks

Similar questions

Hydrogen is manufactured on an industrial scale by this sequence of reactions: CH4 (g) + H₂O(g) = CO (g) + 3H₂(g) CO(g) + H₂O(g) = CO₂ (g) + H₂(g) The net reaction is: CH4 (g) + 2 H₂O(g) = CO₂(g) + 4H₂(g) Write an equation that gives the overall equilibrium constant K in terms of the equilibrium constants K₁ and K₂. If you need to include any physical constants, be sure you use their standard symbols, which you'll find in the ALEKS Calculator. K = 0 ロ・ロ X K₁ K₂ 4 K
The human body burns glucose (C6H₁2O6) for energy according to this chemical reaction: C6H₁206+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 2.8 kg of carbon dioxide. Calculate how many breaths it takes an average person to "exhale" 3.00 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 X
Acetylene torches are used for welding. These torches use a mixture of acetylene gas, C2H2C2H2, and oxygen gas, O2O2 to produce the following combustion reaction: 2C2H2(g)+5O2(g)→4CO2(g)+2H2O(g)2C2H2(g)+5O2(g)→4CO2(g)+2H2O(g) Part A Imagine that you have a 7.00 LL gas tank and a 4.50 LL gas tank. You need to fill one tank with oxygen and the other with acetylene to use in conjunction with your welding torch. If you fill the larger tank with oxygen to a pressure of 125 atmatm , to what pressure should you fill the acetylene tank to ensure that you run out of each gas at the same time? Assume ideal behavior for all gases. Express your answer with the appropriate units.
Hh.81.
Hydrogen peroxide, H2O2, decomposes according to the equation below (see attached image). This reaction is thermodynamically favorable at room temperature. 2 H2O2(aq) ィ 2 H2O(l) + O2(g) (a) A particulate representation of the reactants is shown below in the box on the left. In the box below on the right, draw the particulate representation of all the molecules that would be produced from these four reactant molecules.
A household water heater containing 50 gallons (227 L) of water is heated burning natural gas (methane, molar mass = 16.043 g mol-1) via the following reaction: CH4(g) + O2(g) CO2(g) + H20(O A,H = -891 kJ mol-1 What mass of methane, in units of g, is needed to heat the 227 L of water in the heater from 25.0°C to 44.0°C? Assume: • the heater is 100% efficient in its use of heat energy • no heat is lost to the surroundings specific heat of water is: 4.184 Jg-1 °C-1 density of water is: 0.9970 g mL¯1
Classify each chemical reaction.
Dimethyl ether, a useful organic solvent, is prepared in two steps. In the first step, carbon dioxide and hydrogen react to form methanol and water: CO₂(g) + 3H₂(g) → CH₂OH(/) + H₂O(1) In the second step, methanol reacts to form dimethyl ether and water: 2 CH3OH(1) > CH3OCH3(9) + H₂O(1) ΔΗ = 8. kJ Calculate the net change in enthalpy for the formation of one mole of dimethyl ether from carbon dioxide and hydrogen from these reactions. Round your answer to the nearest kJ. ☐ kJ X AH-131. kJ
Br (CH3)¿CuLi CuLi Br K H20 MgBr H20 M МоBr
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 4(aq) Cu(s) + FeSO4(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 450. 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 147. mg. Calculate the original concentration of copper(II) sulfate in the sample. Round your answer to 3 significant digits. ?
What is the mass of 5.22 x 1021 formula units of sodium hydroxide: NaOH (Mw. 40.00 g/mol)?
Dimethyl ether, a useful organic solvent, is prepared in two steps. In the first step, carbon dioxide and hydrogen react to form methanol and water: CO₂(g) + 3 H₂(g) CH₂OH(1) + H₂O(1) In the second step, methanol reacts to form dimethyl ether and water: 2 CH₂OH(1)→ CH₂OCH3(g) + H₂O(1) Calculate the net change in enthalpy for the formation of one mole of dimethyl ether from carbon dioxide and hydrogen from these reactions. Round your answer to the nearest kJ. เม kJ AH=-131. kJ Ś ΔΗ= 8. kJ