What is the value for this equation? Given: CO(g)+H2O(g)=co2(g)+H2(g) = 1.0 and initial concentrations are [CO2(g))= 2.0 M, [H2(g)]= 2.0 M, [CO(g)]= 1.0 M, [H2O(g)]= 1.0 M
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![What is the value for this equation? Given: CO(g)+H20(g)=CO2(g)+H2(g)
= 1.0 and initial concentrations are [CO2(g)]= 2.0 M, [H2(g)]= 2.0 M, [CO(g)]= 1.0 M, [H2O(g)]= 1.0 M](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5a207364-abe5-457b-ac18-b934c4bc22d8%2Fa1d403c5-7121-470c-aee2-56acb862d11a%2Fthpl9e_processed.jpeg&w=3840&q=75)
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- Ko is related to Ko by the equation K, = Kc (RT)An, What is the value of An for the reaction below? N2 (g) + 3H2 (g)= 2NH3 (g)1. When potassium dichromate (K2CRO4) is added to a solution containing 0.500 g silver nitrate (AGNO3), solid silver chromate (Ag2CrO4) is formed. ( Note: Be sure to write down the balanced chemical equation.) a) Determine the theoretical yield of the silver chromate precipitate. b) If 0.455 g of silver chromate is obtained, calculate the percentage yield.Silver dichromate, Ag2Cr2O7, is insoluble. It forms a brick red precipitate. Calculate the mass of silver dichromate produced when 50.0 mL of silver nitrate is added to 25.0 mL of 0.150 mol/L sodium dichromate.
- 3. Upon decomposition, a sample of sodium bicarbonate produces 0.0118 g of sodium carbonate, Na2CO3. How many grams of water does it produce? (Use the balanced equation from question #1). NaHCO3->Na2CO3+H2O+CO2For the reaction: Na2CO3(s) + CO2(g) + H2O (g) ↔ 2NaHCO3(s). The formula for computing Kc is?For the steam hydrocarbon reforming process, the equilibrium law expression is [CO₂(g)][H₂(g)]* [CH][H₂0² Kc The reaction described by this equilibrium is CH4 (a) + H₂O(g) = CO₂(g) + H₂(g) CH4 (q) + 2H₂O(g) = CO₂(g) + 4H₂(g) CO₂(g) + 4H₂(g) = CH₁ (a) +2H₂O(g) CO₂(g) + H₂ (a) CH4 (q) + H₂O(g)
- Write the equilibrium expression for Kc for the reaction: 2 O3(g) => 3 O2(g)Aluminum in the Al3 + form can be precipitated as Al (OH) 3, adding ammonia to an aluminum solution, but the precipitate is usually gelatinous and difficult to filter. Precipitation from a homogeneous solution provides a more filterable precipitate. The reaction used in this process is the hydrolysis of urea: (image attached) Suppose this reaction occurs in a 100.00 mL solution with an initial Al3 + concentration of 1.50x10-3 mol / L. How many moles of urea must be hydrolyzed to supply enough hydroxide to stoichiometrically combine Al3 + and form the precipitate Al (OH) 3?1. Consider the following reaction: 2 NO (g) + O2 (g) 2 2 NO2 (g); Kc = 6.9 x 105 A 5.0 L vessel contains 0.060 mol NO, 1.0 mol O2, and 0.80 mol NO2. Is this system at equilibrium? If the system is not at equilibrium, does the reaction proceed in the forward or reverse direction to reach equilibrium?
- If 30.0 g of LiOH is added to 0.650 L of 1.00 M Cd(NO₃)₂, how many grams of precipitate will be formed in the following precipitation reaction? a) Write a balanced equation. Identify a precipitate. Include states of matter. b) Determine how much precipitate would form if all reactant 1 ( LiOH) would be used up. c) Determine how much precipitate would form if all reactant 2 ( Cd(NO3 )2 would be used up. d) State Limiting reactant , and theoretical yield ( in grams) of the precipitate that would form from the given amounts.Consider three hypothetical ionic solids: AX,AX2, and AX3 (each X forms X-). Each of these solids has the same Ksp value, 5.5 x10-7. You place 0.25 mol of each compound in a separate container and add enough water to bring the volume to 1.0 dm3 in each case. Write the chemical equation for each of the solids dissolving in water. Would you expect the concentration of each solution to be 0.25M in the compound? Explain, in some detail, why or why not. Would you expect the concentrations of the A cations (A+, A2+, and A3+) in the three solutions to be the same? Does just knowing the stoichiometry of each reaction help you determine the answer, or do you need something else? Explain your answer in detail, but without doing any arithmetic calculations. Of the three solids, which one would you expect to have the greatest molar solubility? Explain in detail, but without doing any arithmetic calculations. e. Calculate the molar solubility of each compoundCalculate the volume of 02(g) that nust be supplied to completely burn 20.0 L of CHA(g). CHA(g) + 02(g) - -> CO2 (g) + 2 H20 (g)
