4.80g of Ch4 is mixed with 17.6g of co2 in a 9.00l flask at temprature of...

4.80g of Ch4 is mixed with 17.6g of co2 in a 9.00l flask at temprature of 67.2 degree celsius. what is the total pressure of the flask.(Assume there is no reaction)

Expert Solution

queen_honey_blossom answered 2 years ago

Question 2 options: For the reaction CH4 + O2 →CO2 + H2OCH4 + O2 →CO2 + H2O...

Question 2 options: For the reaction CH4 + O2 →CO2 + H2OCH4 + O2 →CO2 + H2O what are the coefficients for each reactant or product? a. CH4 b. O2 c. CO2 d. H2O Question 3 (2 points) Question 3 options: For the reaction NaOH + AlCl3 →NaCl + Al(OH)3NaOH + AlCl3 →NaCl + Al(OH) what are the coefficients for each reactant or product? a. NaOH b. AlCl3 c. NaCl d. Al(OH)3 Question 4 (2 points) Question 4 options: For the reaction H2O2...

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4a. For the following reaction, 3.96 grams of carbon tetrachloride are mixed with excess methane (CH4) . The reaction yields 3.67 grams of dichloromethane (CH2Cl2) . methane (CH4) ( g ) + carbon tetrachloride ( g ) -------> dichloromethane (CH2Cl2) ( g ) What is the theoretical yield of dichloromethane (CH2Cl2) ? _______ grams What is the percent yield for this reaction ? ________% 4b. For the following reaction, 5.03 grams of silver nitrate are mixed with excess copper(II) chloride....

Given the following chemical equations: I. CH4 + 2O2 → CO2 + 2H2O (1.25...

Given the following chemical equations: I. CH4 + 2O2 → CO2 + 2H2O (1.25 L of CH4 with density = 0.656 g/L) II. 6CO2 + 6H2O → C6H12O6 (7.25 g of CO2 ) Which equation will have the highest number of carbon atoms produced based on the information given next to each chemical equation? A. I B. II

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Be sure to answer all parts. Determine the mole fractions and partial pressures of CO2, CH4, and He in a sample of gas that contains 1.25 moles of CO2, 1.49 moles of CH4, and 3.61 moles of He, and in which the total pressure is 5.78 atm. ΧCO2 = PCO2 =-----atm ΧCH4 = PCH4 = -----atm ΧHe = PHe =---- atm

If 01.2 KOH is mixed with 0.05g of CO2 according to the following equation, 2KOH +...

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1.00atm of H2 and 1.00atm of Br2 were mixed in a 1.00L flask at 25°C. Under...

1.00atm of H2 and 1.00atm of Br2 were mixed in a 1.00L flask at 25°C. Under the appropriate conditions, gaseous HBr will form. At equilibrium, 1.10×10^13 molecules of H2 were found. Given the information below, calculate the values of K, delta G°, and delta S°. (for this problem, you do not have available values of free energies of formation and values of entropies of formation.) H2(g) + Br2(g) ----> 2HBr(g) delta H°= -103.8kJ

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