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Question- The following reaction have the indicated equilibrium constants at a particular temp: N2(g) + O2 (g) ->(double arrow) 2NO(g) with a kc= 4.3 X 10^-252NO(g) +O2(g) ->(double arrow) 2NO2 (g) at a kc= 6.4 X10^9. Determine the value of the Equilibrium constants for 2NO (g) +2NO2(g)->(double arrow) 3O2 (g) + 2N2 (g).
I am stuck in between this question please help me out
calculate the volume, in liters, occupied by 3.25 moles of Cl2 gas at 1.54 atm pressure and a temperature of 213 degrees celcius?
if the freezing point of a 0.106m CH3COOH solution is -0.323 degrees celcius, what is the percent of acid that has undergone ionization?
what is the condensed structural formula of
Question- For the reaction N2O4(g)↔2NO2(g), Kc=0.21 at 100 Celsius. At an early point during the reaction [N2O4(g)]= 0.12M and [NO2]= 0.55M. Is the reaction at equilibrium? If not, in which direction will it proceed
A 13 mL sample of a solution of AlBr3 was diluted with water to 27 mL. A 15 mL sample of the dilute solution was found to contain 0.044 moles of Br-. What was the concentration of AlBr3 in the original undiluted solution
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Balance the following redox reaction if it occurs in acidic solution. What are the coefficients in front of Zn and H+ in the balanced reaction. Zn^2+(aq) + NH4+(aq) yields Zn(s) + NO3-(aq)
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An aqueous solution of methylamine (CH3NH2) has a pH of 10.68. How many grams of methylamine are there in 100mL of the solution
As a chemist for an agricultural products company, you have just developed a new herbicide,"Herbigon," that you think has the potential to kill weeds effectively.
Problem- A volume of 80.0mL of aqueous potassium hydroxide (KOH) was titrated against a standard solution of sulfuric acid (H2SO4). What was the molarity of the KOH solution if 21.7mL of 1.50 M H2SO4 was needed
Mass of magnesium: 0.6 g Moles of magnesium. Mass of magnesium oxide: 1.00 g Moles of magnesium oxide
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