When 2.00 mol of SO2Cl2 is placed in a 5.00-L flask at 310 K, 40% of the SO2Cl2 decomposes to SO2 and Cl2: (a) Calculate Kc for this reaction at this temperature. (b) Calculate Kp for this reaction at 310 K. (c) According to Le Chatelier's principle, would the percent of SO2Cl2 that decomposes increase, decrease or stay the same if the mixture was transferred to a 1.00-L vessel? (d) Use the equilibrium constant you calculated above to determine the percentage of SO2Cl2 that decomposes when 2.00 mol of SO2Cl2 is placed in a 1.00-L vessel at 310 K.

the equation that correctly represent the reaction for formation of ammonia is

n2+ 3h2 → 2nh3 (answer d)

1 mole of nitrogen gas (n2) react with 3 moles of hydrogen gas (h2) to form 2 moles of ammonia ( nh3). this is in a process known as haber process were iron is used as a catalyst and reaction take place that a higher temperature and pressure. the process is exothermic hence energy is released.

number of molecules / avogadro's number * molecule molecular = mass

explanation:

we define a gram-molecular weight as the mass of one mole of any element or compound. a mole contains avogadro's number of units (molecules) –  

6.022

x

10

23

. so, dividing the number of molecules by avogadro's number gives us the number of moles. multiplying that by the molecular weight gives us the mass. from the periodic table we find the gram-molecular weight of u to be238 and of f to be19. so,  

u

f

6

will have a gram-molecular weight of 352g.

c, liquids evaporate, creating a gas

it takes on an electronical energy