General Chemistry Answers

C (s) + O2(g) --> CO2 (g) is a chemical reaction in which the element Carbon reacts with Oxygen gas to produce Carbon Dioxide. According to table I on the Reference Tables, how much energy is released when during the following reaction: 2C (s) + 2O2 (g) --> 2CO2

Silicone carbide formula

if 4.4g of nitrogen combine with 11.46g tom produce a compound with a formula mass of 108.0amu what is the molecular formula for this compound

1. Ethylene glycol, commonly known as antifreeze is composed of 38.7 % C, 9.7 % H, 

and 51.6 % O. If the molecular mass of ethylene glycol is 192.6 g/mol, what is the molecular formula?

calculate the molar volume of argon at 100'C and 100 atm on the assumption that it is a van der waals gas

what is an atom

Alesia, decided to mix pure iodine and hydrogen gases and allowed 80 minutes an equilibrium to be reached. The equilibrium concentrations of iodine and hydrogen gases at 490oC were each found to be 3.00mol dm-3. These figures were confirmed by Tim, Alesia’s PhD research assistant, to be correct. 

(i). What was the equilibrium concentration of gaseous hydrogen iodide at this temperature if the equilibrium constant is 45?

(ii). What were the starting concentrations of reactants?

 The Kc for the reaction of tin(II) ions with iron(III) ions

Sn2+(aq)     +     2Fe3+(aq)            Sn4+(aq)     +     2Fe2+(aq)

is 1.0  X  1010 at room temperature of 298K. In an experiment conducted by Jessica under the watchful eye of Christine, at 25oC, in which solutions of SnCl2 and Fe(NO3)3 were mixed, the equilibrium concentration of tin ions were found to be 

Sn2+(aq)  =  0.050mol dm-3   and Sn4+(aq) =   0.040mol dm-3  

Calculate the concentrations of iron(III) and iron(II) ions at equilibrium.

.The equilibrium constant Kc for the dissociation of dinitrogen tetroxide

is 4.65  X  10-3 at 25oC.

N2O4(g)            2NO2(g)

[0.00020]=[NO2]

[0.098]= [N2O4]

Starting with 0.100mol of N2O4(g) in a 4.00L reaction vessel, calculate the concentrations of N2O4(g) and NO2(g) at equilibrium.

 Determine which, if any of the following reaction mixtures of N2O4 and NO2 are at equilibrium. For any that are not at equilibrium, state which direction the reaction would proceed to establish an equilibrium mixture.

N2O4(g)           2NO2(g) Kc  =  0.16 at 25oC

1. [N2O4(g)]  =  0.15M [NO2(g)]  =  0.65M Find Q (left)
   
2. [N2O4(g)]  =  0.68M [NO2(g)]  =  0.33M at equilibrium
   
3. [N2O4(g)]  =  0.30M [NO2(g)]  =  0.22M at equilibrium