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Consider the following three reactions: 1. H2(g) + Cl2(g) ? 2HCl(g) 2. C(s) + H2O(g) ? CO(g) + H2(g) 3. Fe3O4(s) + 4H2(g) ? 3Fe(s) + 4H2O(g) For which of these is Kp not equal to Kc?? A) 1 only? B) 2 only? C) 3 only ?D) 1 and 2 only? E) 1 and 3 only
mercury has a density of 13.6 g per ml. a barometer holding 9.50ml of mercury has broken. the cost of mercury disposal
If 12.5 g of magnesium nitride is treated with water, what volume of ammonia gas would be collected at 28°C and 753 mm Hg?
How many gigagrams of niobium contain the same number of atoms as 12.5 nanograms of vanadium
the following set of data was obtained by the method of initial rates for the reaction: 2 HgCl(aq) +C2O42-(aq)-> 2Cl-(aq) + 2 CO2(g) + Hg2Cl2(s) what is te rate law for the reaction
Given the parent compound, draw the mass spectrum fragment that is observed at m/z 91. Include any hydrogen atoms and the charge.
Suppose that after delivery several drops of the water cling to the inner wall of the pipette (because the pipette is dirty). How does this technique error affect the reported density of water?
an automobile gasoline tank holds 21 kg of gasoline. when gasoline burs 81 kg of oxygen is consumed and carbon dioxide
A beaker with 130 mL of an acetic acid buffer with a pH of 5.00 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 M. A student adds 7.20 mL of a 0.370 M HCl solution to the beaker. How much will the pH..
Consider a solution formed by mixing 30.0 mL of 0.100 M H2SO4, 24.5 mL of 0.100 M HOCl, 25.0 mL of 0.200 M NaOH, 25.0 mL of 0.100 M Ca(OH)2, and 10.0 mL of 0.150 M KOH. Calculate the pH of this solution.
What would be the pressure of the gas, in kPa, if it were transferred to a container at 24°C whose volume is 55.0L?
How much heat must be supplied to 38 g of ice at -22°C to convert it to steam at 147°C? (Specific heats: ice = 2.0 J/g·°C; water = 4.2 J/g·°C; steam = 2.0 J/g·°C. Molar heat of fusion of water at 273 K = 6.01 kJ/mol. Molar heat of vaporization of ..
the standard free energy change delta G*T at 500K is equal to 9.8*10^4 J/mol. Calculte the equilibrium constant at 500 K.
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