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Write the equilibrium expression for the value of Q in the given reaction below.
a). 2 NOBr(g)←→2 NO(g)+Br2(g)
b). 2 NO(g)+Br(2)(g)←→2 NOBr(g)
c). NH3(g)+HCl(g)←→NH4Cl(s)
Write the equilibrium expression for the value of K, in the given reaction below.
(A). 2 O3(g)←→3 O2(g)
(B). 2 NO(g)+Cl(g)←→2 NOCl(g)
(C). Ag+(aq)+2 NH3(aq)←→Ag(NH3)2+(aq)
Calculate the standard entropy change for the following using the table of standard values.(first, predict the sign for ∆S qualitatively)
2H2(g)+O2(g)→2H2O(g)
Explain chemical thermodynamics
Spontaneous for T>0°C
Spontaneous for T<0°C
What is the above words all about?
What is the spontaneous reaction based from the observation from the given above?
Determine and describe the factors that involve in the reaction:
Temperature
Sizes and shape
Motion
380.0 cm3 hydrogen gas was collected over water at 23c and 613 find the volume of dry hydrogen at stp (vapour pressure of water at 23c=21 torr)
How many grams of potassium chloride are needed to make 1L of a 0.400M potassium chloride solution
How many grams of potassium chloride are needed to make 1L of a 0.400M potassium chloride solution
5 g of zinc pieces are added to 400 cm³ of 0.5 mol. dm-3 hydrochloric acid. To investigate the average rate of the reaction, the change in the mass of the flask containing the since and the acid is measured by placing the flask on a direct reading balance. The reading on the balance shows that there is a decrease in mass during the reaction. The reaction which takes place is given by the following equation: Zn(s)+2HCl(aq)→ZnCl2(aq)+H2(g)
Why is there a decrease in mass during the reaction?
The experiment is repeated, this time using 5 g of powdered zinc instead of pieces of zinc. How will this influence the average rate reaction?
The experiment bus repeated once more,this time using 5 g of the zinc pieces of 600 cm³ of 0.5 mol.dm-3 hydrochloric acid. How does the average rate of this reaction compare with the original reaction rate?
What effect would a catalyst have on the average rate of this reaction?
5 g zinc are added to 400 cm 3 or 0.5 mol. dm-3 hydrochloric acid. To investigate the average rate of the reaction, the change in the mass of the flask containing the since and the acid is measured by placing the flask on a direct reading balance. The reading on the balance shows that there is a decrease in mass during the reaction. The reaction which takes place is given by the following equation: Zn(s)+2HCl(aq)→ZnCl2(aq)+H2(g)
