Consider the equilibrium describing the endothermic dissolution of a solid in water. Z n ( O H ) 2 ( s ) − ⇀ ↽ − Z n 2 + ( a q )
1 answer:
Answer:
- Add more zinc hydroxide.
- Increase the temperature.
Explanation:
Hello,
Based on the given chemical reaction at equilibrium:
Thus, by considering the Le Chatelier's principle, increasing the zinc hydroxide solubility, it means favor the direct reaction, could be attained by:
- Adding more zinc hydroxide as the addition of products favor the formation of products.
- As the reaction is endothermic, the energy is considered as a reactant, therefore, increasing the temperature the direct reaction is favored.
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<u>Answer:</u> The temperature in degree Celsius is 301.31°C
<u>Explanation:</u>
To calculate the temperature, we use the equation given by ideal gas, which is:
P = pressure of the gas = 670 torr = 0.882 atm (Conversion factor: 1 atm = 760 torr)
V = volume of gas = 42.5 L
n = number of moles of gas = 0.795 mol
R = Gas constant =
T = temperature of gas
Putting values in above equation, we get:
Converting the temperature from kelvins to degree Celsius, by using the conversion factor:
Hence, the temperature in degree Celsius is 301.31°C
Answer : The empirical formula of the compound is
Explanation :
The chemical equation for the combustion of hydrocarbon having carbon, hydrogen and oxygen follows:
where, 'x', 'y' and 'z' are the subscripts of Carbon, hydrogen and oxygen respectively.
We are given:
Mass of
Mass of
We know that:
Molar mass of carbon dioxide = 44 g/mol
Molar mass of water = 18 g/mol
For calculating the mass of carbon:
In 44 g of carbon dioxide, 12 g of carbon is contained.
So, in 1.043 g of carbon dioxide, of carbon will be contained.
For calculating the mass of hydrogen:
In 18 g of water, 2 g of hydrogen is contained.
So, in 0.5670 g of water, of hydrogen will be contained.
Mass of oxygen in the compound = (0.600) - (0.284 + 0.063) = 0.253 g
To formulate the empirical formula, we need to follow some steps:
Step 1: Converting the given masses into moles.
Moles of Carbon =
Moles of Hydrogen =
Moles of Oxygen =
Step 2: Calculating the mole ratio of the given elements.
For the mole ratio, we divide each value of the moles by the smallest number of moles calculated which is 0.0158 moles.
For Carbon =
For Hydrogen =
For Oxygen =
The ratio of C : H : O = 1.5 : 4 : 1
To make in a whole number we are multiplying the ratio by 2, we get:
The ratio of C : H : O = 3 : 8 : 2
Step 3: Taking the mole ratio as their subscripts.
The ratio of C : H : O = 3 : 8 : 2
Hence, the empirical formula for the given compound is