Advertisements
Advertisements
Question
Find the mass of KNO3 required to produce 126 kg of nitric acid. Find whether a larger or smaller mass of NaNO3 is required for the same purpose.
\[\ce{KNO3 + H2SO4 -> KHSO4 + HNO3}\]
\[\ce{NaNO3 + H2SO4 -> NaHSO4 + HNO3}\]
Solution
The molecular mass of KNO3 = 101 g
63 g of HNO3 is formed by = 101 g of KNO3
So, 126 Kg of HNO3 is formed by = `(126 xx 101)/63` = 202 kg
Now, The molecular mass of NaNO3 = 85 Kg
126 g of HNO3 is formed by `(85 xx 126)/63` = 170 kg of NaNO3
So, a smaller mass of NaNO3 is required.
APPEARS IN
RELATED QUESTIONS
Oxygen oxidises ethyne to carbon dioxide and water as shown by the equation:
\[\ce{2C2H2 + 5O2 -> 4CO2 + 2H2O}\]
What volume of ethyne gas at STP required to produce 8.4 dm3 of carbon dioxide at STP?
[H = 1, C = 12, O = 16]
Prove the Following :
Oxygen is a diatomic molecule.
Under the same conditions of temperature and pressure you collect 2L of carbon dioxide, 3L of chlorine, 5L of hydrogen, 4L of nitrogen and 1L of sulphur dioxide. In which gas sample will there be :
a. The greatest number of molecules.
b. The least number of molecules.
Justify your answer.
Samples of the gases O2, N2, CO2 and CO under the same conditions of temperature and pressure contain the same number of molecules represented by X. The molecules of Oxygen, occupy V litres and have a mass of 8 g. Under the same conditions of temperature and pressure :
What is the volume occupied by : X molecules of N2.
O2 is evolved by heating KCIO3 using MnO2 as a catalyst.
\[\ce{2KCI3 ->[MnO2] 2KCl + 3O2}\]
- Calculate the mass of KClO3 required to produce 6.72 litres of O2 at STP. [atomic masses of K = 39, Cl = 35.5, O = 16].
- Calculate the number of moles of oxygen present in the above volume and also the number of molecules.
- Calculate the volume occupied by 0.01 mole of CO2 at STP.
Solve the following:
What volume of oxygen is required to burn completely 90 dm3 of butane under similar conditions of temperature and pressure?
\[\ce{2C4H10 + 13O2 -> 8CO2 + 10H2O}\]
Give two tests of the following:
Water vapour
The reaction between 15 g of marble and nitric acid is given by the following equation:
\[\ce{CaCO3 + 2HNO3 -> Ca(NO3)2 + H2O + CO2}\]
Calculate the volume of carbon dioxide evolved at S.T.P.
1.56 g of sodium peroxide reacts with water according to the following equation:
\[\ce{2Na2O2 + 2H2O -> 4NaOH + O2}\]
Calculate the mass of sodium hydroxide formed.
What volume of oxygen is required to burn completely a mixture of 22.4 dm3 of methane and 11.2 dm3 of hydrogen into carbon dioxide and steam?
\[\ce{CH4 + 2O2 -> CO2 + 2H2O}\]
\[\ce{2H2 + O2 -> 2H2O}\]
