Advertisements
Advertisements
Question
Potassium nitrate on strong heating decomposes as under :
2KNO3 → 2KNO2 + O2
Calculate : Weight of potassium nitrite formed.
(K = 39, 0 = 16, N = 14)
Advertisements
Solution
From the equation :
Molecular weight of KNO3 = (Atomic mass of K + Atomic mass of N + Atomic mass of O) = (39 + 14 + 16 x 3 ) = 101
Molecular mass of of KNO2 = (39 + 14 + 16 x 2) = 85
From the reaction :
2 moles of KNO3 gives = 2 moles of KNO2
So, 202g of KNO3 gives = 170g of KNO2
APPEARS IN
RELATED QUESTIONS
Give balanced chemical equations for the following conversions A, B, and C:
Mention the term defined by the following sentence:
The mass of a given volume of gas compared to the mass of an equal volume of hydrogen.
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 mass of CO2 in g?
What is the vapour density of ethylene? (Avogadro's number = 6 x 1023; Atomic weight of C = 12, H = 1; Molar volume = 22.4 litres at STP)
Explain the term:
Vapour density
Find the weight of 0.2 mole of H2 gas.
Calculate the mass of nitrogen supplied to soil by 5 kg of urea [CO(NH2)2].
[O = 16; N = 14; C = 12; H = 1]
The atomic mass of Chlorine is 35.5. What is its vapour density?
A gas cylinder can hold 1 kg of hydrogen at room temperature and pressure. What mass of carbon dioxide can it hold under similar conditions of temperature and pressure?
The following question refers to one mole of chlorine gas.
If the relative atomic mass of chlorine is 35.5, what will be the mass of 1 mole of chlorine gas?
