- Volume of oxygen at NTP, required to completely burn 1 kg of coal (100% a..
- Volume at NTP of oxygen required to completely burn 1 kg of coal (100 % carbon) is:(A) $22.4$L(B) $22.4 \\times {10^3}$L(C) $1.86 \\times {10^3}$L(D) $1000$L
- [Solved] For complete combustion of 1 kg of Carbon, the required Oxyg
Download: Volume at ntp of oxygen required to completely burn 1 kg of coal
Size: 62.4 MB
Volume of oxygen at NTP, required to completely burn 1 kg of coal (100% a..
Question 1 n 2 = n 1 e x p [ − m g ( h 2 − h 1 ) / k B T ] where n 2 , n 1 refer to number density at heights h 2 and h 1 respectively. Use this relation to derive the equation for sedimentation equilibrium of a suspension in a liquid column: n 2 = n 1 e x p [ − m g N A ( ρ − ρ ′ ) ( h 2 − h 1 ) / ( ρ RT )] where ρ is the density of the suspended particle and ρ ′ that of surrounding medium. [N A is Avogadro's number, and R the universal gas constant.] [Hint : Use Archimedes principle to find the apparent weight of the suspended particle.]
Volume at NTP of oxygen required to completely burn 1 kg of coal (100 % carbon) is:(A) $22.4$L(B) $22.4 \\times {10^3}$L(C) $1.86 \\times {10^3}$L(D) $1000$L
Hint: First find out the moles of carbon. Then write the combustion reaction of coal and see the amount of oxygen required for combustion of 1 mole of carbon. Then use the unitary method to find out the amount of oxygen required. At NTP conditions 1 mole of a gas occupies 22.4 L of volume. Complete step by step solution: -First of all, let us find out the number of moles associated with 1 kg of carbon. The weight of coal given in the question is = 1 kg = 1000 g We know that number of moles = $\dfrac$) released during complete combustion causes a rise in atmospheric temperature. This leads to global warming.
[Solved] For complete combustion of 1 kg of Carbon, the required Oxyg
Concept: Mass of oxygen needed to completely burn fuel: \(m_o=\times m_f\) wherem o= mass of oxygen, m f= mass of fuel. Calculation: Given: m f= 1 Kg (mass of carbon) The basic reactions involved are: For carbon and oxygen C + O 2→ CO 2 1 mole Crequires 1mole of O 2. The mass of carbon is 12 gm, and oxygen is 16 gm. 1 mole of C = 12gm 2 moleof O 2= 2 × 16= 32gm Hence 32 gm of oxygen required to burn 12gm of carbon.
