Home
Class 11
CHEMISTRY
Assuming ideal behaviour, calculate Boyl...

Assuming ideal behaviour, calculate Boyle's law constant for each of the following gase at `25^(@)C`
a. 10g of `O_(2)` in 2 L container
b. 8g of `CH_(4)` in 5 L container

Text Solution

AI Generated Solution

To calculate Boyle's law constant for the given gases, we will use the formula for Boyle's law constant (K), which is defined as the product of pressure (P) and volume (V) at a constant temperature. According to the ideal gas law, we have: \[ PV = nRT \] Where: - \( n \) = number of moles of the gas - \( R \) = ideal gas constant - \( T \) = temperature in Kelvin ...
Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • STATES OF MATTER

    CENGAGE CHEMISTRY ENGLISH|Exercise Ex 5.3|16 Videos

  • STATES OF MATTER

    CENGAGE CHEMISTRY ENGLISH|Exercise Concept Application 5.3|1 Videos

  • STATES OF MATTER

    CENGAGE CHEMISTRY ENGLISH|Exercise Ex 5.1|15 Videos

  • SOME BASIC CONCEPTS AND MOLE CONCEPT

    CENGAGE CHEMISTRY ENGLISH|Exercise Archives Subjective|11 Videos

  • STOICHIOMETRY

    CENGAGE CHEMISTRY ENGLISH|Exercise Archives Subjective|33 Videos

Similar Questions

Explore conceptually related problems

Calculate the mass of each of the following at STP: 5.6L O_(2)

Calculate : the number of moles of O_(2) which contain 8.00 g of O_(2) .

Molar concentration of 96 g of O_(2) contained in a 2 L vessel is:

Calculate the volume strength of a hydrogen peroxide solution containing 60.7 g L^(-1) of H_(2)O_(2) .

Calculate the quantity of lime required to soften 10^(3)L of H_2O which contains 7.5 g L^(-1) of Ca(HCO_3)_2 and 5.0 g L^(-1) of Mg(HCO_3)_2

Three different containers contain three different gases with following parameter Container 1 of 67.2 L containing gas X at 0^@C and 1.01325 bar Container 2 of 44. 8L contaning gas Y at 546 K & 760 mm of Hg Container 3 of 89.6 L containing Z gas at 101325 N//m^2 & 0^@C Now they are mixed in single container. If gram molecular mass of X ,Y & Z are 10 g/mol, 20 g/mol and 40 g/mol respectively Then which of the following statements are correct

Calculate the ratio of number of molecules in 10 L of O_(2) and 10 L of N_(2) at 25^(@)C and 1 atm. State the law used in the calculation

Calculate relative rate of effusion of O_(2) to CH_(4) from a container container containing O_(2) and CH_(4) in 3 :2 mass ratio.

The heat librerated on complete combustion of 1 mole of CH_(4) gas to CO_(2)(g) and H_(2)O(l) is 890 kJ. Calculate the heat evolved by 2.4 L of CH_(4) on complete combustion. ( 1 mol of CH4 at 298K and 1 atm= 24L)

Calculate the equilibrium constant for the following reaction at 298 K: 2H_2O (l) to 2H_2(g) + O_2(g) Given : Delta_fG^@ [ H_2O (l)] = - 273.2 kJ mol^(-1) R = 8.314 J mol^(-1) K^(-1) .

Home
Profile