Home
Class 11
Chemistry
How much work is done by the gas when 1....

How much work is done by the gas when `1.00g` of sodium azide, `NaN_(3)` (`M=65.01 gxxmol^(-1)`), decomposes in a container of changeable volume (e.g. and airbag in a car) against a constant pressure of 1.00 atm at 298K?
`2NaN_(3)(s)to2Na(s)+3N_(2)(g)`

Promotional Banner

Similar Questions

Explore conceptually related problems

The work done during the expansion of a gas from a volume of 3 dm^(3) against a constant external pressure of 3 atm is (1 L atm = 101.3 J)

1.00 mol of N_(2) and 3.00 mol of H_(2) are present in a container of volume 10.0 dm^(3) at 298 K. What is the total pressure of the mixture?

2.8 g of N_(2) gas at 300 K and 20 atm was allowed to expand isothermally against a constant external pressure of 1 atm. Calculate W for the gas.

1 mole of gas occupying 3 litre volume is expanded against a constant external pressure of 1 atm to a volume of 15 litre. The work done by the system is:

An ideal gas expands in volume from 1 xx 10^(3) m^(3) at 300 K against a constant pressure of 1 xx 10^(5) N m^(-2) .The work done is

Calulate the work done (in cal.). When 1.0 mole of N_(2)H_(4) decomposes completely against a pressure of 1.0 atm at 27^(@)C (Given R=2 cal//mol//K) N_(2)H_(4)(l)toNH_(3)(g)+N_(2)(g)

1 mole of a gas occupying 3 L volume is expanded against a constant external pressure of 5 atm to a volume of 15 L. The work done by the system is __________ .

Indicate the incorrect statement for a 1 liter sample of N_(2)(g) and CO_(2)(g) at 298 K and 1 atm pressure