An experimenter adds 979 j of heat to an ideal gas to heat it from 10.6 c to 26.4 c at constant pressure. the gas does +221 j of work during the expansion. calculate the number of mol of gas. give an answer with 3 significant figures.

n = 0.594 mol

Explanation:

Parameters of the question.

Heat = 979J

Initial Temperature (T1) = 10.6 C =  283.6 K (converting to Kelvin by adding 273)

FinalTemperature (T2) = 26.4 C = 299.4 K (converting to Kelvin by adding 273)

ΔT =  T2 -T1 = 299.4 - 283.6 = 15.8K

Work done (W) = 221 J

number of moles (n) = ?

Formular to be used;

W=PΔV

From ideal gas equation,

PV = nRT

PΔV = nRΔT

where R = gas constant =  8.314 J / mol·K

Sunstituting in the work done equation,

we have W=nRΔT

Making n subject of formular,

n = [8.314 * 15.8]/221

n = 131.36/221

n = 0.594 mol