The temperature of a 500. ml sample of gas increases from 150. k to 350. k. what is the final volume of the sample of gas, if the pressure in the container is kept constant?

To solve this we assume that the sample gas is an ideal gas. Then, we can use the ideal gas equation which is expressed as PV = nRT. At a constant pressure and number of moles of the gas, the ratio T/V is equal to some constant. At another set of condition of temperature, the constant is still the same. Calculations are as follows:

T1 / V1 = T2 / V2

V2 = T2 x V1 / T1

V2 = 350 K x 500 mL / 150 K

V2 = 1166.67 mL

Therefore, the new volume of the system from the temperature change would be 1166.67 mL or about 1.2 L.

Spontaneity tell us the direction of the reaction, but not how fast it goes. gibbs free energy brings together enthalpy, entropy and temperature in one easy formula. g = h - ts. and, finally the sign of delta g is always negative for a spontaneous reaction.

The answer is letter c