If 1.00 mol of oxygen is heated at constant pressure of 1.00 atm from 10.0$^{\circ}$C to 25.0$^{\circ}$C.How much heat is absorbed by the gas?
A) 389 J
B) 544 J
C) 436 J
D) 288 J

Question

Quizplus · Accepted Answer

We can use the equation: q = nCpΔT, where q is the heat absorbed, n is the number of moles, Cp is the specific heat capacity at constant pressure, and ΔT is the change in temperature. 
First, we need to convert the temperature from Celsius to Kelvin. 
Initial temperature, Ti = 10.0°C + 273.15 = 283.15 K 
Final temperature, Tf = 25.0°C + 273.15 = 298.15 K 
Since the pressure is constant, we can use the specific heat capacity at constant pressure, which is Cp = 29.1 J/(mol*K) for oxygen gas. 
Substituting the values: 
q = (1.00 mol)(29.1 J/(mol*K))(298.15 K - 283.15 K) 
q = 435.9 J ≈ 436 J 
Therefore, the best choice is C, with q = 436 J of heat absorbed by the gas.

If 100 Mol of Oxygen Is Heated at Constant Pressure of of 1.00