500 J of energy is transferred as heat to 0. | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(A) Argon is a monoatomic gas,so $C_v = \frac{3}{2}R$ and $C_p = \frac{5}{2}R$. Since the process occurs at constant pressure $(1.00 \ atm)$,the heat

Vedclass · Accepted Answer

$348 \ K$ and $300 \ J$

Vedclass · Answer

(A) Argon is a monoatomic gas,so $C_v = \frac{3}{2}R$ and $C_p = \frac{5}{2}R$. Since the process occurs at constant pressure $(1.00 \ atm)$,the heat transferred is $q_p = n 	imes C_p 	imes \Delta T$. $500 = 0.5 	imes (\frac{5}{2} 	imes 8.3) 	imes (T_f - 298)$. $500 = 10.375 	imes (T_f - 298)$. $T_f - 298 = 48.19 \ K \Rightarrow T_f \approx 346.2 \ K$. However,checking the options,let us re-evaluate using $C_p = \frac{5}{2}R \approx 20.75 \ J \ K^{-1} \ mol^{-1}$. $500 = 0.5 	imes 20.75 	imes \Delta T \Rightarrow \Delta T = 48.19 \ K$. $T_f = 298 + 48.19 = 346.19 \ K$. For internal energy change: $\Delta U = n 	imes C_v 	imes \Delta T = 0.5 	imes (\frac{3}{2} 	imes 8.3) 	imes 48.19 \approx 300 \ J$. Given the options provided,$348 \ K$ is the closest value to $346.2 \ K$ and $\Delta U = 300 \ J$ is correct.

$500 \ J$ of energy is transferred as heat to $0.5 \ mol$ of Argon gas at $298 \ K$ and $1.00 \ atm$. The final temperature and the change in internal energy respectively are $:$ Given $: R = 8.3 \ J \ K^{-1} \ mol^{-1}$

Similar Questions

An ideal gas undergoes a reversible cyclic process as shown in the figure. The work done in this process is: (in $,V_1P_1$)

One mole of an ideal gas is allowed to expand freely and adiabatically into vacuum until its volume has doubled. Which of the following statements is $NOT$ true concerning this expansion?

One mole of an ideal gas for which $C_v = (3/2)R$ is heated at a constant pressure of $1 \ atm$ from $25 \ ^oC$ to $100 \ ^oC$. The value of $\Delta H$ is $...... \ cal$.

How much energy in $kJ$ is required to convert $54 \ g$ of ice at $0 \ ^\circ C$ to water at $27 \ ^\circ C$? $\left( \Delta H_{fusion} = 6.01 \ kJ \ mol^{-1}, C_{p(liquid)} = 4.18 \ J \ K^{-1} \ g^{-1} \right)$

$X \, g$ of ethanol $(CH_3CHO)$ is burnt in a bomb calorimeter and $Y \, J$ of heat is produced. Then,which of the following is correct for the enthalpy of combustion?

Vedclass Test Series

Exam Paper Generator

Online Exam Module