Calculate the change in internal energy (Delt | vedclass

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(A) Step $1$: Identify the given values.Heat absorbed $(q)$ = $+1800 	ext{ J}$ (positive as heat is absorbed).Pressure $(P)$ = $2 	ext{ bar} = 2 	i

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$1200$

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(A) Step $1$: Identify the given values.Heat absorbed $(q)$ = $+1800 	ext{ J}$ (positive as heat is absorbed).Pressure $(P)$ = $2 	ext{ bar} = 2 	imes 10^5 	ext{ Pa}$.Initial volume $(V_1)$ = $0.5 	ext{ dm}^3 = 0.5 	imes 10^{-3} 	ext{ m}^3$.Final volume $(V_2)$ = $3.5 	ext{ dm}^3 = 3.5 	imes 10^{-3} 	ext{ m}^3$.Step $2$: Calculate the work done $(w)$.$w = -P \Delta V = -P(V_2 - V_1)$.$w = -2 	imes 10^5 	ext{ Pa} 	imes (3.5 - 0.5) 	imes 10^{-3} 	ext{ m}^3$.$w = -2 	imes 10^5 	imes 3 	imes 10^{-3} 	ext{ J} = -600 	ext{ J}$.Step $3$: Calculate the change in internal energy $(\Delta U)$ using the first law of thermodynamics.$\Delta U = q + w$.$\Delta U = 1800 	ext{ J} + (-600 	ext{ J}) = 1200 	ext{ J}$.

Calculate the change in internal energy $(\Delta U)$ if an ideal gas expands from $0.5 \text{ dm}^3$ to $3.5 \text{ dm}^3$ at a constant pressure of $2 \text{ bar}$ by absorbing $1800 \text{ J}$ of heat energy. (in $\text{ J}$)

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