Isobaric Expansion: Finding Internal Energy & Heat w/ 2.0 Moles Ideal Gas

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In the isobaric expansion of a monatomic ideal gas with 2.0 moles, the work done by the gas is -3600 J, and the change in temperature is calculated to be 216.6 K. To find the change in internal energy and heat, the equation for heat at constant pressure should be used, which incorporates the specific heat capacity of the gas. The relationship between work (W), heat (Q), and internal energy (ΔU) can be applied using the First Law of Thermodynamics, where ΔU = Q - W. By determining Q and using the known value of W, ΔU can be calculated. This approach effectively utilizes the properties of ideal gases and thermodynamic principles.
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I have a Pressure vs Volume Graph and A -> B.
It's just an isobaric expansion, the work done by the gas is -3600 J.
The gas is monatomic ideal (2.0moles).
If I used it correctly, PV=nRT, I found the change in temperature to be 216.6K.

My question is: How do I find the change in internal energy and heat? I don't have any info about the gas except that it's ideal and 2.0 moles worth.
 
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Use the equation for the amount of heat required to change the temperature of that gas (at constant pressure). You will have W and Q, then find delta U using the First Law.
 

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