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Question 5.5: Ideal Gas Law . If there is 5.0 g of CO2 gas in a 10. L cyli...

Ideal Gas Law . If there is 5.0 g of CO_{2}  gas in a 10. L cylinder at 25°C, what is the gas pressure within the cylinder?

Strategy : We are given the quantity of CO_{2} in grams but, to use the ideal gas law, we must express the quantity in moles. Therefore, we must first convert grams of CO_{2} to moles CO_{2} , and then use this value in the ideal gas law. To convert from grams to moles, we use the conversion factor 1.00 mol CO_{2}  =  44 g CO_{2}.

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Step 1: Convert grams of CO_{2} to moles of CO_{2}.

5.0 \cancel{g CO_{2} }\times \frac{1 mol CO_{2} }{44 \cancel{g CO_{2} } } =0.11 mol CO_{2}

Step 2: We now use this value in the ideal gas equation to solve for the pressure of the gas. Note that temperature must be expressed in kelvins.

P=\frac{nRT}{V}

 

=\frac{nT}{V} \times R=\frac{(0.11 \cancel{mol}CO_{2} )(298 K)}{10L} \times \frac{0.0821 L .atm}{\cancel{mol} \cancel{K}} =0.27 atm

 

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