Question

question 1 (1 point)
what is the temperature of a 1.59 l flask containing 0.175 mol of ne at a pressure of 1.09 atm?
121 k
217 k
336 k
829 k

Explanation:

Step1: Use ideal gas law

The ideal gas law is \(PV = nRT\). We need to solve for \(T\), so \(T=\frac{PV}{nR}\).

Step2: Substitute values

Given \(P = 1.09\ atm\), \(V=1.59\ L\), \(n = 0.175\ mol\), and \(R = 0.0821\ L\cdot atm/(mol\cdot K)\).

$$T=\frac{1.09\times1.59}{0.175\times0.0821}$$

Step3: Calculate

First, calculate the numerator: \(1.09\times1.59 = 1.7331\).
Then, calculate the denominator: \(0.175\times0.0821=0.0143675\).

$$T=\frac{1.7331}{0.0143675}\approx121\ K$$

Answer:

121 K