Question

Please help me, I’m stuck on this question

Answer 1

`\large \boxed{\text{0.0820 L$\cdot$atm$\cdot$K$^(-1)$mol}^(-1 )}`

Step-by-step explanation:

To solve this problem, we can use the Ideal Gas Law:

pV = nRT

Data:

p = 3.00 atm

V = 17.4 L

n = 2.00 mol

T = 45 °C

Calculations:

1. Convert the temperature to kelvins

T = (45 + 273.15) K = 318.15 K

2. Calculate the value of R

`\begin{array}{rcl}pV & = & nRT\\\text{3.00 atm} * \text{17.4 L} & = & \text{2.00 mol} * R * \text{318.15 K}\\\text{52.2 L$\cdot$atm} & = & 636.30R \text{ K$\cdot$mol}\\R & = & \frac{\text{52.2 L$\cdot$atm}}{636.30 \text{ K$\cdot$mol}}\\\\ & = & \textbf{0.0820 L$\cdot$atm$\cdot$K$^(-1)$mol}^(-1) \\\end{array}\\\text{The value of the gas constant R is $\large \boxed{\textbf{0.0820 L$\cdot$atm$\cdot$K$^(-1)$mol}^(-1 )}$}`