isme ye 6.0 kyu aaya

Question

ScanSolve AI Tutor · Accepted Answer

The value 6.0 is incorrect for the number of moles in this problem. It seems you might have incorrectly divided the volume by the pressure ( $12.0\ \text{L} / 2.0\ \text{atm} = 6.0$ ). However, to calculate the number of moles of a gas, you must use the Ideal Gas Law, which also accounts for temperature and the gas constant.

Here's the correct calculation:

Recall the Ideal Gas Law.
The Ideal Gas Law is given by $PV = nRT$ , where:
- $P$ = Pressure
- $V$ = Volume
- $n$ = Number of moles
- $R$ = Ideal Gas Constant
- $T$ = Temperature
Rearrange the formula to solve for the number of moles ( $n$ ).
$n = \frac{PV}{RT}$
Substitute the given values into the equation.
Given:
- $P = 2.0\ \text{atm}$
- $V = 12.0\ \text{L}$
- $T = 300\ \text{K}$
- $R = 0.0821\ \text{L atm/mol K}$
$n = \frac{(2.0\ \text{atm})(12.0\ \text{L})}{(0.0821\ \text{L atm/mol K})(300\ \text{K})}$
$n = \frac{24.0\ \text{L atm}}{24.63\ \text{L atm/mol}}$
$n \approx 0.9744\ \text{mol}$
Round to appropriate significant figures.
The given pressure (2.0 atm) has two significant figures, so the answer should also be rounded to two significant figures.
$n \approx 0.97\ \text{mol}$

The correct number of moles is approximately $0.97\ \text{mol}$ .

Isme ye 6.0 kyu aaya

Answer

Step-by-step solution

Recall the Ideal Gas Law.

Rearrange the formula to solve for the number of moles ( $n$ ).

Substitute the given values into the equation.

Round to appropriate significant figures.

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