# How many moles are in a gas in 890mL at 21 °C and 750 mmHg?

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To find the number of moles of a gas, you can use the ideal gas law equation:

[PV = nRT]

Where:

- (P) is the pressure in atmospheres (atm)
- (V) is the volume in liters (L)
- (n) is the number of moles
- (R) is the ideal gas constant ((0.0821) L·atm/mol·K)
- (T) is the temperature in Kelvin (K)

First, convert the volume from milliliters (mL) to liters (L): (890 \text{ mL} = 0.890 \text{ L})

Then, convert the temperature from Celsius to Kelvin: (21 °C + 273.15 = 294.15 \text{ K})

Plug in the values into the ideal gas law equation:

[750 \text{ mmHg} \times 1 \text{ atm} / 760 \text{ mmHg} = 0.987 \text{ atm}]

(PV = nRT) becomes (0.987 \text{ atm} \times 0.890 \text{ L} = n \times 0.0821 \text{ L·atm/mol·K} \times 294.15 \text{ K})

Solve for (n), the number of moles:

(0.877 \text{ atm·L} = n \times 24.189 \text{ L·atm/mol})

(n = \frac{0.877 \text{ atm·L}}{24.189 \text{ L·atm/mol}})

(n \approx 0.036 \text{ moles})

So, there are approximately 0.036 moles of gas in the given conditions.

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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

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