1 z Information Question 3 (4 points) Given: Kr (g) V: 59.4 L n: 6.675 mol T: 140.68 C What is the pressure in atmospheres? 3.82 atm 4.31 atm 4.62 atm 4.92 atm Question 4 (1 point)

To find the pressure in atmospheres, we can use the ideal gas law formula: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is ideal gas constant, and T is the temperature in Kelvin.

First, we need to convert the temperature from Celsius to Kelvin: T(K) = T(C) + 273.15

T(K) = 140.68 + 273.15 = 413.83 K

Next, we can plug in the given values into the ideal gas law formula:

P = (nRT) / V

P = (6.675 mol * 0.0821 atm*L/mol*K * 413.83 K) / 59.4 L

Calculating the pressure:

P = (220.03) / 59.4

P ≈ 3.70 atm

Therefore, the pressure is approximately 3.70 atm.

1 z Information Question 3 (4 points) Given: Kr (g) V: 59.4 L n: 6.675 mol T: 140.68 C What is the pressure in atmospheres? 3.82 atm 4.31 atm 4.62 atm 4.92 atm Question 4 (1 point)​

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1 z Information Question 3 (4 points) Given: Kr (g) V: 59.4 L n: 6.675 mol T: 140.68 C What is the pressure in atmospheres? 3.82 atm 4.31 atm 4.62 atm 4.92 atm Question 4 (1 point)