question 3\n10 pts\ntrue or false? when the temperature of a gas in a 8 - l balloon drops from 50 degrees…

question 3\n10 pts\ntrue or false? when the temperature of a gas in a 8 - l balloon drops from 50 degrees celsius to 25 degrees celsius, the volume decreases to 4 l.\ntrue\nfalse\nquestion 4\n10 pts\ncalculate the pressure of 1.8 moles of oxygen in a 2.5 l gas tank kept at 15.0°c.\n17 atm\n56 atm\n33 atm\n0.89 atm

question 3\n10 pts\ntrue or false? when the temperature of a gas in a 8 - l balloon drops from 50 degrees celsius to 25 degrees celsius, the volume decreases to 4 l.\ntrue\nfalse\nquestion 4\n10 pts\ncalculate the pressure of 1.8 moles of oxygen in a 2.5 l gas tank kept at 15.0°c.\n17 atm\n56 atm\n33 atm\n0.89 atm

Answer

Question 3

Explanation:

Step1: Convert temperatures to Kelvin

$T_1 = 50 + 273.15=323.15$ K, $T_2=25 + 273.15 = 298.15$ K, $V_1 = 8$ L. According to Charles's law $\frac{V_1}{T_1}=\frac{V_2}{T_2}$ for a constant - pressure and amount of gas.

Step2: Solve for $V_2$

$V_2=\frac{V_1T_2}{T_1}=\frac{8\times298.15}{323.15}\approx7.39$ L $\neq4$ L

Answer:

False

Question 4

Explanation:

Step1: Convert temperature to Kelvin

$T=15.0 + 273.15=288.15$ K, $n = 1.8$ mol, $V = 2.5$ L. Use the ideal - gas law $PV=nRT$, where $R = 0.0821$ L$\cdot$atm/(mol$\cdot$K).

Step2: Solve for $P$

$P=\frac{nRT}{V}=\frac{1.8\times0.0821\times288.15}{2.5}\approx17$ atm

Answer:

17 atm