2) a 15.0 l container contains a mixture of 23 g of co₂ gas and 17 g of h₂s gas. if the temperature is 25.0…

Explanation:

Step1: Calculate moles of CO₂

The molar - mass of CO₂ is (M_{CO_2}=(12 + 2\times16)\text{ g/mol}=44\text{ g/mol}). Using the formula (n=\frac{m}{M}), for (m = 23\text{ g}) of CO₂, (n_{CO_2}=\frac{23\text{ g}}{44\text{ g/mol}}\approx0.523\text{ mol}).

Step2: Calculate moles of H₂S

The molar - mass of H₂S is (M_{H_2S}=(2\times1 + 32)\text{ g/mol}=34\text{ g/mol}). Using the formula (n=\frac{m}{M}), for (m = 17\text{ g}) of H₂S, (n_{H_2S}=\frac{17\text{ g}}{34\text{ g/mol}} = 0.5\text{ mol}).

Step3: Calculate total moles

(n_{total}=n_{CO_2}+n_{H_2S}=0.523\text{ mol}+0.5\text{ mol}=1.023\text{ mol}).

Step4: Convert temperature to Kelvin

(T=(25.0 + 273.15)\text{ K}=298.15\text{ K}), and (V = 15.0\text{ L}).

Step5: Use the ideal gas law (PV=nRT) to find total pressure

The ideal gas constant (R = 0.0821\text{ L}\cdot\text{atm}\cdot\text{mol}^{-1}\cdot\text{K}^{-1}). Rearranging the ideal - gas law for (P), we get (P=\frac{n_{total}RT}{V}). Substitute (n_{total}=1.023\text{ mol}), (R = 0.0821\text{ L}\cdot\text{atm}\cdot\text{mol}^{-1}\cdot\text{K}^{-1}), (T = 298.15\text{ K}), and (V = 15.0\text{ L}) into the formula: [P=\frac{1.023\text{ mol}\times0.0821\text{ L}\cdot\text{atm}\cdot\text{mol}^{-1}\cdot\text{K}^{-1}\times298.15\text{ K}}{15.0\text{ L}}] [P=\frac{1.023\times0.0821\times298.15}{15.0}\text{ atm}] [P\approx1.67\text{ atm}]

Answer:

(1.67\text{ atm})