Answer :
Final answer:
The molecular weight of gases can be computed using the ideal gas law. Variables are substituted from condition data provided in each question, solve for moles and hence calculate molecular weight. STP (Standard Temperature and Pressure) conditions were utilized to answer question 6.
Explanation:
To calculate the molecular weight of a gas, we can use the ideal gas law (PV=nRT).
For question 3, the volume has to be in liters (which it is), the temperature in Kelvin (12.8°C + 273.15 = 286 K), and pressure in atmospheres (611.6 mmHg = 0.804 atm). Substitute the given values and solve for n (number of moles), then you can determine the molecular weight (n = m/M where M = m/n).
Similarly for question 5, use the gas constant R=8.314 and modify units as necessary, calculate the molecular weight.
For question 4, gas laws allows us to compare situations when a gas changes temperature. The volume, number of moles, and pressure of the neon gas are given and we are solving for T (temperature).
For question 6, STP conditions are used where the temperature is 273.15 K and the pressure is 1 atm. From this, we know that 1 mole of any gas occupies 22.4 liters at STP. So, calculate the molecular weight similar to question 3 and 5.
Ensure to maintain precision as instructed for significant figures in your calculations.
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Final answer:
The molecular weight of a gas can be calculated using the ideal gas law and the formula m/n (where m is the weight of the gas and n the number of moles). The temperature must be in Kelvin, and the pressure must be in atmospheres for calculations.
Explanation:
The molecular weight of a gas can be computed using the ideal gas law which is given as PV=nRT where P is the pressure, V is the volume, n is the moles of gas, R is the ideal gas constant, and T is the temperature. Here we can solve for n (the number of moles) and then use it to figure out the molecular weight (MW=m/n where m is mass of the gas).
Now, let's solve each question step-by-step:
- Question 3: Convert the pressure from mm Hg to atm (1 atm = 760 mmHg), also convert the temperature from °C to Kelvin by adding 273.15. Upon substituting the given values, we get n = 0.575 moles. Then, using the formula MW=m/n and substituting the values, we find MW = 172.70 g/mol.
- Question 4: Use the given values to compute the temperature using the ideal gas law, results is 266 K.
- Question 5: Convert pressure from kPa to atm (1 atm = 101.3 kPa). Solve for n and compute for MW as we did in the first question, and we find MW = 246.22 g/mol.
- Question 6: At STP, 1 mole of any gas occupies 22.4 L. Therefore, n can be calculated as V/22.4. Substituting the values, and solving for MW = 31.68 g/mol.
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