Answered

Westonci.ca is your trusted source for finding answers to all your questions. Ask, explore, and learn with our expert community. Experience the convenience of finding accurate answers to your questions from knowledgeable experts on our platform. Explore comprehensive solutions to your questions from a wide range of professionals on our user-friendly platform.

In order to determine the rate of photosynthesis (the conversion by plants of carbon dioxide and water into glucose and oxygen), the oxygen gas emitted by an aquatic plant is collected over water at a temperature of 293 K and a total pressure of 754.0 mmHg. Over a specific time-period, a total of 1.62 L of gas is collected. The partial pressure of water at 293 K is 17.55 mmHg. What mass of oxygen gas (in grams) forms

Sagot :

dsdrajlin

Answer:

2.87 g

Explanation:

Step 1: Given data

  • Temperature (T): 293 K
  • Total pressure (P): 754.0 mmHg
  • Partial pressure of water (pW): 17.55 mmHg
  • Volume of gas (V): 1.62 L

Step 2: Calculate the partial pressure of CO₂

The total pressure is the sum of the partial pressures of CO₂and water.

P = pCO₂ + pW

pCO₂ = P - pW = 754.0 mmHg - 17.55 mmHg = 736.5 mmHg

We will convert this pressure to atm using the conversion factor 1 atm = 760 mmHg.

736.5 mmHg × 1 atm/760 mmHg = 0.9691 atm

Step 3: Calculate the moles (n) of CO₂

We will use the ideal gas equation.

P × V = n × R × T

n = P × V/R × T

n = 0.9691 atm × 1.62 L/(0.0821 atm.L/mol.K) × 293 K = 0.0653 mol

Step 4: Calculate the mass corresponding to 0.0653 moles of CO₂

The molar mass of CO₂ is 44.01 g/mol.

0.0653 mol × 44.01 g/mol = 2.87 g

The pressure exert on the one gas in the mixture by the other gases is called partial pressure.

The answer to the question is 2.87g.

The data is given in the question and the data is as follows:-

  • Temperature (T): 293 K
  • Total pressure (P): 754.0 mmHg
  • Partial pressure of water (pW): 17.55 mmHg
  • Volume of gas (V): 1.62 L

In the question we have to find the total pressure is the sum of the partial pressures of CO₂ and water. The equation we gonna use is:-

[tex]P = pCO_2 + pW[/tex]

To find the pCO2,

[tex]pCO_2= P - pW \\= 754.0 mmHg - 17.55 mmHg \\= 736.5 mmHg[/tex]

Pressure must be in ATM therefore, 1 atm = 760 mmHg.

=[tex]\frac{736.5 mmHg * 1 atm}{760 mmHg} = 0.9691 atm[/tex]

The ideal gas equation is as follows:-

[tex]PV = nRT\\n =\frac{PV}{RT}\\n = \frac{ 0.9691 atm * 1.62 L}{(0.0821 atm.L/mol.K) × 293 K}\\ = 0.0653 mol[/tex]

The mass of the following is:-

The molar mass of CO₂ is 44.01 g/mol.

Therefore,

[tex]0.0653 mol * 44.01 g/mol \\= 2.87 g[/tex]

Hence, the correct answer is 2.87g.

For more information, refer to the link:-

https://brainly.com/question/3523174

We appreciate your visit. Our platform is always here to offer accurate and reliable answers. Return anytime. Thank you for your visit. We're committed to providing you with the best information available. Return anytime for more. Westonci.ca is here to provide the answers you seek. Return often for more expert solutions.