QuestionA gas mixture at 1.0 atm has $P_{N_2}=5C$ mm Hg, $P_{CO_2}=0.3$ mm Hg, and $P_{others}=7.1$ mm Hg. Find $P_{Oxygen}$ .

Studdy Solution

STEP 1

Question: What is the concept of pressure in a mixture of gases?
A) The pressure of each individual gas B) The sum of the pressures of all the gases C) The average pressure of the gases D) The pressure of the most abundant gas
Answer: B) The sum of the pressures of all the gases

STEP 2

Question: If the total pressure of a mixture of gases is 1.0 atm, what is it in mmHg?
A) 1.0 mmHg B) 760.0 mmHg C) 101325.0 mmHg D) 100.0 mmHg
Answer: B) 760.0 mmHg

STEP 3

Question: If the partial pressures of Nitrogen, Carbon Dioxide, and other gases are 593.4 mmHg, 0.3 mmHg, and 7.1 mmHg respectively, what is their total pressure?
A) 600.8 mmHg B) 600.0 mmHg C) 601.8 mmHg D) 599.8 mmHg
Answer: A) 600.8 mmHg

STEP 4

Question: If the total pressure of a mixture of gases is 760 mmHg and the total pressure of Nitrogen, Carbon Dioxide, and other gases is 600.8 mmHg, what is the partial pressure of Oxygen?
A) 159.2 mmHg B) 160.0 mmHg C) 160.2 mmHg D) 159.0 mmHg
Answer: A) 159.2 mmHg

STEP 5

Question: What is the correct formula to find the partial pressure of a gas in a mixture?
A) P_gas = P_total - P_other gases B) P_gas = P_total + P_other gases C) P_gas = P_total / P_other gases D) P_gas = P_total * P_other gases
Answer: A) P_gas = P_total - P_other gases

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QuestionA gas mixture at 1.0 atm has $P_{N_2}=5C$ mm Hg, $P_{CO_2}=0.3$ mm Hg, and $P_{others}=7.1$ mm Hg. Find $P_{Oxygen}$ .

Studdy Solution

STEP 1

Question: What is the concept of pressure in a mixture of gases?
A) The pressure of each individual gas B) The sum of the pressures of all the gases C) The average pressure of the gases D) The pressure of the most abundant gas
Answer: B) The sum of the pressures of all the gases

STEP 2

Question: If the total pressure of a mixture of gases is 1.0 atm, what is it in mmHg?
A) 1.0 mmHg B) 760.0 mmHg C) 101325.0 mmHg D) 100.0 mmHg
Answer: B) 760.0 mmHg

STEP 3

Question: If the partial pressures of Nitrogen, Carbon Dioxide, and other gases are 593.4 mmHg, 0.3 mmHg, and 7.1 mmHg respectively, what is their total pressure?
A) 600.8 mmHg B) 600.0 mmHg C) 601.8 mmHg D) 599.8 mmHg
Answer: A) 600.8 mmHg

STEP 4

Question: If the total pressure of a mixture of gases is 760 mmHg and the total pressure of Nitrogen, Carbon Dioxide, and other gases is 600.8 mmHg, what is the partial pressure of Oxygen?
A) 159.2 mmHg B) 160.0 mmHg C) 160.2 mmHg D) 159.0 mmHg
Answer: A) 159.2 mmHg

STEP 5

Question: What is the correct formula to find the partial pressure of a gas in a mixture?
A) P_gas = P_total - P_other gases B) P_gas = P_total + P_other gases C) P_gas = P_total / P_other gases D) P_gas = P_total * P_other gases
Answer: A) P_gas = P_total - P_other gases

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QuestionA gas mixture at 1.0 atm has PN2=5CP_{N_2}=5CPN2​​=5C mm Hg, PCO2=0.3P_{CO_2}=0.3PCO2​​=0.3 mm Hg, and Pothers=7.1P_{others}=7.1Pothers​=7.1 mm Hg. Find POxygenP_{Oxygen}POxygen​.

Studdy Solution

STEP 1

Question: What is the concept of pressure in a mixture of gases?A) The pressure of each individual gas B) The sum of the pressures of all the gases C) The average pressure of the gases D) The pressure of the most abundant gasAnswer: B) The sum of the pressures of all the gases

STEP 2

Question: If the total pressure of a mixture of gases is 1.0 atm, what is it in mmHg?A) 1.0 mmHg B) 760.0 mmHg C) 101325.0 mmHg D) 100.0 mmHgAnswer: B) 760.0 mmHg

STEP 3

Question: If the partial pressures of Nitrogen, Carbon Dioxide, and other gases are 593.4 mmHg, 0.3 mmHg, and 7.1 mmHg respectively, what is their total pressure?A) 600.8 mmHg B) 600.0 mmHg C) 601.8 mmHg D) 599.8 mmHgAnswer: A) 600.8 mmHg

STEP 4

Question: If the total pressure of a mixture of gases is 760 mmHg and the total pressure of Nitrogen, Carbon Dioxide, and other gases is 600.8 mmHg, what is the partial pressure of Oxygen?A) 159.2 mmHg B) 160.0 mmHg C) 160.2 mmHg D) 159.0 mmHgAnswer: A) 159.2 mmHg

STEP 5

Question: What is the correct formula to find the partial pressure of a gas in a mixture?A) P_gas = P_total - P_other gases B) P_gas = P_total + P_other gases C) P_gas = P_total / P_other gases D) P_gas = P_total * P_other gasesAnswer: A) P_gas = P_total - P_other gases

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Studdy solves anything!

Start learning now

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QuestionA gas mixture at 1.0 atm has $P_{N_2}=5C$ mm Hg, $P_{CO_2}=0.3$ mm Hg, and $P_{others}=7.1$ mm Hg. Find $P_{Oxygen}$ .

Question: What is the concept of pressure in a mixture of gases?
A) The pressure of each individual gas B) The sum of the pressures of all the gases C) The average pressure of the gases D) The pressure of the most abundant gas
Answer: B) The sum of the pressures of all the gases

Question: If the total pressure of a mixture of gases is 1.0 atm, what is it in mmHg?
A) 1.0 mmHg B) 760.0 mmHg C) 101325.0 mmHg D) 100.0 mmHg
Answer: B) 760.0 mmHg

Question: If the partial pressures of Nitrogen, Carbon Dioxide, and other gases are 593.4 mmHg, 0.3 mmHg, and 7.1 mmHg respectively, what is their total pressure?
A) 600.8 mmHg B) 600.0 mmHg C) 601.8 mmHg D) 599.8 mmHg
Answer: A) 600.8 mmHg

Question: If the total pressure of a mixture of gases is 760 mmHg and the total pressure of Nitrogen, Carbon Dioxide, and other gases is 600.8 mmHg, what is the partial pressure of Oxygen?
A) 159.2 mmHg B) 160.0 mmHg C) 160.2 mmHg D) 159.0 mmHg
Answer: A) 159.2 mmHg

Question: What is the correct formula to find the partial pressure of a gas in a mixture?
A) P_gas = P_total - P_other gases B) P_gas = P_total + P_other gases C) P_gas = P_total / P_other gases D) P_gas = P_total * P_other gases
Answer: A) P_gas = P_total - P_other gases