A container has 2 g of gas A at 1 atm. 3 g of gas B is added. The total pressure becomes 1.5 atm. What is the molar mass of gas B?

April 1, 2026Chemistry

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April 1, 2026

Answer

2 $g,$ P_A = 1$ atm.

Here are the solutions to the problems:

Question 52: Step 1: Identify the given information and the relevant gas law. We are given:

Initial gas A: $m_A = 2$ g, $P_A = 1$ atm.
Added gas B: $m_B = 3$ g.
Final total pressure: $P_{total} = 1.5$ atm.
Temperature and volume are constant. For ideal gases at constant temperature and volume, pressure is directly proportional to the number of moles ( $P \propto n$ ). Also, $n = \frac{m}{M}$ . So, $P \propto \frac{m}{M}$ .

Step

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Question 52: Step 1: Identify the given information and the relevant gas law. We are given: Initial gas A: m_A = 2 g, P_A = 1 atm.

Asked on April 1, 2026Chemistry

This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.

ScanSolve AI AnswerAnswered on April 1, 2026

Here are the solutions to the problems: Question 52: Step 1: Identify the given information and the relevant gas law. We are given: Initial gas A: m_A = 2 g, P_A = 1 atm. Added gas B: m_B = 3 g. Final total pressure: P_total = 1.5 atm. Temperature and volume are constant. For ideal gases at constant temperature and volume, pressure is directly proportional to the number of moles (P n). Also, n = (m)/(M). So, P (m)/(M). Step