This problem can be solved using the ideal gas law, which states that the volume of a gas is directly proportional to the number of moles of the gas if the temperature and pressure are held constant. This can be expressed as V1/n1 = V2/n2, where V1 and n1 are the initial volume and number of moles, and V2 and n2 are the final volume and number of moles.

Step 1: Identify the initial volume (V1) and number of moles (n1). From the problem, we know that V1 = 1.90 L and n1 = 0.0920 mol.

Step 2: Identify the final number of moles (n2). The problem states that 0.0210 mol of helium is added to the balloon, so n2 = n1 + 0.0210 mol = 0.0920 mol + 0.0210 mol = 0.113 mol.

Step 3: Solve for the final volume (V2) using the equation V1/n1 = V2/n2. Rearranging the equation to solve for V2 gives V2 = V1 * (n2/n1) = 1.90 L * (0.113 mol / 0.0920 mol) = 2.33 L.

So, the new volume of the balloon is 2.33 L.

Question

This problem can be solved using the ideal gas law, which states that the volume of a gas is directly proportional to the number of moles of the gas if the temperature and pressure are held constant. This can be expressed as V1/n1 = V2/n2, where V1 and n1 are the initial volume and number of moles, and V2 and n2 are the final volume and number of moles.

Step 1: Identify the initial volume (V1) and number of moles (n1). From the problem, we know that V1 = 1.90 L and n1 = 0.0920 mol.

Step 2: Identify the final number of moles (n2). The problem states that 0.0210 mol of helium is added to the balloon, so n2 = n1 + 0.0210 mol = 0.0920 mol + 0.0210 mol = 0.113 mol.

Step 3: Solve for the final volume (V2) using the equation V1/n1 = V2/n2. Rearranging the equation to solve for V2 gives V2 = V1 * (n2/n1) = 1.90 L * (0.113 mol / 0.0920 mol) = 2.33 L.

So, the new volume of the balloon is 2.33 L.

Knowee AI · Accepted Answer

This problem can be solved using the ideal gas law, which states that the volume of a gas is directly proportional to the number of moles of the gas if the temperature and pressure are held constant. This can be expressed as V1/n1 = V2/n2, where V1 and n1 are the initial volume and number of moles, and V2 and n2 are the final volume and number of moles.

Step 1: Identify the initial volume (V1) and number of moles (n1). From the problem, we know that V1 = 1.90 L and n1 = 0.0920 mol.

Step 2: Identify the final number of moles (n2). The problem states that 0.0210 mol of helium is added to the balloon, so n2 = n1 + 0.0210 mol = 0.0920 mol + 0.0210 mol = 0.113 mol.

Step 3: Solve for the final volume (V2) using the equation V1/n1 = V2/n2. Rearranging the equation to solve for V2 gives V2 = V1 * (n2/n1) = 1.90 L * (0.113 mol / 0.0920 mol) = 2.33 L.

So, the new volume of the balloon is 2.33 L.

A balloon has been filled to a volume of 1.90 L with 0.0920 mol of helium gas. If 0.0210 mol of additional helium is added to the balloon while the temperature and pressure are held constant, what is the new volume of the balloon?

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