in 1D there are 4g of Zinc. How many moles of Barium Hydroxide are required?

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To determine the number of moles of Barium Hydroxide required, we need to use the molar ratio between Zinc and Barium Hydroxide.

Here's how we can calculate it step by step:

Step 1: Determine the molar mass of Zinc (Zn)
The molar mass of Zinc can be found on the periodic table, and it is approximately 65.38 g/mol.

Step 2: Convert the mass of Zinc to moles
To convert the given mass of Zinc (4g) to moles, we can use the following formula:
moles = mass / molar mass

moles of Zn = 4g / 65.38 g/mol
moles of Zn ≈ 0.061 moles

Step 3: Determine the molar ratio between Zinc and Barium Hydroxide
The balanced chemical equation between Zinc (Zn) and Barium Hydroxide (Ba(OH)2) is needed to determine the molar ratio. Without that information, we cannot accurately determine the ratio. If you have the balanced equation, please provide it so we can proceed with the calculation.

Once you have the balanced equation, let's say it is:
Zn + 2Ba(OH)2 → Zn(OH)2 + 2Ba

In this case, the molar ratio between Zinc and Barium Hydroxide is 1:2, which means that for every 1 mole of Zinc, we need 2 moles of Barium Hydroxide.

Step 4: Calculate the moles of Barium Hydroxide required
Using the molar ratio, we can calculate the moles of Barium Hydroxide required:
moles of Barium Hydroxide = moles of Zn x (moles ratio of Ba(OH)2 / moles ratio of Zn)

moles of Barium Hydroxide = 0.061 moles x (2 moles Ba(OH)2 / 1 mole Zn)
moles of Barium Hydroxide = 0.122 moles

So, approximately 0.122 moles of Barium Hydroxide are required based on the given information.