when water is added to solid calcium carbide, CaC2, acetylene gas, C2H2, and calcium hydroxide, Ca(OH)2 are produced.
how many moles of calcium carbide are needed to completely react with 5.00 * 10^22 water molecules?
can someone explain the steps
See below.
To determine the number of moles of calcium carbide needed to completely react with 5.00 * 10^22 water molecules, we need to follow a few steps:
Step 1: Identify the balanced chemical equation representing the reaction between calcium carbide and water.
The balanced chemical equation for the reaction is:
CaC2 + 2H2O → C2H2 + Ca(OH)2
From this equation, we can see that 1 mole of calcium carbide (CaC2) reacts with 2 moles of water (H2O).
Step 2: Convert the number of water molecules to moles.
Given that there are 5.00 * 10^22 water molecules, we need to use Avogadro's number to convert them to moles.
Avogadro's number (NA) is 6.022 × 10^23 particles per mole.
Number of moles of water molecules = (5.00 * 10^22) / (6.022 × 10^23)
Step 3: Determine the number of moles of calcium carbide.
Since 1 mole of calcium carbide (CaC2) reacts with 2 moles of water (H2O), the number of moles of calcium carbide will be half of the number of moles of water.
Number of moles of calcium carbide = (Number of moles of water molecules) / 2
Now, you can substitute the value calculated in Step 2 into this equation to find the answer.
After calculating these steps, you will have the number of moles of calcium carbide needed to completely react with 5.00 * 10^22 water molecules.