Question

2.35 x 1023 molecules of CO₂ gas are in a sealed container. What is the volume, in liters, of the container? 2. How do the following affect the position of equilibrium in the following reaction? CaC₂(s) + 2H₂O(g) ⇌ Ca(OH)₂(aq) + C₂H₂(g) a. addition of acetylene (C₂H₂) gas b. removal of some of the water c. increase in pressure d. removing some of the calcium hydroxide e. increase in volume of reaction container f. addition of more calcium carbide (CaC₂) For problem 1, you are required to show ONLY the last 2 steps - the answer and the step leading up to it. For example: a). 23 L + 51 L = 74 L b). 15.00 g /25.00 mL = 0.60 g/mL

A. Shifts to the right
B. Shifts to the left
C. No effect
D. Depends on temperature

Answer 1

To calculate the volume of C₂H₂ gas formed by the reaction of CaC₂ with water, you need to convert the mass of CaC₂ to moles, use the balanced equation to determine the mole ratio between CaC₂ and C₂H₂, and then use the ideal gas law equation to calculate the volume of C₂H₂ gas.

Step-by-step explanation:

To calculate the volume of C₂H₂ gas formed by the reaction of CaC₂ with water, you need to convert the mass of CaC₂ to moles, use the balanced equation to determine the mole ratio between CaC₂ and C₂H₂, and then use the ideal gas law equation to calculate the volume of C₂H₂ gas.

Here are the steps:

1. Convert the mass of CaC₂ to moles using its molar mass.
2. Use the balanced equation to determine the mole ratio between CaC₂ and C₂H₂.
3. Convert the moles of C₂H₂ to volume using the ideal gas law equation.

Using these steps, you can calculate the volume of C₂H₂ gas formed.