Question
Calculate the amount of heat required to completely sublime50.0 g of solid dry ice (CO2) at its sublimation temperature. Theheat of sublimation for carbon dioxide is 32.3 kJ/mol.
Step 1
We can do this using the molar mass of carbon dioxide, which is 44.01 g/mol. The conversion is as follows: \[ \text{Moles of CO}_2 = \frac{\text{Mass of CO}_2}{\text{Molar mass of CO}_2} = \frac{50.0 \, \text{g}}{44.01 \, \text{g/mol}} \] Show more…
Show all steps
Your feedback will help us improve your experience
Christopher Nilsen and 89 other Chemistry 102 educators are ready to help you.
Ask a new question
Labs
Want to see this concept in action?
Explore this concept interactively to see how it behaves as you change inputs.
Recommended Videos
Calculate the amount of heat required to completely sublime 50.0 g of solid dry ice (CO2) at its sublimation temperature. The heat of sublimation for carbon dioxide is 32.3 kJ/mol.
Calculate the amount of heat required to completely sublime 50.0 g of solid dry ice $\left(\mathrm{CO}_{2}\right)$ at its sublimation temperature. The heat of sublimation for carbon dioxide is 32.3 $\mathrm{kJ} / \mathrm{mol}$ .
Calculate the amount of energy as heat absorbed by the sublimation of $100.0$ grams of dry ice (solid carbon dioxide). The value of $\Delta H_{\text {sub }}$ for $\mathrm{CO}_{2}$ is $25.2 \mathrm{k} J \cdot \mathrm{mol}^{-1}$
Transcript
18,000,000+
Students on Numerade
Trusted by students at 8,000+ universities
Watch the video solution with this free unlock.
EMAIL
PASSWORD