Multiple Choice
What volume, in liters, of sulfur dioxide gas at 455 K and 2.03 atm is needed to produce 89.6 g of sulfur trioxide, SO₃, according to the reaction: 2 SO₂(g) + O₂(g) → 2 SO₃(g)?
3. Chemical Reactions
Stoichiometry
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When 50.0 mL of 0.104 M HClO4 and 75.0 mL of 0.0753 M NaOH are combined, 291 J of heat are produced. If the initial temperature of both solutions was 22.5°C, determine the final temperature of the solution. Assume the density of the solution is 1.00 g/mL and the specific heat capacity is 4.18 J/g°C.
A
23.5°C
B
22.8°C
C
23.1°C
D
22.7°C
Verified step by step guidance1
Calculate the moles of HClO4 and NaOH using the formula \( \text{moles} = \text{concentration} \times \text{volume} \). For HClO4: \( 0.104 \text{ M} \times 50.0 \text{ mL} \) and for NaOH: \( 0.0753 \text{ M} \times 75.0 \text{ mL} \).
Determine the limiting reactant by comparing the moles of HClO4 and NaOH. The reaction is \( \text{HClO}_4 + \text{NaOH} \rightarrow \text{NaClO}_4 + \text{H}_2\text{O} \), which is a 1:1 ratio.
Calculate the total mass of the solution by adding the volumes of HClO4 and NaOH solutions and multiplying by the density: \( (50.0 \text{ mL} + 75.0 \text{ mL}) \times 1.00 \text{ g/mL} \).
Use the formula for heat transfer \( q = m \cdot c \cdot \Delta T \) to find the change in temperature \( \Delta T \). Rearrange to \( \Delta T = \frac{q}{m \cdot c} \), where \( q = 291 \text{ J} \), \( m \) is the total mass, and \( c = 4.18 \text{ J/g°C} \).
Add the change in temperature \( \Delta T \) to the initial temperature (22.5°C) to find the final temperature of the solution.
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