Multiple Choice
In the reaction 2Al + 3Cl_2 → 2AlCl_3, if 4.0 moles of Al are mixed with 6.0 moles of Cl_2, how many moles of the excess reactant remain after the completion of the reaction?
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3. Chemical Reactions
Stoichiometry
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A reaction requires 0.50 mol of H2SO4. What is the minimum mass of H2SO4 (in grams) needed to provide this amount?
A
19.6 g
B
49.0 g
C
25.0 g
D
98.0 g
Verified step by step guidance1
Identify the given quantity: 0.50 mol of H\_2SO\_4 is required.
Recall the molar mass of sulfuric acid (H\_2SO\_4). Calculate it by summing the atomic masses: 2 hydrogens, 1 sulfur, and 4 oxygens. Use the periodic table values (H = 1.0 g/mol, S = 32.1 g/mol, O = 16.0 g/mol).
Calculate the molar mass of H\_2SO\_4 using the formula: \(\text{Molar mass} = 2 \times 1.0 + 32.1 + 4 \times 16.0\) g/mol.
Use the relationship between moles, molar mass, and mass: \(\text{mass} = \text{moles} \times \text{molar mass}\).
Multiply the given moles (0.50 mol) by the molar mass of H\_2SO\_4 to find the minimum mass required in grams.
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