Multiple Choice
In the reaction 2 H_2 + O_2 → 2 H_2O, how many moles of water (H_2O) are produced from 13.35 mol of oxygen (O_2)?
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3. Chemical Reactions
Stoichiometry
Multiple Choice
How many grams of SiH_4 contain 8.23 \(\times\) 10^{22} atoms of hydrogen?
A
2.40 g
B
1.20 g
C
0.60 g
D
0.15 g
Verified step by step guidance1
Identify the given information: the number of hydrogen atoms is \(8.23 \times 10^{22}\) atoms, and the compound is silane, \(\mathrm{SiH_4}\).
Determine the number of hydrogen atoms per molecule of \(\mathrm{SiH_4}\). Since the formula is \(\mathrm{SiH_4}\), each molecule contains 4 hydrogen atoms.
Calculate the number of \(\mathrm{SiH_4}\) molecules corresponding to the given hydrogen atoms by dividing the total hydrogen atoms by 4: \(\text{molecules of } \mathrm{SiH_4} = \frac{8.23 \times 10^{22}}{4}\).
Use Avogadro's number (\(6.022 \times 10^{23}\) molecules/mol) to convert the number of molecules to moles of \(\mathrm{SiH_4}\): \(\text{moles of } \mathrm{SiH_4} = \frac{\text{number of molecules}}{6.022 \times 10^{23}}\).
Calculate the mass of \(\mathrm{SiH_4}\) by multiplying the moles by the molar mass of \(\mathrm{SiH_4}\). The molar mass is calculated as \(28.09 \text{ g/mol (Si)} + 4 \times 1.008 \text{ g/mol (H)}\). Then, \(\text{mass} = \text{moles} \times \text{molar mass}\).
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