element mass fraction of rubidium iodide

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rubidium iodide | elemental composition

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$Find the elemental composition for rubidium iodide in terms of the atom and mass percents: atom percent = N_i/N_atoms × 100% mass percent = (N_im_i)/m × 100% Plan: • Write the chemical formula and gather atomic masses from the periodic table. • Determine values for N_i, m_i, N_atoms and m using these items. • Finally, compute the percents and check the results. Write the chemical formula: RbI Use the chemical formula, RbI, to count the number of atoms, N_i, for each element and find the total number of atoms, N_atoms: | number of atoms I (iodine) | 1 Rb (rubidium) | 1 N_atoms = 1 + 1 = 2 Divide each N_i by N_atoms to calculate atom fractions. Then use the property that atom fractions must sum to one to check the work: | number of atoms | atom fraction I (iodine) | 1 | 1/2 Rb (rubidium) | 1 | 1/2 Check: 1/2 + 1/2 = 1 Compute atom percents using the atom fractions: | number of atoms | atom percent I (iodine) | 1 | 1/2 × 100% = 50.0% Rb (rubidium) | 1 | 1/2 × 100% = 50.0% Look up the atomic mass, m_i, in unified atomic mass units, u, for each element in the periodic table: | number of atoms | atom percent | atomic mass/u I (iodine) | 1 | 50.0% | 126.90447 Rb (rubidium) | 1 | 50.0% | 85.4678 Multiply N_i by m_i to compute the mass for each element. Then sum those values to compute the molecular mass, m: | number of atoms | atom percent | atomic mass/u | mass/u I (iodine) | 1 | 50.0% | 126.90447 | 1 × 126.90447 = 126.90447 Rb (rubidium) | 1 | 50.0% | 85.4678 | 1 × 85.4678 = 85.4678 m = 126.90447 u + 85.4678 u = 212.37227 u Divide the mass for each element by m to calculate mass fractions. Then use the property that mass fractions must sum to one to check the work: | number of atoms | atom percent | mass fraction I (iodine) | 1 | 50.0% | 126.90447/212.37227 Rb (rubidium) | 1 | 50.0% | 85.4678/212.37227 Check: 126.90447/212.37227 + 85.4678/212.37227 = 1 Compute mass percents using the mass fractions: Answer: | | | number of atoms | atom percent | mass percent I (iodine) | 1 | 50.0% | 126.90447/212.37227 × 100% = 59.76% Rb (rubidium) | 1 | 50.0% | 85.4678/212.37227 × 100% = 40.24%$

Find the elemental composition for rubidium iodide in terms of the atom and mass percents: atom percent = N_i/N_atoms × 100% mass percent = (N_im_i)/m × 100% Plan: • Write the chemical formula and gather atomic masses from the periodic table. • Determine values for N_i, m_i, N_atoms and m using these items. • Finally, compute the percents and check the results. Write the chemical formula: RbI Use the chemical formula, RbI, to count the number of atoms, N_i, for each element and find the total number of atoms, N_atoms: | number of atoms I (iodine) | 1 Rb (rubidium) | 1 N_atoms = 1 + 1 = 2 Divide each N_i by N_atoms to calculate atom fractions. Then use the property that atom fractions must sum to one to check the work: | number of atoms | atom fraction I (iodine) | 1 | 1/2 Rb (rubidium) | 1 | 1/2 Check: 1/2 + 1/2 = 1 Compute atom percents using the atom fractions: | number of atoms | atom percent I (iodine) | 1 | 1/2 × 100% = 50.0% Rb (rubidium) | 1 | 1/2 × 100% = 50.0% Look up the atomic mass, m_i, in unified atomic mass units, u, for each element in the periodic table: | number of atoms | atom percent | atomic mass/u I (iodine) | 1 | 50.0% | 126.90447 Rb (rubidium) | 1 | 50.0% | 85.4678 Multiply N_i by m_i to compute the mass for each element. Then sum those values to compute the molecular mass, m: | number of atoms | atom percent | atomic mass/u | mass/u I (iodine) | 1 | 50.0% | 126.90447 | 1 × 126.90447 = 126.90447 Rb (rubidium) | 1 | 50.0% | 85.4678 | 1 × 85.4678 = 85.4678 m = 126.90447 u + 85.4678 u = 212.37227 u Divide the mass for each element by m to calculate mass fractions. Then use the property that mass fractions must sum to one to check the work: | number of atoms | atom percent | mass fraction I (iodine) | 1 | 50.0% | 126.90447/212.37227 Rb (rubidium) | 1 | 50.0% | 85.4678/212.37227 Check: 126.90447/212.37227 + 85.4678/212.37227 = 1 Compute mass percents using the mass fractions: Answer: | | | number of atoms | atom percent | mass percent I (iodine) | 1 | 50.0% | 126.90447/212.37227 × 100% = 59.76% Rb (rubidium) | 1 | 50.0% | 85.4678/212.37227 × 100% = 40.24%