A mixture of xenon and nitrogen gases, at a total pressure of 783 mm Hg, contains 9.00 grams of xenon and 6.65 grams of nitrogen. What is the partial pressure of each gas in the mixture? PXe = mm Hg PN2 = mm Hg

Partial pressure Xe = 175.4 mm Hg

Partial pressure N2 = 607.6 mm Hg

Explanation:

Step 1: Data given

Total pressure of the mixture = 783 mm Hg

Mass of Xenon = 9.00 grams

Atomic mass Xenon = 131.29 g/mol

Mass of N2 gas = 6.65 grams

Molar mass of 28.0 g/mol

Step 2: Calculate moles

Moles = mass / molar mass

Moles xenon = 9.00 grams / 131.29 g/mol

Moles Xenon = 0.06855 moles

Moles nitrogen gas = 6.65 grams / 28.0 g/mol

Moles nitrogen gas = 0.2375 moles

Step 3: Calculate mol ratio

Mol ratio = number of moles / total moles

Mol ratio xenon = 0.06855 / (0.06855+0.2375)

Mol ratio xenon = 0.224

Mol ratio nitrogen gas = 0.2375 / (0.06855+0.2375)

Mol ratio nitrogen gas = 0.776

Step 4: Calculate the partial pressures

Partial pressure = mol ratio * total pressure

Partial pressure Xe = 0.224 * 783 mmHg

Partial pressure Xe = 175.4 mm Hg

Partial pressure N2 = 0.776 * 783 mmHg

Partial pressure N2 = 607.6 mm Hg

175.4 + 607.6 = 783 mmHg

the equation that correctly represent the reaction for formation of ammonia is

n2+ 3h2 → 2nh3 (answer d)

1 mole of nitrogen gas (n2) react with 3 moles of hydrogen gas (h2) to form 2 moles of ammonia ( nh3). this is in a process known as haber process were iron is used as a catalyst and reaction take place that a higher temperature and pressure. the process is exothermic hence energy is released.

a galvanic cell( aka voltaic cell) and electrolytic cell

explanation:

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