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If 175.0g of nitrogen is reacted with 250.0g of hydrogen, what is the theoretical yield of the reaction? What is the excess reactant? What is the limiting reactant? Show your work.

Nitrogen gas is the limiting reactant

Hydrogen gas is the excess reactant

The theoretical yield is 425 g of ammonia

Explanation:

Equation of reaction: 3H2 + N2 ---> 2NH3

From the equation of reaction, 3 moles of hydrogen gas reacts with 1 mole of nitrogen to produce 2 moles of ammonia gas.

Molar mass of hydrogen gas = 2.0 g

Molar mass of nitrogen gas = 14.0 g

Molar mass of ammonia gas = 17.0 g

Number of moles of hydrogen gas in 250 g = 250/2 = 125 moles

Number of moles of nitrogen gas in 175 g = 175/14 = 12.5 moles

Mole ratio of Hydrogen to Oxygen = 125/12.5 = 10 : 1

Therefore, nitrogen gas is the limiting reactant.

Hydrogen gas is the excess reactant

14 g of nitrogen gas produces 17 × 2 g of ammonia = 34 g of ammonia

175 g will produce (34 × 175)/14 = 425 g of ammonia

Therefore the theoretical yield is 425 g of ammonia

water at room temperature is flowing through a pipe with pressure taps located 10 ft apart along one section of the pipe, which are connected to a mercury (s=13.6) manometer.

metric time was an attempt to create a standard unit of time based off of 10, but it never took off an is not included in the metric system (si)