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18 Nov 2019

Consider the following reaction: 2NH3 (g)+3Cl2 (g)---->N2 (g)+6HCl (g). 19.8 L of NH3 gas(measured at STP) is mixed with 26.8 Lof Cl2 (measured at a pressure of 722 torr and a temperature of35.0 degrees celsius). What mass (in grams) of HCl is possible withthis reaction?

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Lelia Lubowitz
Lelia LubowitzLv2
2 Aug 2019

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Question text

A mixture is prepared from 15.0 L of NH3 and 15.0 L of Cl2 measured at the same conditions and allowed to react according to the following equation:

2NH3(g) + 3Cl2(g) → N2(g) + 6HCl(g)

When the reaction is completed, what is the volume of Cl2 and HCl in the mixture?

(R= 0.082 atm. L/mol.K= 8.314 J/mol.K; 1 atm=76 cm Hg = 760 torr = 760 mmHg = 101325 Pa )

A mixture is prepared from 15.0 l of ammonia and 15.0 l chlorine measured at the same conditions these compounds react according to the following equation 2NH3+3Cl2---> N2+6HCl When the reaction is completed what is the volume of each gas (NH3, Cl2, N2 and HCl respectively)? Assume the final volumes are measured under identical conditions.

Hydrogen gas (a potential future fuel) can be formed by the reaction of methane with water according to the following equation: CH4(g)+H2O(g)→CO(g)+3H2(g) In a particular reaction, 25.0 L of methane gas (measured at a pressure of 736 torr and a temperature of 25 ∘C) is mixed with 22.2 L of water vapor (measured at a pressure of 700 torr and a temperature of 125 ∘C). The reaction produces 27.0 L of hydrogen gas measured at STP. What is the percent yield of the reaction?

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