Question 3 (1 point) N_(2)+3H_(2)arrow 2NH_(3) Which of the following statements is FALSE for the chemical equation given above in which nitrogen gas reacts with hydrogen gas to form ammonia gas assuming the reaction goes to completion? a One molecule of nitrogen requires three molecules of hydrogen for a complete reaction. The reaction of three moles of hydrogen gas will produce 17 g of ammonia. The reaction of 14g of nitrogen produces 17 g of ammonia. The reaction of one mole of H2 will produce 2/3 moles of NH3.

To determine which statement is FALSE, we need to analyze each statement based on the given chemical equation.<br /><br />The balanced chemical equation is:<br />$N_{2}+3H_{2}\rightarrow 2NH_{3}$<br /><br />a) One molecule of nitrogen requires three molecules of hydrogen for a complete reaction.<br />This statement is TRUE. According to the balanced equation, one molecule of nitrogen (N2) reacts with three molecules of hydrogen (H2) to produce two molecules of ammonia (NH3).<br /><br />b) The reaction of three moles of hydrogen gas will produce 17 g of ammonia.<br />To determine if this statement is TRUE or FALSE, we need to calculate the amount of ammonia produced from three moles of hydrogen gas.<br /><br />From the balanced equation, we know that 3 moles of hydrogen gas (H2) produce 2 moles of ammonia (NH3).<br /><br />The molar mass of ammonia (NH3) is 17 g/mol.<br /><br />Therefore, the amount of ammonia produced from three moles of hydrogen gas is:<br />2 moles of NH3 * 17 g/mol = 34 g of ammonia.<br /><br />Since the statement claims that the reaction of three moles of hydrogen gas will produce 17 g of ammonia, this statement is FALSE.<br /><br />c) The reaction of 14g of nitrogen produces 17 g of ammonia.<br />To determine if this statement is TRUE or FALSE, we need to calculate the amount of ammonia produced from 14g of nitrogen.<br /><br />The molar mass of nitrogen (N2) is 28 g/mol.<br /><br />Therefore, 14g of nitrogen is equivalent to 0.5 moles of nitrogen.<br /><br />From the balanced equation, we know that 1 mole of nitrogen (N2) produces 2 moles of ammonia (NH3).<br /><br />Therefore, 0.5 moles of nitrogen will produce 1 mole of ammonia.<br /><br />The molar mass of ammonia (NH3) is 17 g/mol.<br /><br />Therefore, 1 mole of ammonia is equivalent to 17 g of ammonia.<br /><br />Since the statement claims that the reaction of 14g of nitrogen produces 17 g of ammonia, this statement is TRUE.<br /><br />d) The reaction of one mole of H2 will produce $2/3$ moles of $NH3.$<br />To determine if this statement is TRUE or FALSE, we need to calculate the amount of ammonia produced from one mole of hydrogen gas.<br /><br />From the balanced equation, we know that 3 moles of hydrogen gas (H2) produce 2 moles of ammonia (NH3).<br /><br />Therefore, 1 mole of hydrogen gas will produce $2/3$ moles of ammonia.<br /><br />Since the statement claims that the reaction of one mole of H2 will produce $2/3$ moles of NH3, this statement is TRUE.<br /><br />Based on the analysis, the FALSE statement is:<br />b) The reaction of three moles of hydrogen gas will produce 17 g of ammonia.