Potassium metal reacts with water according to this balanced equation: 2 K(s)+2 H2O (1) KOH(aq)+H2(g) 2 K(s) + 2 H20 () 2 KOH(aq) + H2 (9) 516 a. If one mole of potassium reacts in this manner, how many moles of water are consumed? b. If one mole of potassium reacts in this manner, how many moles of H2 are produced? c. How many moles of potassium are required to produce 14.0 moles of H2? d. How many moles of KOH are produced if 3,014.2 moles of H20 are consumed?
The Correct Answer and Explanation is :
he reaction between potassium metal and water is represented by the balanced chemical equation:
[ 2\text{K}(s) + 2\text{H}_2\text{O}(l) \rightarrow 2\text{KOH}(aq) + \text{H}_2(g) ]
a. Moles of water consumed when 1 mole of potassium reacts:
ccording to the balanced equation, 2 moles of potassium (K) react with 2 moles of water (H₂O).his indicates a 1:1 molar ratio between potassium and water.herefore, if 1 mole of potassium reacts, it will consume 1 mole of water.
b. Moles of hydrogen gas produced when 1 mole of potassium reacts:
he balanced equation shows that 2 moles of potassium produce 1 mole of hydrogen gas (H₂), establishing a 2:1 molar ratio between potassium and hydrogen gas.hus, if 1 mole of potassium reacts, it will produce 0.5 moles of hydrogen gas.
c. Moles of potassium required to produce 14.0 moles of hydrogen gas:
rom the equation, 2 moles of potassium yield 1 mole of hydrogen gas, indicating a 2:1 ratio.o produce 14.0 moles of hydrogen gas, the required moles of potassium can be calculated as follows:
[ \text{Moles of K} = 14.0\ \text{moles H}_2 \times \frac{2\ \text{moles K}}{1\ \text{mole H}_2} = 28.0\ \text{moles K} ]
d. Moles of KOH produced if 3,014.2 moles of water are consumed:
he balanced equation indicates that 2 moles of water produce 2 moles of potassium hydroxide (KOH), showing a 1:1 molar ratio between water and KOH.herefore, if 3,014.2 moles of water are consumed, an equal number of moles of KOH will be produced:
[ \text{Moles of KOH} = 3,014.2\ \text{moles H}_2\text{O} \times \frac{2\ \text{moles KOH}}{2\ \text{moles H}_2\text{O}} = 3,014.2\ \text{moles KOH} ]
Explanation:
n chemical reactions, balanced equations provide the stoichiometric relationships between reactants and products.hese relationships are expressed as molar ratios, which allow for the calculation of the amounts of substances involved in the reaction.
n the reaction between potassium and water, the balanced equation:
[ 2\text{K}(s) + 2\text{H}_2\text{O}(l) \rightarrow 2\text{KOH}(aq) + \text{H}_2(g) ]
ndicates that 2 moles of potassium react with 2 moles of water to produce 2 moles of potassium hydroxide and 1 mole of hydrogen gas.hese coefficients represent the molar ratios of the substances involved.
or part (a), the 1:1 molar ratio between potassium and water means that 1 mole of potassium will consume 1 mole of water.
n part (b), the 2:1 molar ratio between potassium and hydrogen gas implies that 1 mole of potassium will produce 0.5 moles of hydrogen gas.
or part (c), to determine the moles of potassium needed to produce 14.0 moles of hydrogen gas, we use the inverse of the 2:1 molar ratio (i.e., 1:2), resulting in 28.0 moles of potassium required.
n part (d), the 1:1 molar ratio between water and potassium hydroxide indicates that consuming 3,014.2 moles of water will produce an equal number of moles of KOH.
nderstanding these stoichiometric relationships is crucial in chemistry, as they allow for the precise calculation of reactant consumption and product formation in chemical reactions.