a=(1)/(n)times 10.95,Mole5=5.465,Mults at STP in order to produce potassium nitride according to the following reaction? 6K+N_(2)arrow 2K_(3)N

To determine the number of moles of potassium (K) needed to produce potassium nitride (K3N) at standard temperature and pressure (STP), we need to use the balanced chemical equation provided:<br /><br />\[ 6K + N_2 \rightarrow 2K_3N \]<br /><br />First, let's find the molar ratio between potassium (K) and potassium nitride (K3N). According to the balanced equation, 6 moles of potassium (K) are required to produce 2 moles of potassium nitride (K3N).<br /><br />Next, we need to calculate the number of moles of potassium (K) using the given molar mass of potassium (K) and the given mass of potassium (K):<br /><br />\[ a = \frac{1}{n} \times 10.95 \]<br /><br />Given:<br />- Molar mass of potassium (K) = 39.10 g/mol<br />- Mass of potassium (K) = 10.95 g<br /><br />First, calculate the number of moles of potassium (K):<br /><br />\[ \text{Number of moles of K} = \frac{\text{Mass of K}}{\text{Molar mass of K}} = \frac{10.95 \text{ g}}{39.10 \text{ g/mol}} = 0.28 \text{ moles of K} \]<br /><br />Now, use the molar ratio to find the number of moles of potassium nitride (K3N) produced:<br /><br />\[ \text{Number of moles of K3N} = \frac{\text{Number of moles of K}}{6} = \frac{0.28 \text{ moles of K}}{6} = 0.047 \text{ moles of K3N} \]<br /><br />Therefore, 0.047 moles of potassium nitride (K3N) will be produced when 0.28 moles of potassium (K) react with nitrogen (N2) at STP.